use of light-supported oxidation processes towards microbiological and chemical contaminants
TRANSCRIPT
POUR L'OBTENTION DU GRADE DE DOCTEUR ÈS SCIENCES
acceptée sur proposition du jury:
Prof. C. Ludwig, président du juryProf. C. Pulgarin, Dr L. F. De Alencastro, directeurs de thèse
Prof. D. V. Vione, rapporteurDr P. Fernández-Ibáñez, rapporteuse
Prof. U. von Gunten, rapporteur
Use of light-supported oxidation processes towards microbiological and chemical contaminants elimination in
hospital wastewaters
THÈSE NO 7387 (2016)
ÉCOLE POLYTECHNIQUE FÉDÉRALE DE LAUSANNE
PRÉSENTÉE LE 2 DÉCEMBRE 2016
À LA FACULTÉ DES SCIENCES DE BASEGROUPE PULGARIN
PROGRAMME DOCTORAL EN GÉNIE CIVIL ET ENVIRONNEMENT
Suisse2016
PAR
Stefanos GIANNAKIS
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“Success consists of going from failure to failure without loss of enthusiasm.”
- Winston Churchill
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Acknowledgements With these words, I would like to thank everyone and everything that contributed to the successful
delivery of my Doctoral Thesis, and I would like to start with the Swiss National Foundation, for the funding
through the project “Treatment of the hospital wastewaters in Cote d’Ivoire and in Colombia by Advanced
Oxidation Processes”, during the last years.
First and foremost, this journey would have never even started if it was not for Prof. Cesar Pulgarin. I was
a young and foolish dreamer when I started working under his supervision, but with exemplary guidance,
tireless advice and time investment off his own well-being, I can safely say that I am now an old and foolish
dreamer, albeit with a purpose. I had the rare privilege to grow and learn with truly the best, and I hope
to never fail evolving, learning, getting better, as he would always want me to do. Thank you for breaking
all the stereotypes in the student-supervisor relation, and for being a true mentor in every aspect.
Also, I would like to thank my co-supervisor, Dr. Luiz Felippe de Alencastro, as his contribution was more
than crucial in the successful delivery of this Thesis. It takes a lot of patience and good will to work with
me, but he, along with Dominique Grandjean, surely went out of their way to help me complete my work.
My gratitude is also expressed to my Thesis examination Jury, Prof. Christian Ludwig, Dr. Pilar Fernández-
Ibáñez, Prof. Davide Vione and Prof. Urs von Gunten, for their comments, corrections, thoughts and the
very educative experience during the exam day.
All this work, would have never been completed without my trusted partners, my students, who tirelessly
and great zeal worked endless hours to complete their Master Projects: Miquel Pastor Gelabert, Simon
Schindelholz, David Muzard, Barbara Androulaki, Franco Alejandro Gamarra Vives, Margaux Voumard,
Idriss Hendaoui, Samuel Watts, Siting Liu and Christian Pinilla, and rest of the vibrant team members as
Ana Isabel Merino Gamo, Alba Camarasa, Marco Mangayayam. I sincerely wish you the best in your career
and your personal life. May you all find your path and look back at this time at EPFL with the same nostalgia
as I will do.
Special thanks to the rest of my co-authors for their constructive comments and contribution to
successfully publishing this work: Michael Bensimon, Jean-Marie Furbringer, Milica Jovic, Anna Carratala,
Natalia Gasilova, Hubert Girault, Anoys Magnet, Sana Thabet, Pascale Cotton, Maria Inmaculada Polo
Lopez, Jose Antonio Sanchez Perez and Pilar Valero.
A separate mention to the good friends I made through this work, my colleagues who were there seeing
me at my best and worst. Stefanos Papoutsakis and Sami Rtimi, thank you for your friendship and for the
countless times a short or extensive, scientific or not exchange took place among us, even if people around
us had to change a table during lunchtime. Sometimes a word is all people need. Laura Suarez and Paola
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Villegas, my more-than-officemates, for the moral and scientific support and for being more than my
neighbors, but a balance and a perspective in the difficult times during this period.
A special shout-out to Lambros Alexandrou, Kostas Karalazos and Christopher Zolotas. Sons of Berlusconi,
Macedonian Phalanx, €urogroup, many names of the same face: true friends, 2000 km away. The value
of knowing that you always have someone to turn to: Priceless. Special thanks to my Ballets, in Greece
and abroad: Alexandra (Young and Tall), Olga, Giota, Anastasia, Vanessa and Kiki. Andrew and Panagioti,
many years have gone by, but every time we meet it is High School all over again, thank you guys!
Saving the best for last, I want to thank and apologize to my family, my parents Fotis and Elektra and my
brothers George and Vangelis. Thank them for being there, at the other end of the phone line, the other
side of a Skype call, in any way they could, they supported my every step. They never put their own
happiness before mine, even when I had to expatriate, and for that I feel the need to apologize, for
depriving me from them.
Finally, I would like to thank the EPFL Language Services for the fortunate arrangements during the
German A1 Course placement, and for introducing me to the person who was fated to change me and my
life forever. My inspiration, my muse, my source of strength and happiness, my truly everything. Thank
you for every single time you were there for me, with your words and your care, even throughout the
most difficult of times… Sofia, my anticipation to spend the rest of my life with you cannot be described
by words…
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Abstract Hospital wastewaters have been long identified as carriers of chemical and microbiological pollutants.
Their amounts and risk levels have initiated numerous works on changing the existing practices of co-
treatment with municipal wastewaters and safe disposal in the environment. In this work, the issue of
hospital wastewater treatment is studied in two different contexts, in Switzerland and in developing
countries (Ivory Coast and Colombia). For this purpose, their treatment with municipal wastewater
effluents is recreated, simulating the developed countries’ context, while cheap and sustainable solutions
are proposed for the developing countries, to form a barrier between hospitals and receiving water
bodies. In both examples, the use of Advanced Oxidation Processes is implemented, focusing on UV-based
and solar-supported ones, in the respective target areas. A list of emerging contaminants and bacteria are
firstly studied to provide operational and engineering details on their removal by AOPs. Fundamental
mechanistic insights are provided as well on the degradation of the effluent wastewater organic matter.
The use of viruses and yeasts as potential model pathogens is also accounted for, treated by the photo-
Fenton process. Emphasis is given on the influence of the wastewater matrix parameters (organic matter,
pH, iron speciation etc.) and the exploration of the internal oxidative events, by the use of genomic and
proteomic analyses, respectively. Finally, two pharmaceutically active compound (PhAC) models of
hospital and/or industrial origin are studied in wastewater and urine, treated by all accounted AOPs, as a
proposed method to effectively control concentrated point-source pollution from industrial and hospital
wastewaters, respectively. Their elimination was modeled and the degradation pathway was elucidated
by the use of state-of-the-art analytical techniques (TOF-MS, Orbitrap). The use of light-supported AOPs
was proven to be effective in degrading the respective target and further insights were provided by each
application, which could facilitate their divulgation and potential application in the field.
Keywords: Advanced Oxidation Process, hospital wastewater, urine treatment, E. coli bacteria,
Saccharomyces cerevisiae yeast, MS2 Coliphage virus, emerging contaminants, UV/H2O2, photo-Fenton,
degradation pathway
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Résumé Les eaux usées hospitaliers ont longtemps été identifiés comme porteurs des polluants chimiques et
microbiologiques. Leurs montants et les niveaux de risque ont entrepris de nombreux travaux pour
modifier les pratiques existantes de co-traitement avec les eaux usées municipales et l'élimination sûre
dans l'environnement. Dans ce travail, le sujet du traitement des effluents d’eaux usées hospitaliers est
étudié dans deux contextes différents, en Suisse et dans des pays en développement (Côte d'Ivoire et la
Colombie). À cette fin, leur traitement avec les eaux usées municipales est recréé, avec la simulation du
contexte des pays développés, alors que des solutions économiques et durables sont proposées pour les
pays en développement, afin de former une barrière entre les hôpitaux et les eaux réceptrices. Dans les
deux exemples, l’utilisation des Procédés d'Oxydation Avancée (POA) est effectuée, en se concentrant
sur les procédés basés sur la lumière Ultraviolette et ceux solaires, respectivement dans les zones cibles.
Une liste de contaminants émergents et des bactéries sont premièrement étudiés pour fournir des détails
opérationnels et technologiques, concernant leur élimination par les POA. En outre, des aperçus sur les
mécanismes fondamentaux sont fournis sur la dégradation des matières organiques des effluents des
eaux usées. L’utilisation des virus et des levures comme des modèles de pathogènes potentiels ont été
également considérés et traités par le procédé photo-Fenton. L'accent est mis sur l'influence des
paramètres de la matrice des eaux usées (matière organique, pH, spéciation de fer, etc.) et l'exploration
des événements oxydatifs internes, par l'utilisation respective des analyses génomiques et protéomiques.
Enfin, deux modèles de composés pharmaceutiquement actifs d’origine hospitalière et/ou industrielle
sont étudiés dans les eaux usées et dans l’urine, et ils sont traités par tous les représentants POA, comme
une méthodologie proposée pour contrôler la pollution dense et ponctuelle par les eaux usées
respectivement industrielles et hospitalières. Leur élimination a été modélisée et la voie de dégradation
a été élucidée par l'utilisation de techniques d'analyse de pointe (TOF-MS, Orbitrap). L’utilisation de POA
basés sur la lumière a été démontrée efficace pour la dégradation de la cible respective et des conceptions
supplémentaires ont été fournies par chaque application, lesquelles pourraient faciliter leur divulgation
et implémentation potentielle dans le domaine.
Mots-clés : Procédés d'Oxydation Avancée, eaux usées hospitaliers, traitement d’urine, bactéries E. coli,
levure Saccharomyces cerevisiae, virus MS2 Coliphage, contaminants émergents, UV/H2O2, photo-Fenton,
voie de dégradation
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Contents
Acknowledgements ...................................................................................................................................... 5
Abstract ........................................................................................................................................................ 7
Résumé ......................................................................................................................................................... 9
Contents ..................................................................................................................................................... 11
List of Figures .............................................................................................................................................. 15
List of Tables ............................................................................................................................................... 18
Abbreviations list ........................................................................................................................................ 19
1. Chapter 1 – Introduction & state of the art ....................................................................................... 21
1.1. Basic characteristics of the targets ............................................................................................. 23
1.1.1. Categories/micropollutants classification .......................................................................... 24
1.1.2. Categories/microorganisms classification .......................................................................... 24
1.2. Problems related with microorganisms’ and micropollutants’ presence .................................. 27
1.3. Hospital WW and pollutants ...................................................................................................... 29
1.3.1. HWW and MPs ................................................................................................................... 29
1.3.2. HWW and MOs ................................................................................................................... 31
1.4. Occurrence, treatment and fate of MPs in MWWTPs ............................................................... 32
1.4.1. MP Occurrence in WWTPs ................................................................................................. 32
1.4.2. MP evolution path in WWTPs ............................................................................................ 32
1.4.3. Factors affecting MP removal in WWTPs ........................................................................... 33
1.5. AOPs action in chemical and microbiological pollutants’ degradation ...................................... 34
1.5.1. UV-based processes (UV, UV/H2O2) ................................................................................... 36
1.5.2. Fenton-related reactions (Fenton, photo-Fenton, solar light) ........................................... 41
1.6. Problem identification and contextualization: Micropollutants and microorganisms in developed and developing countries ..................................................................................................... 44
1.7. AOPs vs. Micropollutants and Microorganisms: current status ................................................. 46
1.8. Thesis aims and objectives ......................................................................................................... 48
2. Chapter 2: Effect of advanced oxidation processes on the micropollutants and the effluent organic matter contained in municipal wastewater previously treated by three different secondary methods .. 53
2.1. Introduction ................................................................................................................................ 54
2.2. Materials and Methods .............................................................................................................. 56
2.2.1. Sampling campaign ............................................................................................................. 56
2.2.2. Chemicals and reagents...................................................................................................... 56
2.2.3. Employed reactors .............................................................................................................. 57
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2.2.4. Advanced Oxidation Processes specifics ............................................................................ 57
2.2.5. Physicochemical parameters .............................................................................................. 58
2.2.6. Analytical methods ............................................................................................................. 58
2.2.7. Secondary treatment systems specifications ..................................................................... 59
2.3. Results ........................................................................................................................................ 59
2.3.1. Initial conditions ................................................................................................................. 59
2.3.2. Efficacy of the various advanced oxidation processes ....................................................... 62
2.3.3. Degradation kinetics evaluation for the 6 different pollutants ......................................... 67
2.3.4. Evolution of the Average Oxidation State during the 5 different treatment processes .... 68
2.4. Discussion ................................................................................................................................... 71
2.4.1. Degradation of micropollutants in wastewater: characteristics, influence and role of the Effluent Organic Matter ..................................................................................................................... 71
2.4.2. Pathways of MP degradation in secondary effluent .......................................................... 72
2.5. Conclusions ................................................................................................................................. 76
3. Chapter 3 - Micropollutant degradation, bacterial inactivation and regrowth risk in wastewater effluents: influence of the secondary (pre)treatment on the efficiency of Advanced Oxidation Processes 79
3.1. Introduction ................................................................................................................................ 80
3.2. Materials and Methods .............................................................................................................. 81
3.2.1. Collection of wastewater samples and treatment plant specifications ............................. 81
3.2.2. Employed chemicals and reagents ..................................................................................... 82
3.2.3. Experimental set-up: reactors and apparatus .................................................................... 82
3.2.4. Application of AOPs: details and specifications ................................................................. 82
3.2.5. Analytical methods, physicochemical and microbiological parameters ............................ 83
3.3. Results ........................................................................................................................................ 84
3.3.1. Micropollutant elimination in the selected wastewater effluents .................................... 84
3.3.2. Microorganism elimination in the different wastewater effluents, per AOP: inactivation and post-treatment regrowth ............................................................................................................ 86
3.4. Discussion ................................................................................................................................... 91
3.4.1. The major threat and treatment focus: micropollutants or microorganisms? .................. 91
3.4.2. Common events and dissimilarities in the treatment of different targets in secondary effluents 93
3.5. Conclusions ................................................................................................................................. 97
4. Chapter 4 - Effect of Fe(II)/Fe(III) species, pH, irradiance and bacterial competition on viral inactivation in wastewater by the photo-Fenton process: Kinetic modeling and mechanistic interpretation. .......................................................................................................................................... 101
4.1. Introduction .............................................................................................................................. 102
4.2. Materials and methods ............................................................................................................ 103
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4.2.1. Chemicals and reagents.................................................................................................... 103
4.2.2. Sunlight source and reactors ............................................................................................ 105
4.2.3. Microorganisms and quantification methods .................................................................. 105
4.2.4. Inactivation experiments .................................................................................................. 106
4.2.5. Data treatment and analysis ............................................................................................ 106
4.3. Results and Discussion ............................................................................................................. 107
4.3.1. Isolated effect of the photo-Fenton constituents ............................................................ 107
4.3.2. Parametrization of MS2 inactivation by the photo-Fenton process in wastewater ........ 109
4.3.3. Effect of bacterial competition on MS2 inactivation in wastewater ................................ 113
4.3.4. Iron cations solubility in wastewater ............................................................................... 115
4.3.5. MS2 inactivation modeling ............................................................................................... 116
4.3.6. Integrated proposal for the inactivation mechanism of viruses in wastewater .............. 118
4.4. Conclusions ............................................................................................................................... 120
5. Chapter 5 - Castles fall from inside: Evidence for dominant internal photo-catalytic mechanisms during treatment of Saccharomyces cerevisiae by photo-Fenton at near-neutral pH ............................ 121
5.1. Introduction .............................................................................................................................. 122
5.2. Materials and Methods ............................................................................................................ 124
5.2.1. Chemicals .......................................................................................................................... 124
5.2.2. Fe–citrate complex and Goethite preparation ................................................................. 124
5.2.3. Yeast strains and growth media ....................................................................................... 124
5.2.4. Photo-inactivation experiments ....................................................................................... 125
5.2.5. Cultivability assays ............................................................................................................ 125
5.2.6. Analytical methods ........................................................................................................... 126
5.2.7. Biochemical methods ....................................................................................................... 126
5.2.8. Experimental Planning ...................................................................................................... 127
5.3. Results and Discussion ............................................................................................................. 127
5.3.1. Preliminary assays in simulated wastewater ................................................................... 127
5.3.2. Cultivability assays – Efficiency of treatment ................................................................... 128
5.3.3. Flow cytometry results – Localization of damage ............................................................ 134
5.3.4. Identification of targets – Nuclear DNA, cell wall and cytoplasmic protein damage ....... 141
5.3.5. Holistic proposal for the inactivation mechanism of S. cerevisiae ................................... 144
5.4. Conclusions ............................................................................................................................... 146
6. Chapter 6 - Iohexol degradation in wastewater and urine by UV-based Advanced Oxidation Processes (AOPs): Process modeling and by-products identification. ..................................................... 151
6.1. Introduction .............................................................................................................................. 152
6.2. Materials and Methods ............................................................................................................ 153
6.2.1. Chemicals and Reagents ................................................................................................... 153
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6.2.2. Reactors and experimental apparatus ............................................................................. 154
6.2.3. Analytical methods ........................................................................................................... 154
6.2.4. Water matrices and treatment conditions ....................................................................... 156
6.2.5. Statistics, modeling and data treatment .......................................................................... 157
6.3. Results and Discussion ............................................................................................................. 158
6.3.1. Engineering approach – investigation on the operational parameters ........................... 158
6.3.2. Statistical approach – modeling and mathematical optimization of the treatment ........ 163
6.3.3. Analytical approach – Global measurements (COD, TOC, and UV-vis absorbance) combined with specific HPLC and MS analysis ................................................................................. 170
6.4. Conclusions ............................................................................................................................... 175
7. Chapter 7 - Solar photo-Fenton and UV/H2O2 processes against the antidepressant Venlafaxine in urban wastewaters and human urine. Intermediates formation and biodegradability assessment. ..... 177
7.1. Introduction .............................................................................................................................. 178
7.2. Materials and methods ............................................................................................................ 179
7.2.1. Chemicals and reagents.................................................................................................... 179
7.2.2. Water, wastewater and urine matrices............................................................................ 180
7.2.3. Light sources and corresponding reactors-experimental apparatus ............................... 181
7.2.4. Analytical methods ........................................................................................................... 181
7.3. Results and Discussion ............................................................................................................. 182
7.3.1. UV-based AOPs degradation of Venlafaxine .................................................................... 182
7.3.2. Fenton-related AOPs degradation of Venlafaxine ........................................................... 187
7.3.3. Venlafaxine degradation experiments in wastewater and urine ..................................... 192
7.3.4. Elucidation of the AOP-driven degradation pathway and inherent biodegradability properties of Venlafaxine ................................................................................................................. 197
7.4. Conclusions ............................................................................................................................... 200
8. Chapter 8 - General conclusions, perspectives and future work ..................................................... 201
9. References ........................................................................................................................................ 205
Appendix A: Supplementary material of Chapter 2 ................................................................................. 222
Appendix B: Supplementary material of Chapter 3 ................................................................................. 230
Appendix C: Supplementary material of Chapter 4 ................................................................................. 235
Appendix D: Supplementary material of Chapter 5 ................................................................................. 237
Appendix E: Supplementary material of Chapter 6 .................................................................................. 240
Appendix F: Supplementary material of Chapter 7 .................................................................................. 261
Curriculum Vitae of the Candidate ........................................................................................................... 273
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List of Figures Figure 1.1 – E. coli structure (adaptation: Source: http://www.bevpease.force9.co.uk/p.Dawn-of-Life_files/image004.gif) ............................................................................................................................ 25 Figure 1.2 – Infection mechanism of the bacteriophage MS2 (Source file: http://faculty.washington.edu/jclara/301/images/ssRNA.jpg). Inset: MS2 structure (Credits: Stephan Spencer, http://www.virology.wisc.edu/virusworld/imgency/ms2MS22.jpeg) .................................... 26 Figure 1.3 – Saccharomyces cerevisiae (yeast model) structure (Thabet et al. 2013)............................. 27 Figure 1.4 – Bioaccumulation of MPs (http://toxics.usgs.gov/regional). ............................................... 29 Figure 1.5 – Contribution of HWW in pollutants integration to the environment (http://www.frontiersin.org/files). .......................................................................................................... 30 Figure 1.6 – Categorization of Advanced Oxidation Process (Poyatos et al. 2010)................................. 36 Figure 1.7 – Light absorption of Fe3+ species at normal solar irradiance (I) on the Earth’s surface ....... 41 Figure 1.8 – Routes of pharmaceutical contamination of the aquatic environment (Ikehata et al. 2006). .................................................................................................................................................................... 45 Figure 1.9 – Thesis graphical representation and organization of aims and objectives. ........................ 48 Figure 2.1 – Simplified overview of the Vidy WWTP and the sampling points used in the study. ......... 56 Figure 2.2 – UV treatment results. a) % degradation vs. time b) % COD & TOC reduction vs. time. ...... 62 Figure 2.3 – UV/H2O2 treatment results. a) % degradation vs. time. b) % COD & TOC reduction vs. time. .................................................................................................................................................................... 63 Figure 2.4 – Solar exposure results. a) % degradation vs. time b) % COD & TOC reduction vs. time. .... 64 Figure 2.5 – Fenton process results. a) % degradation vs. time. b) % COD & TOC reduction vs. time. ... 65 Figure 2.6 – photo-Fenton process results. a) % degradation vs. time. b) % COD & TOC reduction vs. time. ........................................................................................................................................................... 67 Figure 2.7 – Overall mechanistic interpretation for the action of UVC and solar light within the effluent wastewater (adapted from (De la Cruz et al. 2012)). ............................................................................... 76 Figure 3.1 – Schematic representation of the WWTP of Vidy, Lausanne (VD, Switzerland) and the sampling points for this research. ............................................................................................................. 81 Figure 3.2 – Micropollutants’ degradation by AOPs after secondary treatment. a) UV and UV/H2O2 processes. b) Fenton, solar and photo-Fenton process. AS: blue trace, MBBR: red trace, CF: green trace. Continuous lines and colored symbols show the measured evolution of the experiment, while the dashed lines and open symbols indicate the projection of the experiment according to the measured first order degradation rate constant. ...................................................................................................... 85 Figure 3.3 – UV-based disinfection and respective regrowth after 24 h. A) UVC irradiation alone. B) UV/H2O2 process (20 ppm initial H2O2 addition). The shaded part and the dashed lines symbolize the dark storage and regrowth after treatment, for 24 h. ............................................................................. 87 Figure 3.4 – Fenton-related disinfection and respective regrowth after 24 h. A) Fenton process (2:10 ppm initial Fe2+/H2O2 addition). B) bare solar light. C) photo-Fenton process (2:10 10 ppm initial Fe2+/H2O2 addition). The shaded part and the dashed lines symbolize the dark storage and regrowth4 after treatment, for 24 h. .......................................................................................................................... 89 Figure 3.5 – UV-based disinfection and decontamination. A) UVC irradiation alone. B) UVC/H2O2 process. The lines indicate the microorganism inactivation, while the bars the micropollutant degradation (%). The circles indicate the regrowth suppression points with the respective colors indicating the secondary treatment method, while the horizontal lines indicate the minimal micropollutant (brown line) and microorganism removal (orange line). ................................................ 91 Figure 3.6 – Fenton-related disinfection and respective regrowth after 24 h. A) Fenton process. B) Bare solar light. C) photo-Fenton process. The lines indicate the microorganism inactivation, while the bars the micropollutant degradation (%). The circles indicate the regrowth suppression points with the
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respective colors indicating the secondary treatment method, while the horizontal lines indicate the minimal micropollutant (brown line) and microorganism removal (orange line). ................................. 93 Figure 4.1 – Solar/H2O2 and Solar/Fe control experiments. a) Isolated effect of the operating H2O2 levels of this work. b) Addition of 0.5 or 1 mg/L Fe(II) or Fe(III) salts. DL: detection limit. ................... 108 Figure 4.2 – Effect of solar irradiance on the evolution of the photo-Fenton reaction. A) Fe(II) as starting iron species. B) Fe(III) as starting iron species. A notable difference exists in the kinetic families of Fe(II) or Fe(III). DL: detection limit. ....................................................................................... 109 Figure 4.3 – Effect of the Fe:H2O2 ratio on the evolution of the photo-Fenton process. a) Fe(II) as starting species. b) Fe(III) as starting species. ........................................................................................ 110 Figure 4.4 – Effect of the starting pH on the evolution of the photo-Fenton process. a) Fe(II) as starting species. b) Fe(III) as starting species. ...................................................................................................... 113 Figure 4.5 – Bacterial competition tests: Inactivation of MS2 and E. coli by the photo-Fenton process. a) Bacterial inactivation with increasing Fe:H2O2 ratios, in absence or presence of MS2. b) E. coli inactivation in presence of MS2 and MS2 inactivation in presence or absence of the bacterial host (Fe:H2O2 ratio 1:1). Higher Fenton reagents addition than 1:1 resulted in <2-min inactivation. ......... 114 Figure 4.6 – Iron evolution during (dark) Fenton or photo-Fenton process followed by ICP-MS analysis. A) Fe(II) starting salts. B) Fe(III) starting salts. The dashed lines indicate the dark Fenton experiments, closed trace symbols indicate dissolved iron and open trace symbols the total iron. .......................... 116 Figure 4.7 – Proposed MS2 inactivation pathway by the photo-Fenton process in wastewater at near-neutral pH. The events 1-6 are further analyzed in the text. ................................................................. 119 Figure 5.1 – Overview of the photo-Fenton tests in simulated wastewater. ........................................ 128 Figure 5.2 – Overview of the photocatalytic inactivation tests and their respective controls. a) The plots describe the cultivability evolution over time. b) Comparison between pH 5.5 and 7.5 for the FeSO4-assisted photo-Fenton system. c) Comparison between pH 6.0 and 7.5 for the iron citrate-assisted photo-Fenton system. Standard deviation < 5%. ..................................................................... 129 Figure 5.3 – Control tests and an indicative presentation of the flow cytometry results evolution, during photo-Fenton reaction, at pH = 5.5. ............................................................................................ 135 Figure 5.4 – Flow cytometry results. Control tests: a) Simulated solar light only. b) hv/H2O2 system. FeSO4–assisted photo–Fenton processes: c) pH = 5.5. d) pH = 7.5. Fe-cit–assisted photo–Fenton processes: e) pH =6.0. f) pH = 7.5. Standard deviation < 5%. ................................................................. 140 Figure 5.5 – Nuclear DNA damage in the four different systems. Comparison of the pH effect in FeSO4-assisted photo-Fenton systems. .............................................................................................................. 141 Figure 5.6 – Cell wall (a) and cytoplasmic proteins damage (b) in the four different systems. (i-ii): Comparison of the pH effect in FeSO4-assisted photo-Fenton systems. ............................................... 142 Figure 5.7 – Mechanistic proposition of the pathways towards yeast cell inactivation. a) (direct) Simulated solar light. b) (Indirect) hv/H2O2. c) FeSO4–assisted photo–Fenton process. d) Fe-cit–assisted photo–Fenton process. ............................................................................................................................ 145 Figure 6.1 – UV photolysis and UV/H2O2 experiments in Mili-Q water. Note that the results in the 10-1000 mg/L range are plotted in double-logarithmic scale and axis breaks for clarity purposes only. 159 Figure 6.2 – Effect of pH, dilution and Iohexol, H2O2 and Fe2+ amounts. Dotted lines represent the undiluted matrices, continuous lines indicate the x10 times dilution experiments, and for Figure 3b, the x100 times diluted UR experiments are signified with long dashed lines. Note the mixed axes scales. .................................................................................................................................................................. 161 Figure 6.3 – Real wastewater and urine experiments: UV/H2O2/Fe2+ process. A) Iohexol in untreated or biologically treated WW, and B) diluted/undiluted urine, H2O2 added in 0, 10 or 50 ppm, iron was added in 0, 1, or 5 ppm, and changing of the initial pH value (3, 5 or near-neutral). The two main groups of Figure 3a data are separated by continuous (10 ppm Iohexol) or dashed lines (100 ppm). The
17
respective groups in Figure 3b are designated by color. The vertical bars show the variation in efficiency when pH was changed. Note the mixed axes scales. ............................................................. 162 Figure 6.4 – HPLC peak areas evolution during Iohexol degradation by the UV photolytic and photocatalytic process. A) UV only, B) 10 ppm H2O2, C) 100 ppm H2O2, D) 1000 ppm H2O2. 100 ppm of Iohexol was chosen as initial spiking. ..................................................................................................... 171 Figure 6.5 – Iohexol elimination by the UV-based AOPs. Iohexol degradation was followed by HPLC (blue trace), COD (red trace) and TOC decrease (green trace) during the following treatment methods: UV photolysis (trace: ), UV/H2O2 process (50 ppm H2O2, trace: ), and UV/H2O2/Fe2+ process (5 ppm Fe2+, 50 ppm H2O2, trace: ). H2O2 reduction: brown traces. A system employing 35-W UV-C lamps (instead of the 11-W ones of the previous parts, but otherwise identical) was used here. 100 ppm Iohexol was chosen as initial spiking. ..................................................................................................... 172 Figure 6.6 – Overall mechanistic degradation pathway of Iohexol treated by UV-based AOPs. Products common for all three treatments were marked with P, UV marked with A, for UV/H2O2 with B and for UV/H2O2/Fe2+ with C. Products common for A and C treatment were marked as AC, and accordingly, products common for B and C treatment were marked as BC. .............................................................. 174 Figure 7.1 – Summary of the UV-C photolysis experiments. a) UV-induced degradation of Venlafaxine followed by HPLC, COD removal and TOC reduction during UV photolysis. b) Evolution of the COD/TOC ratio. ......................................................................................................................................................... 183 Figure 7.2 – UV/H2O2 Advanced Oxidation of Venlafaxine: degradation and process optimization. a) Degradation of VFA by UV/H2O2 with addition of 5-50 mg/L H2O2. b) Evolution of COD/TOC ratio (for 50 mg/L initial H2O2 addition). c) Consumption of H2O2 (black axis and traces) and changes in the t90% (blue axis and traces) as a function of initial H2O2 amounts. ................................................................. 185 Figure 7.3 – Treatment of Venlafaxine by the Fenton process in the dark. a) Evolution of the t90% with increasing Fe|H2O2 ratio and pH. b) COD/TOC ratio modification by the Fenton process at various Fe|H2O2 ratios (pH=3) and increasing pH for a 20|50 (mg/L|mg/L) ratio. ........................................... 188 Figure 7.4 – Absorbance spectra during the 24-h Fenton treatment of Venlafaxine, for various Fe|H2O2 ratios (panels a-d) and pH levels (panels i-iii). Fe|H2O2 ratios: a) 5|10, pH=3. b) 5|50, pH=3. c) 12.5|30, pH=3. d) 20|50, pH=3. pH levels: i) 20|50, pH=3. ii) 20|50, pH=5. iii) 20|50, pH=7. ............................. 190 Figure 7.5 – Treatment of Venlafaxine by the photo-Fenton process (irradiance: 900 W/m2). a) Evolution of the t90% with increasing Fe|H2O2 ratio and pH. b) COD/TOC ratio evolution by the solar photo-Fenton process at various Fe|H2O2 ratios (pH=3) and increasing pH for a 20|50 ratio. ............ 191 Figure 7.6 – Absorbance spectra during the 3-h photo-Fenton treatment of Venlafaxine, for various Fe|H2O2 ratios (panels a-d) and pH levels (panels i-iii). Fe|H2O2 ratios: a) 5|10, pH=3. b) 5|50, pH=3. c) 12.5|30, pH=3. d) 20|50, pH=3. pH levels: i) 20|50, pH=3. ii) 20|50, pH=5. iii) 20|50, pH=7. .............. 192 Figure 7.7 – Treatment of Venlafaxine by AOPs in urban WW effluents. The experimental conditions are marked in the corresponding graphs. a) VFA degradation by UV-based AOPs in AS, MBBR and CF effluents. b) VFA degradation by the Fenton-related processes in AS, MBBR and CF effluents. .......... 194 Figure 7.8 – Treatment of Venlafaxine by UV-based methods in human urine. a) VFA degradation by UV-based AOPs (0, 50 or 100 mg/L H2O2 and 0/100% or 10%-90% urine/water ratio. b) COD reduction and DOC (0.45μm filtration) removal in the same conditions. .............................................................. 196 Figure 7.9 – Combined Venlafaxine degradation pathway through the application of the treatment methods analyzed. ................................................................................................................................... 198 Figure 7.10 – Zahn-Wellens inherent biodegradability test of Venlafaxine and treated solutions in MQ. a) ZW test after treatment of 50% of the initial VFA solution. b) ZW test after treatment of 100% of the initial VFA solution. Note that results are normalized towards the initial DOC to enable comparison. .................................................................................................................................................................. 199
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List of Tables Table 1.1 – Examples of fecal-related viruses contained in the feces and their associated diseases (Carter 2005, Glass et al. 2009, Mayer et al. 2008, Okoh et al. 2010, Rodriguez et al. 2014) ................. 26 Table 1.2 – Comparison between indicative UWW and HWW effluents characteristics (Carraro et al. 2016, El-Ogri et al. 2016, Verlicchi et al. 2010) and references therein). ................................................ 31 Table 1.3 – Classification of commonly studied micropollutants (based on removal efficiency). .......... 33 Table 2.1 – Evolution of indicator pollutants in the Swiss legislation. .................................................... 55 Table 2.2 – Summary of the advanced treatment methods applied. ...................................................... 58 Table 2.3 – Initial physicochemical characteristics of the effluents of the different secondary treatment units. ........................................................................................................................................................... 60 Table 2.4 – Initial micropollutant concentration and limit of quantification (LOQ) for micropollutants in the effluent of the different secondary treatment units. ......................................................................... 61 Table 2.5 – Degradation kinetics of the 6 different pollutants during treatment in the different effluents and treatment methods. ............................................................................................................ 68 Table 2.6 – Evolution of the Average Oxidation State (AOS) during treatment by the various methods in the different effluents. ........................................................................................................................... 69 Table 2.7 – AOS percentile change and correlation with % of degradation. ........................................... 70 Table 3.1 – Basic physicochemical and optical characteristics of the wastewater used in this study (own measurements and (aMargot et al. 2013, bMargot et al. 2011)). ................................................... 83 Table 3.2 – Photochemical characteristics of the various effluents ......................................................... 95 Table 4.1 – Composition of synthetic secondary wastewater (Muthukumaran et al. 2011). ............... 104 Table 4.2 – Effect of photo-Fenton treatment [Fe(II)] on MS2 inactivation. ......................................... 117 Table 4.3 – Effect of photo-Fenton treatment [Fe(III)] on MS2 inactivation. ........................................ 117 Table 5.1 - Timeline of the inflicted damage in the corresponding targets of the different iron-assisted systems ..................................................................................................................................................... 144 Table 6.1 – Synthetic matrices composition. .......................................................................................... 153 Table 6.2 – Physicochemical characteristics of the real wastewater matrices (Giannakis et al. 2015c, Margot et al. 2013, Margot et al. 2011). ................................................................................................ 156 Table 6.3 – Physicochemical characteristics of real urine matrices (own measurements and (Beach 1971)). ...................................................................................................................................................... 156 Table 6.4 – t90% evolution (min) in varied Iohexol (10-1000 ppm) and H2O2 (0-1000) levels ................. 159 Table 6.5 – Wastewater models with S and R2 values. .......................................................................... 165 Table 6.6 – Urine models with S and R2 values ....................................................................................... 167 Table 6.7 – Optimal regions for treatment Iohexol through optimization by the desirability function. .................................................................................................................................................................. 169 Table 7.1 – Venlafaxine characteristics and physicochemical properties (USNLM 2016b). .................. 179 Table 7.2 – Composition of the synthetic matrices used in this study. .................................................. 180 Table 7.3 – Measured pseudo-first order degradation kinetics of Venlafaxine per AOP and matrix. . 185 Table 7.4 – Occurrence and fate of Venlafaxine in urban WW effluents. ............................................. 193
19
Abbreviations list AOPs - Advanced Oxidation Processes
AOS - Average Oxidation State
AS - Activated Sludge
BCF – Bio-concentration Factor
CAT - Catalase
CBS - Carbonate Buffer Solution
CDOM - Chromophoric Dissolved Organic Matter
CF - Coagulation-Flocculation
CFDA - 5-carboxyfluorescein di-acetate
CFU - Colony Forming Units
COD - Chemical Oxygen Demand
CPDs - Cyclobutane Pyrimidine Dimers
D - (Composite) Desirability
DBP - Disinfection By-Product
DL - Detection Limit
DNA - Deoxyribonucleic Acid
DOC - Dissolved Organic Carbon
DOM - Dissolved Organic Matter
EfOM - Effluent Organic Matter
EPS - Extracellular Polymeric Substances
Fe/S - Iron-Sulfur
FOEN - Federal Office for the Environment
HRT - Hydraulic Retention Time
HWW - Hospital Wastewater
hv - Light
ICP-MS - Inductively coupled plasma mass spectrometry
LMCT - Ligand-to-Metal Charge Transfer
MBBR - Moving Bed Bioreactor
MO - Microorganism
MP - Micropollutant
MQ - MiliQ water
MS - Mass Spectrometry
MW - Molecular Weight
MWW - Municipal Wastewater
NOM - Natural Organic Matter
OxOM - Oxidizable Organic Matter
PFU - Plaque Forming Units
PhOM - Photo-sensitizable Organic Matter
pI - Isoelectric point
PI - Propidium Iodide
POM - Particulate Organic Matter
PP - PhotoProduct
ROS - Reactive Oxygen Species
RU - Real Urine
S - Synergy
SDS-PAGE - Polyacrylamide gel electrophoresis
SMP - Soluble Microbial Products
SOD - Superoxide Dismutase
SODIS - Solar Disinfection
SPE - Solid Phase Extraction
SRT - Sludge Retention Time
SS - Suspended Solids
SSNRIs - selective serotonin and norepinephrine reuptake inhibitors
SUR - Synthetic Urine
SUVA - Specific UV Absorbance
SWW - Synthetic Wastewater
T - Transmittance
TDS - Total Dissolved Solids
TKN - Total Kjeldahl Nitrogen
TOC - Total Organic Carbon
20
TSS - Total Suspended Solids
UWW - Urban Wastewater
UV - Ultraviolet
VFA - Venlafaxine
WW - Wastewater
WWTP - Wastewater Treatment Plant
ZW - Zahn-Wellens
21
1. Chapter 1 – Introduction & state of the art
23
Introduction & state of the art
Currently, one of the environmental concerns in global scale is the presence and accumulation of
micropollutants in the natural environment. These substances are comprising an increasing list of
anthropogenic (or not) contaminants, which include among others, pharmaceuticals, personal care
products, steroid hormones, industrial chemicals, pesticides and many other emerging compounds (Luo
et al. 2014). The majority of these substances are designed to be biologically active, and therefore, their
occurrence can affect the receiving environment, even at low concentrations (Santos et al. 2010); this
feature characterized them as “micropollutants”. This exact characteristic, combined with the diversity of
the chemical pollutants, re-instate this topic as high priority and challenging for the treatment facilities.
Wastewater treatment plants have been built, transformed and updated through the years to effectively
prevent solids, organic and inorganic compounds (carbon, nitrogen, phosphorus etc.) and more, that
enter the environment. The challenge posed by the pollutants is a matter that the majority of the WWTPs
are not equipped to handle. The micropollutants are (in a high percentage) invulnerable to biological
treatment; the transfer from source to the environment is therefore facilitated, leading to further
accumulation in the environment. As it will be analyzed later on, their presence has been associated with
minor and major health risks, toxicity and more (Fent et al. 2006, Luo et al. 2014).
The risk of microorganisms’ presence in natural water bodies is more explored compared to
micropollutants. Water scarcity has led to reuse concepts and many countries worldwide have included
legislation concerning the removal thresholds according to the subsequent water reuse (e.g. Italy, (Liberti
et al. 2003)). However, chlorination is still the most widespread technique, with its inherent problems,
such as DBPs (trihalomethanes THM) formation, and where funds are available UV has been applied. In
order to better suggest treatment goals and methods, the present thesis will address the use of Advanced
Oxidation Processes (AOPs) as a greener and sustainable disinfection and decontamination method of
hospital and urban wastewater. The solutions will be studied and provided according to the context of
application (developed or developing country) and the target of reference (microorganisms or
micropollutants). Finally, mechanistic insights will be given to further strengthen the knowledge base and
the know-how on AOPs used in wastewater treatment.
1.1. Basic characteristics of the targets
Before analyzing in detail the problems related with the presence of micropollutants and microorganisms,
the basic categories are hereby mentioned.
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1.1.1. Categories/micropollutants classification
Concerning the categories of chemical pollutants, among the list of contaminants of emerging concern,
we find:
Pharmaceuticals: drug-related compounds.
Personal care products: Fragrances, disinfectants, UV filters, and insect repellents.
Steroid hormones: Estrogenic or androgenic effects
Surfactants: Detergents, wetting agents, emulsifiers, foaming agents, and dispersants.
Industrial chemicals: Plasticizers, flame retardants.
Biocides: Pesticides - insecticides, herbicides and fungicides.
The present work focuses, but is not limited, on the pharmaceutical pollutants, also known as
Pharmaceutically Active Compounds (PhACs). These are considered special micropollutants (Fatta-
Kassinos et al. 2011), due to the complexity of their structure, the polymorphism and the variation due to
the precedent metabolism in the human body (Cunningham 2004).
The PhACs have been long identified as harmful agents against the occurring flora and fauna in the natural
environment. Reports (Halling-Sørensen et al. 1998, Kümmerer 2001, Kümmerer 2004, Sumpter 1998)
link their presence with a wide array of effects on microorganisms, plants, fish, and possibly to humans.
The classes of PhACs that potentially pose a threat are (Ikehata et al. 2006):
Cytostatic agents, immunosuppressive drug and genotoxic drugs: this class has direct impact
(cytotoxic, carcinogenic, embryotoxic, etc.) on the receptors
Antibiotics: Their accumulation can lead to antibiotic-resistant bacteria
Hormones: Their action is profound in low levels, often leading to endocrine disruption and
feminization of male species.
Iodinated contrast media (ICM): Non-biodegradable, and therefore highly persistent in the
environment
Metals: Drugs that contain heavy metals pose toxicity risks.
Other micropollutants that are investigated in this thesis are pesticides, corrosion inhibitors,
antidepressants and beta-blockers, found in urban effluents.
1.1.2. Categories/microorganisms classification
Concerning the representatives of microbiological risk, the main categories of microorganisms in
wastewater are represented by:
Bacteria: Fecal indicator bacteria, wild type pathogenic strains etc.
Viruses: e.g. Coliphages, adenoviruses, rotaviruses etc.
25
Yeasts: e.g. Candida albicans
Protozoa: e.g. Cryptosporidium parvum (cysts and oocysts)
Parasites: e.g. Helminth eggs
Prions
This thesis will deal only with the first three categories of microorganisms, which represent the largest
fraction of pathogens in wastewater. Therefore, some general and structural details will be provided.
The bacterial presence is associated with either enteric or non-enteric source. E. coli has been for over a
century considered an indicator of enteric origin bacteria, and has been used as such ever since, due to
its relative ease to cultivate and maintain in a laboratory, its adequate survival and proper representation
of various water matrices (Edberg et al. 2000, Lin and Ganesh 2013). Also, the wild types have been
associated with various diseases themselves (Nataro and Kaper 1998) and the use of the lab-strain allows
safe recreation of the desired conditions.
Figure 1.1 – E. coli structure (adaptation: Source: http://www.bevpease.force9.co.uk/p.Dawn-of-
Life_files/image004.gif)
Viruses on the other hand differ significantly in structure complexity and morphology. They are also single-
cell microorganisms, but are composed simply by a capsid and the genome. As an obligate parasite, they
require the presence of a host in order to replicate and infect their target (Figure 1.2). Their presence in
wastewaters has been verified and some indicative ones (and their effect) are presented in Table 1.1. The
systematic investigations necessary led to the use of surrogate strains, such as MS2 coliphage, presenting
similar advantages with the lab E. coli strains.
26
Table 1.1 – Examples of fecal-related viruses contained in the feces and their associated diseases
(Carter 2005, Glass et al. 2009, Mayer et al. 2008, Okoh et al. 2010, Rodriguez et al. 2014)
Type (Family) Associated disease
Rotavirus (Reoviridae) Diarrhea in infants
Enterovirus (Picornavidae) Meningitis, severe conjunctivitis, poliomyelitis
Adenovirus (Adenoviridae) Gastro-enteritis, pneumonia
Norovirus (Calciviridae) Gastro-enteritis
Figure 1.2 – Infection mechanism of the bacteriophage MS2 (Source file:
http://faculty.washington.edu/jclara/301/images/ssRNA.jpg). Inset: MS2 structure (Credits: Stephan
Spencer, http://www.virology.wisc.edu/virusworld/imgency/ms2MS22.jpeg)
27
The fungal kingdom is historically the less intensively studied among the ones in this Thesis, but these
microorganisms present characteristics which vary significantly from bacteria or viruses. Yeasts are
eukaryotic microorganisms, which are created with more complex cell walls, more advanced life functions
and suspected higher resistance to treatment (Temple et al. 2005). Although their expected number in
wastewater is low, these traits state them as an interesting target. Furthermore, their presence has been
linked with serious chronic (such as candidiasis) or opportunistic diseases (Thabet et al. 2014). Some
representatives are the Candida species, the Fusarium and the Aspergillus.
Figure 1.3 – Saccharomyces cerevisiae (yeast model) structure (Thabet et al. 2013)
1.2. Problems related with microorganisms’ and micropollutants’
presence
The problem of microorganisms’ occurrence in water sources has been identified for many decades.
Water related diseases plague developing countries using compromised drinking water sources
(McGuigan et al. 2012), or reusing wastewater for food production (Qadir et al. 2010), but also many
outbreaks have occurred by cross contamination of public access waters in the developed states (Hoebe
28
et al. 2004). Apart from the notorious diseases such as cholera, gastro-enteritis or dengue fever, the
contamination of water sources poses risks to populations which have incorporated their use in their
economical-related activities, such as fishing or other artisanal activities.
The main problem associated with the occurrence of micropollutants (MPs) in the environment is the lack
of information, concerning the side-effects of their presence in the receiving matrix (Deblonde et al. 2011).
For instance, little is known on the long term effects of pollutants, classified as “potentially not harmful”;
there are no studies on the accumulation or the chronic toxicity of such substances neither in plants,
animals, nor in humans. There is a relatively long list of MPs actually found in the environment, which
derived from the various anthropogenic activities (Focazio et al. 2008, Schwarzenbach et al. 2006). To
date, not all substances have been assessed on their potential actions against the environment.
Furthermore, toxicologically speaking, most of the substances that have been assessed for their risks,
have been directed through single-compound investigations, when the reality differs significantly
(Gregorio and Chèvre 2014). The environment contains a mixture of a vast number of compounds, which
could even react with each other, affecting their mode of action (Backhaus et al. 2003). The result has
been demonstrated to be severe, with cases reporting compounds that had no prior effect on species, to
demonstrate harmful properties when found in mixtures (Deneer 2000, Junghans et al. 2006, Rodney et
al. 2013).
Apart from the toxicity problems, other critical PhAC-related issues that have emerged over the years are:
i) The enhancement of antibiotic resistance, by the presence of antibiotics and their
metabolites in the environment (Rizzo et al. 2013),
ii) The problematic identification of the transformed metabolites of drugs (Fatta-Kassinos et al.
2011),
iii) The bioaccumulation of pollutants in living organisms in the environment (Figure 1.4).
29
Figure 1.4 – Bioaccumulation of MPs (http://toxics.usgs.gov/regional).
1.3. Hospital WW and pollutants
1.3.1. HWW and MPs
Hospital wastewater (HWW) is the result of the residue collection from the various water-consuming
activities taking place within its premises. These services include (Verlicchi et al. 2012) (Figure 1.5):
i) Human sewage
ii) Kitchen and laundry
iii) Heating and cooling processes’
iv) Laboratorial discharge (clinics, research centers)
v) Wards and outpatients contribution
The first categories are common also in MWW, which is the reason that led practitioners to suggest co-
treatment in MWWTPs, sometimes with only a pre-treatment (e.g. chlorination) (Emmanuel et al. 2004),
only to limit the microbiological-related risk. The reality suggests that within HWW there are many
substances, such as disinfectants, organic compounds, therapeutic metals, rare microbial agents or
antibiotic-resistant ones (Boillot et al. 2008, Emmanuel et al. 2005, Hawkshead III 2008), often in high
concentrations that modify significantly the composition of HWW compared to MWW. For this reason,
30
many authors have openly objected to the co-treatment practice so far (Altin et al. 2003, Pauwels and
Verstraete 2006, Vieno et al. 2007).
The presence of PhACs in hospital wastewater is a hot topic, with a variety of works dedicated in the
characterization of their nature (Kosma et al. 2010, Kümmerer 2001, Mahnik et al. 2007, Suarez et al.
2009, Verlicchi et al. 2012) and their importance in the overall load (Fatta-Kassinos et al. 2011). The
characteristics of HWW are influenced by a variety of factors, such as the size of the hospital, the range
of services and activities, the season of the year, the time of the day (Verlicchi et al. 2012, Verlicchi et al.
2010), and more. Table 1.2 presents an overview comparing HWW with MWW, in terms of a single unit
(patient/inhabitant).
Figure 1.5 – Contribution of HWW in pollutants integration to the environment
(http://www.frontiersin.org/files).
It is obvious that the composition of either micro or macropollutants in each case is significantly different
(see Table 1.2), indicating one of the reasons for failure of treatment by conventional WWTPs. The
micropollutants arriving in WWTPs are of a range of μg or ng, and also are reported to affect the nature
of the WW in the treatment plant (solubility, volatility, adsorbability, absorbability, biodegradability,
polarity and stability) (Verlicchi et al. 2010).
31
Table 1.2 – Comparison between indicative UWW and HWW effluents characteristics (Carraro et al.
2016, El-Ogri et al. 2016, Verlicchi et al. 2010) and references therein).
UWW HWW
BOD 60 160 mg/L COD 110 280 mg/L SS 80 135 mg/L
Bacteria Total Coliforms 106 7.7*109 MOs/L Viruses Norovirus 1.6*102 2.4*106 MOs/L
Hepatitis A virus 102 104 MOs/L Adenovirus 1.6*102 2.8*106 MOs/L
For the pre-mentioned reasons, HWW should be treated as a separate entity (Verlicchi et al. 2010). The
economic and overall risks should be assessed (Pauwels and Verstraete 2006), on-site treatment should
be implemented as close as possible to the source (H. Jones et al. 2005, Ikehata et al. 2006), the
consideration of no-mix toilets for urine separation must be taken into account (Lienert et al. 2007) and
reducing the quantities can considerably mitigate the effluent amounts if direct discharge in surface water
is expected.
1.3.2. HWW and MOs
Similarly to MPs, HWW are carriers of higher microbiological agent loads, compared to their urban
counterparts. In principle, the UWW are subjected to higher dilution and the intrinsic properties of HWW
imply the presence of higher and possibly more infectious agents. Carraro et al. in their recent review
(Carraro et al. 2016) have presented the differences between UWW and HWW effluents in various
countries, with compelling differences in the distribution of microorganisms’ species and quantities. This
microorganism load is usually led to co-treatment with UWW in MWWTPs and their removal efficiency is
a function of the existing treatment. Among others mentioned before, some authors (El-Ogri et al. 2016)
stressed the importance of treating HWW separately, on-site, to effectively reduce micro- and macro-
pollutants, but also stressing the need for microorganisms’ elimination. Problematic treatment or
inexistent treatment can lead to the problems mentioned before (antibiotic resistance, bioaccumulation
etc) but also, can directly jeopardize the drinking water sources in developing countries (Kilunga et al.
2016).
32
1.4. Occurrence, treatment and fate of MPs in MWWTPs
1.4.1. MP Occurrence in WWTPs
As the removal of microorganisms in this Thesis will focus on the mechanistic interpretation of the
inactivation phenomenon, while micropollutant removal will deal with the application in MWWTPs, in this
part their fate and transport within MWWTPs will be mainly addressed to clarify the series of events based
on the existing literature. There are several works reporting the presence and concentrations of MPs in
WWTPs, recently reviewed by Luo et al. (2014). However, one should take into account that the
concentration of MPs is a dynamically evolving phenomenon; measuring the MP content of a WW sample
is simply an instance, a snapshot that does not represent the factors involved in the process. The
occurrence of MPs in WWTPs is related to:
i) Supply rate (the rate of production)
ii) The drug availability (market restrictions)
iii) Population issues (increasing with higher numbers)
iv) GDP of the country (developed vs. developing countries)
v) Size of the WWTP (inhabitants equivalent)
vi) Special connections (industrial effluent and/or hospital WW)
vii) Water consumption (per capita)
viii) Persistence of compounds (type of pollutants)
ix) Metabolic rate of compounds (excretion rates)
1.4.2. MP evolution path in WWTPs
Municipal WWTPs at their current state are designed to handle bulk substances, such as organic matter,
phosphorus and nitrogen. The treatment of micropollutants is a latest addition and elutes specific
handling in the said installations, harboring the danger of subsequent release in water bodies. Typically,
a WWTP consists of primary treatment, followed by biological treatment/secondary clarification. Tertiary
treatment or disinfection units were additions and improvements during the last decades for effluents
destined for specific purposes. During this sequence, MPs are subjected to a number processes during
their passage through the various stages.
a) Primary treatment: In principle, primary treatment is neither destined nor capable of removing
MPs (Carballa et al. 2004, Kosma et al. 2010, Luo et al. 2014). Their low elimination is due to
sorption in primary sludge or bigger solids (Jones et al. 2006, Kosma et al. 2010, Ternes et al.
2004). In cases of aerated grit removal, increase of phenolic compounds is even expected (Kosma
et al. 2010, Nie et al. 2012).
33
b) Secondary treatment: Biological processes are expected to contribute to the removal of the
majority of the pollutants. The processes involved, such as dispersion, dilution, partition,
biodegradation and abiotic transformation (Luo et al. 2014) and less to volatilization (Verlicchi et
al. 2012). It has also been found (Margot et al. 2013) that from the 70 dissolved organic
micropollutants detected in raw effluent, 50 were removed under a 50% in the activated sludge
process. Adding nitrification improved the process in many instances (Jones et al. 2006, Kosma et
al. 2010, Margot et al. 2013). However, the biodegradability of many substances is limited, hence
leading to low percentage removal rates (Kosma et al. 2010).
c) Tertiary treatment/disinfection units: During this step, and more specifically during
flocculation/sedimentation MPs with logKow>3 can be removed, because they are more likely to
adsorb to flocs. Free chlorine has also been reported to react with some micropollutants (Kosma
et al. 2010). More details on the oxidation processes will be given later.
At this point, it is interesting to note the rather peculiar phenomenon of MP concentration increase during
their presence in WWTPs. Some human metabolites of the parent MP are secreted by the human feces
(Luo et al. 2014). More often, some semi-metabolized substances can be re-transformed back to their
original form (Göbel et al. 2007, Kasprzyk-Hordern et al. 2009). In these cases, the effluent concentration
is higher than the reported influent one.
1.4.3. Factors affecting MP removal in WWTPs
Along with the type of MP itself, the case-specific treatment sequence in WWTPs can influence the
removal rates, aided or hindered by the governing environmental conditions (Kosma et al. 2010). In
general, the physicochemical characteristics of each specific MP defines its removal possibilities. A
summary of commonly encountered micropollutants and their removal rates/classification is given in
Table 1.3.
Table 1.3 – Classification of commonly studied micropollutants (based on removal efficiency).
Low removal (<40%) Atrazine, carbamazepine, diclofenac, metoprolol…
Medium removal (40-70%) Atenolol, ketoprofen, sulfamethoxzole…
Highly removed (>70%) Acetaminophen, bisphenol A, ibuprofen, naproxen…
The two main categories of factors affecting the removal of MPs in WWTPs are the internal (MP-specific)
and the external ones (WWTP-specific). More specifically:
i) Internal factors (Luo et al. 2014): sorption, biodegradability, volatility, hydrophobicity etc.
In general, the chemical structure is defining the removal rates in high percentage. The most
34
easily degraded compounds are the ones with long side chains, the unsaturated aliphatic
compounds and the sulfate, halogen or the ones possessing electron withdrawing groups
(Jones et al. 2006, Tadkaew et al. 2011). Another main mechanism (sorption) relies on the
lipophilicity (logkow) and the acidity of the various functional groups (pKa), for absorption and
adsorption, respectively; pH values above pKa causes phenolic dissociation thus causing
charge repulsion with negatively charged membranes. Therefore, the affinity with the
bacterial enzymes is modified (Siegrist et al. 2005). Finally, other important parameters are
the Henry’s coefficient (H), governing the volatilization of MPs while treatment in the aeration
tank, and the biodegradation rate constant (kbiol); however this value is affected by external
factors and changes in dynamic way.
ii) External factors (Luo et al. 2014): treatment conditions, competition among MPs and WW
physicochemical characteristics. Sludge and hydraulic retention times (SRT and HRT)
determine the fate of the (biodegradable) MPs. Nitrifying conditions through buildup of
bacteria can enhance the removal of various compounds (Fernandez-Fontaina et al. 2012,
Suarez et al. 2009), nitrogen removal through nitrification and denitrification above 10 days
influences favorable removal rates (Clara et al. 2005) while extended HRT prolong the
available time for sorption and biodegradation (Göbel et al. 2007). Finally, redox conditions,
pH and temperature during treatment can affect either the biodiversity of microbial flora
(Göbel et al. 2007), their favorable growth conditions or the solubility of MPs in WW, leading
to low removal rates (Cirja et al. 2008), as well as phosphorus precipitation, which enhances
sorption.
Nevertheless, the aforementioned mechanisms cannot remove the micropollutants from WW, and
complete elimination relies on further, “quaternary” treatment, such as advanced oxidation treatment.
1.5. AOPs action in chemical and microbiological pollutants’
degradation
Due to the recalcitrant nature of many existing MPs, the existing biological and physicochemical treatment
methods have been proven unable to efficiently degrade them in WWTPs (Luo et al. 2014). Their
degradation however has been achieved by the use of ozonation or AOPs. These processes have
successfully mineralized or converted the persistent MPs to less harmful forms (Ikehata et al. 2006). AOPs
can be used as pre-treatment or post-biological treatment processes. Depending on the target, they can
achieve conversion of recalcitrant pollutants to biodegradable ones, or act as a polishing step. In the
respective cases, the residence time in biological treatment is reduced or the residual pollutant content
35
can be eliminated (Gernjak et al. 2006, Mantzavinos and Kalogerakis 2005, Oller et al. 2011, Ribeiro et al.
2015).
Ozonation and AOPs are redox technologies with main characteristic the non-selectivity on the target and
share the production of the highly oxidative hydroxyl radical (HO●) (Luo et al. 2014). After fluorine, the
HO● is the second most powerful oxidant (3.03 eV, compared to 2.80), with reaction rates ranging from
10-6 to 10-9 M-1 s-1 (Michael et al. 2013).
The AOPs typically involve chemical agents (metals, ozone or hydrogen peroxide) and an assistive energy
source, such as UV or visible light, current, ultrasound or γ-irradiation (Oppenländer 2003). Some
examples of AOPs are (figure 1.6):
Ozone-based: O3/H2O2, O3/UV, O3/UV/H2O2
UV-based: UV, UV/H2O2
Fenton-related: (Fe/H2O2), including photo-Fenton, electro-Fenton etc
Heterogeneous photocatalysis, such as (TiO2/hv)
γ-radiolysis
Ultrasound-based: sonolysis, ultrasound-supported Fenton etc.
Although the hydroxyl radical is the main oxidizing agent in these processes, their application often
induces the production and participation of other reactive oxygen species (ROS), such as superoxide
radical anions, hydroperoxyl radicals, singlet and triplet oxygen etc. (Ikehata et al. 2006, Oppenländer
2003). Another main advantage of the AOPs application is the characteristic versatility with which the
method can be achieved. For instance, photolysis acts directly or indirectly, by absorption of energy and
excitation or photosensitizing agents, typically dissolved organic matter (DOM) (Michael et al. 2013).
Finally, the AOPs can not only be used as a final, polishing step in order to degrade the persistent MPs in
WW, but also as a means to cause partial degradation of many compounds. This strategy is known to
cause increase in the biodegradability of organic compounds (Alvares et al. 2001), and is interesting
practice, especially for hospital or industrial effluents. If factors as pH are adjusted before and/or after
treatment (to enhance the AOP action and then prevent residual activity from oxidants) and toxicity is
mitigated, the effluent could be discharged at surface water. In the case of MWW, the organic matter
content combined with the high amounts of influent, is a prohibiting factor in this strategy. Hence, in most
applications AOP units are installed after secondary treatment (Ikehata et al. 2006).
36
Figure 1.6 – Categorization of Advanced Oxidation Process (Poyatos et al. 2010)
The two main groups of AOPs under study in the Thesis will be the UVC-based and Fenton-related ones.
More specifically, the methods drawing the interest will be:
1) UV photolysis
2) UV/H2O2
3) Fenton reaction
4) Photo-Fenton reaction
5) Solar exposure
In this thesis, the UV-based studies concern mostly application possibilities, while the Fenton-related
more fundamental and mechanistic aspects. Hence, special focus will be given here in the respective
literature and parameters of each process.
1.5.1. UV-based processes (UV, UV/H2O2)
UV treatment consists on the direct photo-transformation of organic compounds. In UV direct photolysis,
the micropollutant must absorb the incident radiation and undergo degradation starting from its excited
state. This treatment has been the most known and widely used irradiation method in initiating oxidative
degradation processes. Some organic pollutants effectively absorb UV-C light directly, and absorption of
this high-energy can cause destruction of the chemical bonds and subsequent breakdown of the
contaminant.
37
The main factors which will affect the degradation of MPs in light assisted processes are the UV absorption
and its quantum yield (Legrini et al. 1993). The molar absorption coefficient, i.e. UV absorption is an
indication of the strength with which a molecule absorbs UV, and consequently, cause its degradation
(Kim et al. 2009a, b, Michael et al. 2013). In principle, reaction kinetics of the organic substrate with the
oxidant are described by second order law, as follows (Eq.1.1):
(1.1)
where r(-M) represents the rate of degradation of the MP. At the same time, direct photolysis contributes
in the dual manner mentioned before, provided that other WW constituents and physicochemical
characteristics are present, such as pH conditions (Ikehata et al. 2006). However, it must be noted that
although some MPs are susceptible to both ROS damage and light action, others are not easily affected
by the radicals (such as ICM Iohexol) and others (such as TCEP and TCPP) which are impervious to both
types of attacks (Gerrity et al. 2011). Other important factors include the concentration of the target
compound, the pH of the matrix, the amount of H2O2, the presence/absence of scavenging compounds
(e.g. bicarbonates) and the reaction time.
This treatment is considered an advanced oxidation process because it involves the generation of hydroxyl
radicals (HO•) produced by homolytic cleavage of hydrogen peroxide. Photolysis of H2O2 yields two HO•
radicals per photon absorbed. The hydroxyl radicals are strong oxidants (E°=2.8V) with fast reactivity due
to their non-selectiveness. Hence, the removal rate of micropollutants has at least two contributions:
direct photolysis and hydroxyl radical attack. They might achieve high degrees of elimination (final
products are mainly CO2 and H2O) of several micropollutants. The efficiency of the process will depend
strongly on the HO production velocity. The propagation reactions are as follows (Eqs. 1.2-1.7):
2 ● (1.2)
● ● + (1.3)
● ● (1.4)
2 ● (1.5)
2 ● (1.6) ●+ ● (1.7)
The molar absorption coefficient of H2O2 is only 18.7 M-1.cm-1 at 254 nm (Zapata et al. 2010). Hence, the
efficiency of UV/H2O2 process decreases drastically with the presence of strong photon absorbers or when
the UV absorbance of the target pollutant is high.
38
Low-pressure mercury vapor lamps with 254 nm peak emission are the most common UV source used in
UV/H2O2 systems; however the maximum absorbance of H2O2 occurs at 220 nm. Hence, if low-pressure
lamps are used, a high concentration of H2O2 is needed to generate sufficient hydroxyl radicals because
of this low absorption coefficient. At the same time, at high concentrations, H2O2 scavenges the radicals
making the process less effective. Also, low pH is usually preferred, but in the case of UWW the
acidification/neutralization costs and implications rule out this option. The UV/H2O2 processes have
demonstrated efficiency against all compounds being able to be degraded by the HO radicals, but despite
their low environmental footprint, their operation cost halts the high degrees of commercialization.
Nevertheless, on research level, the use of this process in wastewater treatment is depicted by the
important number of publications produced during the last decade.
In order for UV light to inactivate microorganisms, the UV photons must get in contact with the cell. UV
energy penetrates the outer cell membrane, passes through the cell body and disrupts its DNA, preventing
its replication and therefore the microorganism reproduction. More specifically, UV light disrupts the
dividing of the deoxyribonucleic acid (DNA) (genetic material, chromosomes) and the production of
enzymes (Das 2001). The components within the DNA that absorb the UV light are the nucleotide bases:
adenine, guanine, thymine, and cytosine. Although proteins fulfill many vital functions in cells, their UV
absorption compared with that of DNA is of minor importance. This absorption of UV energy forms new
bonds between adjacent nucleotides, creating dimers. Dimerization of adjacent pyrimidine molecules,
particularly thymine, is the most common form of photochemical damage (Das 2001). The nucleotides
differ in their ability to absorb UV light and undergo a permanent chemical change. The pyrimidines
(thymine and cytosine) are ten times more sensitive to UV light than the purines (adenine and guanine).
Among the pyrimidines, thymine undergoes change the most readily and the dimers are very stable (Das
2001). Ultimately, the effect of numerous dimers forming along the DNA chain inhibits replication of the
organism.
The combined UV/H2O2 process builds on the principles of the UVC disinfection, plus the homolytic
disruption of H2O2. The mechanism of UV/H2O2 inactivation, is both external and internal. Externally, the
massive generation of HO● ensures oxidation of the bacterial membrane and cell lysis, while the H2O2
which penetrates the bacterial membrane is also cleaved and HO●-mediated damage ensues internally.
The natural, enzymatic defense mechanisms of the bacterial cell against ROS, such as catalase, dismutases
and peroxidases are unlikely to protect the microorganism in presence of UVC light. When H2O2 is added
into the bulk, the HO● attacks improve all the processes; till now, there is no microorganism found with
resistance to the oxidation by HO●, contrary to damages by UVC irradiation which can be repaired instantly
(Sinha and Häder 2002).
39
The most important factors that affect the UV and UV/H2O2 disinfection/decontamination capacity are
the following:
1) Water Quality
A number of substances can inhibit the transmission of ultraviolet rays through water, so special emphasis
must be given to the treatment prior to the exposure in UV (Darby et al. 1999). Certain contaminants in
water can reduce the transmission of UV light through the water, which reduces the UV dose that reaches
the bacteria. These UV-absorbing substances include micro-contaminants, but also humic and fulvic acids,
with high absorption coefficients.
2) Suspended Solids
Although in influents the suspended solids are mainly of terrestrial origin, the corresponding ones in
biologically treated effluents are typically composed of bacteria-laden particles of varying number and
size. Some of the suspended solids in wastewater will absorb or reflect the UV light before it can penetrate
the solids to kill any occluded microorganisms. UV light can penetrate into suspended solids with longer
contact times and higher intensities but there is still a limit to pathogen inactivation. Suspended particles
are a problem because microorganisms harbored within particles are shielded from the UV light and pass
through the unit unaffected.
3) Particle Size Distribution
Particle size distribution (PSD) measurements of wastewater effluent are used as an indicator of filter and
clarifier performance (Jolis et al. 2001). Even though the SS concentrations of different effluent samples
can be similar, their particle size distributions are significantly different because of the different treatment
processes before disinfection. Therefore, the influence of particle size may explain why traditional solids
measurements do not provide accurate prediction results of UV disinfection (Brownell and Nelson 2006).
4) Iron
Iron affects UV disinfection by absorbing UV light. If the concentration of dissolved iron is high enough in
the wastewater the UV light will be absorbed by the iron complexes before it can kill any microorganisms
(Das 2001). Another common problem is the iron settling onto the quartz sleeves; iron will precipitate on
the quartz sleeves and absorb the UV light before it reaches wastewater (Das 2001). This can increase
maintenance costs since the sleeves must be cleaned regularly. Finally, adsorption of iron onto suspended
solids, clumps of bacteria and other organic compounds can occur. This adsorbed iron will prevent UV
light from penetrating the suspended solids etc. and inactivating the entrapped microbes (Das 2001). On
the other hand, iron can be removed with proper pre-treatment and eliminate possible downstream
issues.
5) Hardness
40
Calcium and magnesium salts, which are generally present in water as bicarbonates or sulfates, are the
source of water hardness. The main problem with hard water is the formation of mineral deposits. These
products precipitate and coat on any warm or cold surfaces. The optimum temperature of the low-
pressure mercury lamp is between 40 °C and 104 °F. Therefore, a molecular layer of warm water can form,
where calcium and magnesium salts will be precipitated. These precipitates will prevent the UV light from
entering the wastewater (Das 2001).
6) Wastewater Source
This category engulfs special wastewater sources, such as the ones originating from textile industries.
These industries may be periodically discharging low concentrations of dye into the municipal wastewater
collection system. In this case, the effluent will be heavily colored when it reaches the treatment plant.
Dyes can readily absorb UV light thereby preventing UV disinfection (Das 2001). Dyes absorbing UV can
seem contradictory with color not affecting UV light. However many textile dyes and colorless auxiliary
substances are absorbent in the UV range.
7) Temperature
The climatic variation as well as the seasonal changes in the environmental temperature affects the
wastewater and the efficiency of UV disinfection. The kinetics of the UV disinfection process was highly
affected by system operations at extreme temperatures, i.e., at 10 and 45°C (Abu-ghararah 1994). Higher
inactivation constants were noticed in temperatures as high as 45°C and lower when the water
temperature was at 10°C, respectively.
8) Bacterial Strains
As in this thesis, only bacteria will be subjected to UV treatment, special focus will be given in the
difference among bacterial strains. Escherichia coli are commonly employed as an indicator
microorganism, as they are easily propagated and detected in the laboratory. The various strains of E. coli
(wild-type, UV-resistant and antibiotic-resistant strains) frequently encountered when the sanitation
system of hospitals malfunction, can demonstrate differential demand of UV fluence in order to be
eliminated (Quek and Hu 2008). Generally, wild or environmental strains show greater resistance to UV
rays. Also, the required laboratorial disinfection doses are lower than the ones of the real applications
and therefore the constants need correction. The evaluated studies (Hijnen et al. 2006) suggest a two
times increased fluence requirement for bacteria and four times for bacterial spores in drinking water.
For wastewater this is most likely not enough and a factor of seven seems more appropriate (Hijnen et al.
2006).
41
1.5.2. Fenton-related reactions (Fenton, photo-Fenton, solar light)
The Fenton process is an attractive oxidative system for wastewater treatment, due to iron abundance in
nature and low inherent toxicity, as well as the fact that hydrogen peroxide is easy to handle and
environmentally safe, decomposing spontaneously to H2O and O2.
It has been demonstrated that Fenton’s reagent is able to destroy toxic compounds in wastewater
(Andreozzi et al. 1999). Production of HO radicals by Fenton reagent occurs by means of addition of H2O2
to Fe2+ salts trough the following reactions (Neyens and Baeyens 2003, Stasinakis 2008). “R” is used to
describe the reacting organic compound and L is an organic ligand (Eqs. 8-11):
(1.8)
(1.9)
(1.10)
● (1.11)
However, exposure to light enhances the Fenton reaction by the photo-regeneration of Fe (II), when
reducing Fe (III). Hence, there is a double production of hydroxyl radicals (Poyatos et al. 2010) (Eq. 1.12):
(1.12)
Thus, photo-Fenton is a process that is able to use solar radiation as input taking advantage not only of
the UV portion contained in solar radiation but also because of the ability of some compounds such as
ferro-hydroxy and ferro-acid to absorb energy in the visible spectra (Figure 1.7).
Figure 1.7 – Light absorption of Fe3+ species at normal solar irradiance (I) on the Earth’s surface
The use of solar light as source of radiation for activating the hydroxyl radicals is not a new concept:
several researches have proved the efficiency of solar light as an activating agent for the Fenton reaction.
In this process, the Fe(II) is continuously recycled, reducing the amount of iron salts required (and their
42
further disposal) for the Fenton’s reaction. This feature makes the photo-Fenton process more applicable
and attractive for application in sunny regions around the globe.
Recently, Giannakis et al. have reviewed the mechanisms of photo-Fenton inactivation of microorganisms,
as well as the reported applications on water and wastewater disinfection (Giannakis et al. 2016a,
Giannakis et al. 2016b). The necessary steps to inflict inactivation of microorganisms (especially bacteria)
is explained below.
1) Direct action of light: The action of solar light (UVA and UVB light) is the baseline action, although
unimportant for MPs (photolysis), has multi-level contribution against biological targets. UVB
wavelengths lead to the formation of same-strand photo-adducts among nitrogen-containing
bases, or even in double stranded DNA. The photoproducts are cyclobutane pyrimidine dimers
(CPDs), pyrimidine (6-4) pyrimidone dimers, monomeric pyrimidine (cytosine) photoproducts, or
purine base photoproducts. In overall, the direct effects of UVA can be characterized as less
harmful, compared with the rest of the UV light wavelengths, but the direct absorption by DNA,
proteins and other structures is noteworthy.
2) Indirect action of light: Light induces a Fenton process inside the cell, which is the main indirect
pathway. When solar light is provided to the bacterial cells, the chain reaction of events follows a
complex mechanism, initiated by two simultaneous fronts: action of light and action of ROS.
Assuming that a cell is preserving its normal ROS cycle, light addition creates a chain of oxidative
events. UVB can enhance H2O2 accumulation and induce excess production in E. coli cells in
vivo (Gomes et al. 2004, Knowles and Eisenstark 1994). Also, singlet oxygen (1 ), key factor in
cytotoxicity and gene expression (Basu-Modak and Tyrrell 1993, Tyrrell And Pidoux 1989, Tyrrell
et al. 2000) can be generated by UVA irradiation, through excitation of chromophoric substances,
such as porfyrins (Tyrrell et al. 2000).
As it seems, there is an over-accumulation of ROS inside the cell, which is only made worse by the
inactivation of the key enzymes by the action of light; CAT and SOD reduce significantly their
activity when exposed to UVB or UVA light (Imlay 2003, 2008, Santos et al. 2013). It has long been
suggested that near-UV induces mutations in bacteria (in macroscopic level) and the explanation
has been attributed to the excess H2O2 accumulated into the cell and the subsequent reactions
involved with it (Eisenstark 1998). UVA has also been known to affect the respiratory chain of E.
coli, with some of the mechanisms suggested (Bosshard et al. 2010) being verified in this cycle of
events. A malfunctioning electron transport chain would provide electrons, with many reductants
now available to accept them and convert themselves to reactive intermediates.
3) Enhancement of the photo-induced actions by H2O2 and/or Fe: The first instance of synergistic
inactivation by near-UV light and H2O2 was demonstrated by Anathaswamy and Eisenstark
43
(Ananthaswamy and Eisenstark 1976) for phages and Hartman and Eisenstark some years later
(Hartman and Eisenstark 1980) for E. coli K-12. The following years many works have been
developed to assess the H2O2-enhanced photokilling modes and parameters that are involved
(Fisher et al. 2008, Fisher et al. 2012, García-Fernández et al. 2012, Hartman and Eisenstark 1978,
Keenan 2001, Khaengraeng and Reed 2005, Ng et al. 2015, Sciacca et al. 2010, Spuhler et al.
2010)). The majority of the works agree that the involved mechanism is in fact a light-enhanced
internal photo-Fenton reaction. The prevailing mechanism is as follows.
i. The direct damage of the light affects the DNA and the enzymes responsible for its
reparation (direct action).
ii. Light is disrupting the normal ROS-scavenging enzymes into the cells such as catalase,
superoxide dismutase, peroxidases etc. (indirect action)
iii. H2O2 penetrates the cell, causing imbalance of ROS into the cells.
iv. ROS and light release iron into the cytoplasm, with reacts with H2O2 to create ●. Other
ROS are involved into the reduction of iron, or directly attack susceptible moieties (oxidative
stress).
v. Added H2O2 affects bacterial membrane (outer damage), initiating its auto-oxidation.
vi. Light reduces ferric iron to ferrous directly, through ligand-to-metal charge transfer
(LMCT) or indirectly, through the reactive intermediates available by the light-induced
malfunctioning into the cell, initiating a photo-catalytic cycle.
As far as iron addition is concerned, the various steps are presented here:
Step 1: addition of Fe2+ internal action. Iron can diffuse into the bacterial cell quite easily (Braun 2001,
Touati 2000) due to low charge density and difference in osmotic pressure between the cell and the
matrix. From this point and onwards, it is available as a readily oxidizable catalyst.
Step 2: addition of Fe2+ external action. Fe2+ addition, in presence of H2O2 in the matrix, can drive a
homogeneous photo-Fenton process, for a limited period of time. Fe2+ is soluble in water, and by reaction
with H2O2, production of ● is achieved in a big extent, effectively degrading the external cell
membrane and resulting in microorganism degradation
Step 3: Fe3+ formation/addition (in presence of bacteria). Bacteria are known to produce siderophores
such as enterobactin, aerobactin, and ferrichrome, which are able to metabolically chelate Fe3+ present
in the cell (Köster 2001, Upritchard et al. 2007), to cover their needs in Fe3+. These proteins efficiently bind
to Fe3+ and create complexes, therefore facilitating internal photo-assisted LMCT and production of ●.
Step 4: Iron Oxides formation from Fe2+/Fe3+ addition. After conversion of Fe2+ to Fe3+, the Fenton process
is considered as limited, since Fe(OH)2+ has limited solubility at near-neutral pH and therefore, exploitation
44
of its photoactivity is limited (Ruales-Lonfat et al. 2014). Instead, zero-charge complexes are formed, such
as , which are prone to oxidation and formation of solid iron oxides, such as magnetite, goethite,
lepidocrocite, or feroxyhyte (Jolivet et al. 2004).
Step 5: Semiconductor action mode of iron oxides. Iron oxides, either naturally present in water (Cornell
and Schwertmann 2006) or laboratory-prepared (Cornell and Schwertmann 2006) are among the most
reactive components within the matrix. Their chemical activity involves potential photocatalyst activity, if
the hole-electron recombination (electron returning to an empty state) problem is overpassed (Zhang et
al. 1993).
Step 6: Heterogeneous (photo)Fenton reaction. Iron oxides in presence of H2O2 can play the role of an
efficient heterogeneous photo-catalyst, towards, bacterial inactivation (Ruales-Lonfat et al. 2015, Ruales-
Lonfat et al. 2014), in two ways. Firstly, in presence of siderophores, they can contribute to the supply of
dissolved Fe2+ in the bulk (Upritchard et al. 2007). Furthermore, H2O2 can start a series of reactions, at
which iron hydroxide ligands can get reduced, with simultaneous hydroperoxyl radical formation
(Upritchard et al. 2007). Under light, the production of hydroxyl radicals is also favored (Han et al. 2011).
1.6. Problem identification and contextualization: Micropollutants
and microorganisms in developed and developing countries
Since micropollutants have been identified in many cases as high risk compounds, many works have been
initiated to identify their presence in the environment (Kolpin et al. 2002, Luo et al. 2014). Moving in
backward steps, the presence in environmental water matrices is a result of a variety of pathways. One of
the main sources which will be further analyzed later on, are the MWWTPs, due to the collection of urban
and sometimes, (pre-treated) industrial effluents (Kasprzyk-Hordern et al. 2009).
Although the treatment in WWTPs is followed by natural processes, such as sorption, photolysis and
biodegradation, that can reduce the contaminant loads up to 10 times (Gros et al. 2007, Pal et al. 2010),
the MPs’ presence is still unambiguous. In a research conducted among many countries, the most
frequently encountered drugs were the non-steroidal anti-inflammatory drugs (NSAIDs),
Sulfamethoxazole, Carbamazepine and Triclosan (Luo et al. 2014). Generally, the occurrence of MPs was
less frequent in summer (probably due to elevated, temperature-driven biodegradation), and even
though winter rain promoted dilution, sometimes the contribution in natural water was important (Wang
et al. 2011). Finally, the concentrations found in surface waters was well correlated with the population
distribution, linked with the massive utilization of parent chemicals by a bigger number of users (Luo et
al. 2014).
45
Concerning drinking water, the studies are relatively few, because the occurrence is sometimes below the
detection limit (Vulliet et al. 2011, Wang et al. 2011). However, this is often a limitation of the
experimental capabilities of the analytical laboratories. Kummerer has discussed this problem, in the
appearance of “new” compounds, which could have been normally encountered (for pollutants in ng or
μg scale) (Kümmerer 2011), if the technology allowed so. Also, as far as long-term side-effects are
concerned, the presence of certain compounds or their intermediated in drinking water has not been
under study (yet). In overall, in the review published by Luo et al. (Luo et al. 2014) it is mentioned that
most of the countries investigated (France, USA, Spain, Canada) were capable of removing the presence
of some MPs in drinking water. This is a critical step, considering that drinking water treatment is literally
the last line of defense among end-users and micropollutants (Ikehata et al. 2006).
Figure 1.8 – Routes of pharmaceutical contamination of the aquatic environment (Ikehata et al. 2006).
Although in developed countries water is considered a de facto supply in each household, in developing
countries, the reality is sometimes far from this state. Water acquisition can be an everyday struggle for
many families. If in this scenario, one thinks of the potential problems that could appear if MP pollution
is high, the risks are more imminent. The quality of life of the affected population is considerably
endangered, and more specifically not by chronic or potential problems, but from the harsh reality of raw,
untreated wastewater in the water supplies.
46
In many developing countries, the combination of rampant population growth and the lack of financial
means, have led to insufficient (up to inexistent) sanitation facilities. Therefore, the collection and the
treatment of wastewater is problematic. The poorest fractions of the population, who employ themselves
in handcraft, fishing and agricultural activities suffer the most, since the situation in centralized, capital
areas is slightly better. However, these areas have demonstrated unacceptable treatment, especially in
(semi)industrial or hospital effluents, with cases describing direct untreated water being discharged in
rivers and sea.
“Fortunately”, the risk of MPs is relatively less, when compared with developed countries. The availability
of drugs and the capability of purchase restrict the widespread use and the diffuse pollution. The main
areas expected to provide major MP flows are the hospitals and similar facilities. Recent research that has
been performed in the framework of the “Treatment of the Hospital wastewaters in Ivory Coast and in
Colombia by advanced oxidation processes” (unpublished data) indicated that even in this case, the
majority of administered drugs are biodegradable and the MP content is limited in isolated hospitals in
Colombia, but in the University Hospital in Abidjan, the situation is quite problematic.
On the other hand, even when the amounts of MPs is not alarming, the presence of microorganisms in
WW is an important matter, which becomes top priority, since no disinfection process is applied in the
effluents. Therefore, the focus should be directed at least to microbial pollution, when it comes to
discharged WW in developing countries, which poses direct and acute illness risks. Hospitals are an
identified contributor to fecal and overall pathogen microorganisms in surface waters, and the lack of
treatment is directly jeopardizing their use (Kilunga et al. 2016). The current practices in agriculture for
instance, include the use of contaminated water for crops irrigation, and the transfer of pathogens is
highly possible. Therefore, monitoring of total coliform bacteria and aerobic mesophilic bacteria, as
representatives of fecal and non-fecal routes, respectively, should be monitored and their elimination
should precede discharge in natural water bodies.
1.7. AOPs vs. Micropollutants and Microorganisms: current status
Previously, the different classes of micropollutants have been mentioned, in order to classify the various
substances into different categories. Nevertheless, the anthropogenic pollutants surpass the 92 million
registered compounds (CAS registry-not all available on market). Hence, it is relatively impossible for
treatment facilities to take into account all substances in order to draw the strategies for protection.
However, not all of them pose a potential threat, nor cause (acute or chronic) problems, so the focus will
remain around the MP classes described in the previous sections.
47
Concerning the work already carried out, a literature review performed in 2013 (Michael et al. 2013)
indicated 5500 instances in Scopus, concerning treatment of pharmaceuticals by AOPs, and comparable
number of works exist for the rest of the classes of MPs (biocides etc). Also, if the topic is divided by the
efficacy of the different AOPs, for each AOP presented in Figure 1.6, the results are equally overwhelming;
against our targets, there are 3500 returned search results for UV-related processes, 4200 for Fenton-
based ones etc. Therefore, it can be easily understood that it is a very dynamic, hot topic, spanning only
in the last 15-20 years. In the same time, AOPs are a very powerful tool against the control of these
substances; the majority of the publications manage to efficiently degrade their targets, one way or
another. This indicates enormous windows of opportunity in applying AOPs as tertiary treatment
methods.
In general, research focuses on certain pillars, when it comes to treating pollutants. Some of the main
points of interest when working with AOPs are:
efficacy of certain processes against pollutants,
testing of classic AOPs against emerging pollutants
new pathways involved in degradation (due to analytical technological advances)
measurement degradation kinetics (compound-specific or mixture),
bench scale or field applications against new contaminants,
intermediates’ formation during treatment (treatment pathways),
potential toxicity problems during/after treatment,
improvement and optimization of the classic treatment processes,
statistical interpretation/integration of new mathematic tools (artificial neural networks),
development of new/combined treatment methods,
reuse and recycling of materials involved in the process,
replacement of old processes with environmentally friendly treatment methods or non-toxic,
“greener” reagents etc.
Another point worth commenting, are the results of the same search terms concerning AOPs against
microorganisms. The search results returned are orders of magnitude lower, when compared to
micropollutants. The reality is that the targets are significantly less, but of equal importance to MPs. In
any other sense, the focuses remain the same (as presented in the list) while shifting from chemical to
microbial contaminants. Keeping all the previous facts in mind, the critical question is to direct research
in context-specific basis, regarding the particularities of each context (developed/developing countries
and MPs/MOs) and suggesting proper solutions.
48
1.8. Thesis aims and objectives
As described in the previous chapters, the issue of hospital wastewater treatment has multiple contextual,
application and engineering extensions. The necessary strategies need to be specifically addressed
towards developed or developing countries, where HWW is channeled in UWW or is directly discharged,
respectively. The context differs significantly; the developed countries have more or less under control
the problem of MOs and focus on MPs, while developing countries’ priority should be the acute risk
caused by MOs presence. Furthermore, the AOP chosen has to be a function of the technical and
economic status of the place of application, with the UV-based methods being more prominent in
developed countries and the solar based ones more suitable for developing countries. As a result, the
present thesis takes account the aforementioned constraints and focuses on HWW treatment by AOPs in
developed and developing countries, both on the application point of view, as well as the underlying
mechanisms governing micropollutant degradation and microorganism inactivation.
Figure 1.9 – Thesis graphical representation and organization of aims and objectives.
In Switzerland (as an example of developed country), the wastewater effluents are treated and the
implementation of the relative AOPs focuses on the elimination of the chronic risk caused by the presence
of micropollutants in natural waters, and the acute risk of microbial infection due to the pathogens carried
within the flows. The micropollutants chosen in this Thesis derive from the modifications in the Swiss
legislation and the wild, indigenous bacterial population as microbial targets. In the first part, the effect
of different pre-treatment methods against these targets is of key interest.
49
In Ivory Coast and Colombia, as the involved countries in this research project, WWTPs are inexistent.
Therefore, the application of solar photo-Fenton as a feasible AOP is implied only after the construction
of basic treatment before (primary-secondary). The acute risk of microbial infections is prioritized and
studied extensively in the second part, taking a viral and a yeast pathogen model into study, as the photo-
Fenton against bacteria has already been a subject of the Thesis.
In the third and final part, as mass flows of special drugs derive from hospital and production sites, two
pollutants (Iohexol and Venlafaxine) in high amounts have been chosen and their degradation by relevant
AOPs was studied. These drugs can be encountered in the production wastewaters or in urine, due to the
treatment of patients, and the (pre)treatment of concentrated flows at hospital or manufacturing level is
desirable before dilution in the municipal wastes.
These objectives, organized in the respective chapters, can be summarized as follows:
Chapter 1: Introduction.
PART 1: Disinfection and decontamination of municipal WW as carrier of HWW pollutants in developed
countries by all proposed AOPs: implications of AOPs application in WW.
Chapter 2: Effect of advanced oxidation processes on the micropollutants and the effluent organic matter
contained in municipal wastewater previously treated by three different secondary methods.
Chapter 3: Micropollutant degradation, bacterial inactivation and regrowth risk in wastewater effluents:
Influence of the secondary (pre) treatment on the efficiency of Advanced Oxidation Processes.
PART 2: Hospital-derived microorganism inactivation in developing countries by Fenton-related AOPs:
mechanistic interpretation and underlying mechanisms of the photo-Fenton process.
Chapter 4: Effect of Fe(II)/Fe(III) species, pH, irradiance and bacterial presence on viral inactivation in
wastewater by the photo-Fenton process: Kinetic modeling and mechanistic interpretation
Chapter 5: Castles fall from inside: Evidence for dominant internal photo-catalytic mechanisms during
treatment of Saccharomyces cerevisiae by photo-Fenton at near-neutral pH..
PART 3: Degradation of hospital PhACs by AOPs, as a point-source treatment option in HWW and urine:
treatment optimization and degradation pathway elucidation.
Chapter 6: Iohexol degradation in wastewater and urine by UV-based Advanced Oxidation Processes
(AOPs): Process modeling and by-products identification.
50
Chapter 7: Solar photo-Fenton and UV/H2O2 processes against the antidepressant Venlafaxine in urban
wastewaters and human urine. Intermediates formation and biodegradability assessment.
Chapter 8: General Conclusions and Perspectives.
51
PART 1
Disinfection and decontamination of municipal WW as carrier of
HWW pollutants in developed countries by all proposed AOPs:
implications of AOPs application in WW.
53
2. Chapter 2: Effect of advanced oxidation processes on the
micropollutants and the effluent organic matter
contained in municipal wastewater previously treated by
three different secondary methods
Published work:
Stefanos Giannakis, Franco Alejandro Gamarra Vives, Dominique Grandjean, Anoys Magnet, Luiz Felippe
De Alencastro, and César Pulgarin. "Effect of advanced oxidation processes on the micropollutants and
the effluent organic matter contained in municipal wastewater previously treated by three different
secondary methods." Water research 84 (2015): 295-306.
Web link:
http://www.sciencedirect.com/science/article/pii/S0043135415301329
Supplementary material:
Appendix A
Doctoral Candidate’s contribution:
Main investigator and author.
54
2.1. Introduction
Currently, one of the environmental concerns in global scales is the presence and accumulation of
micropollutants (MPs) in the natural environment. These substances are comprising an increasing list of
anthropogenic contaminants, which include among others, pharmaceuticals, personal care products,
steroid hormones, industrial chemicals, pesticides and many other emerging compounds (Luo et al. 2014).
The majority of these substances are designed to be biologically active, and therefore, their occurrence
can affect the receiving environment. Some of the associated problems to MPs’ presence are the
ecotoxicity of their mixture (Gregorio and Chèvre 2014), the enhancement of antibiotic resistance by the
presence of antibiotics and their metabolites in the environment (Fatta-Kassinos et al. 2011), or the
problematic identification of the transformed metabolites of drugs in the nature (Fatta-Kassinos et al.
2011).
Wastewater treatment plants have been built, transformed and updated through the years to effectively
remove -among others- solids, organic and inorganic compounds (carbon, nitrogen, phosphorus etc.),
which were previously disposed in the environment. However, the challenge posed by the hydrophilic
MPs, is an obstacle the majority of the WWTPs are not equipped to handle. Margot et al. (Margot et al.
2013) have reported that from the 70 dissolved organic MPs detected in raw effluents, many of them
were removed at less than 30% in the conventional activated sludge process.
However, micropollutant degradation has been achieved by the use of ozonation or Advanced Oxidation
Processes (AOPs). These processes have successfully degraded or converted the persistent MPs to less
harmful forms (Ikehata et al. 2006). Although the hydroxyl radical (HO●) is the main oxidizing agent in
these processes (oxidative power: 2.80 eV), their application often induces the production and
participation of other reactive oxygen species (ROS), such as superoxide radical anions, hydroperoxyl
radicals, singlet and triplet oxygen etc. (Ikehata et al. 2006) The main advantage of the AOPs application
is the characteristic versatility with which the method can be achieved. For instance, photolysis acts
directly or indirectly, by absorption of energy and excitation or photosensitizing agents, typically dissolved
organic matter (DOM) (De la Cruz et al. 2012).
In Switzerland, actions against the issue of MPs were systematically taken since 2006, when the Micropoll
Strategy was implemented, by the Federal Office for the Environment (FOEN 2014). The outcome of the
project was an adaptation of the Water Protection Ordinance (GSchV) and 80% of the total MPs was
decided to be eliminated, with 5 substances playing the role of indicator (Table 2.1). The adaptation was
finally voted in 2014 and will be effective starting January 2016. WWTPs will have to eliminate at least
80% amount of 6 pollutants (from a list of 12), divided in “very well eliminated” and “well eliminated”, as
55
presented in Table 2.1. Oxidation (for instance by ozone or AOPs) or adsorption (activated carbon) are
suggested to tackle the issue.
Table 2.1 – Evolution of indicator pollutants in the Swiss legislation.
5 Indicators List of 12 indicators Pollutant type
(2009 list) (2016 enforcement)
Very Well Eliminated
Benzotriazole Amisulpride Antidepressant
Carbamazepine Carbamazepine Antiepileptic
Diclofenac Citalopram Antidepressant
Mecoprop Clarithromycin Antibiotic
Sulfamethoxazole Diclofenac Analgesic
Hydrochlorothiazide Diuretic
Metoprolol Beta blocker
Venlafaxine Antidepressant
Well Eliminated
Benzotriazole Anticorrosive
Candesartan Angiotensin II antagonist
Irbesartan Angiotensin II antagonist
Mecoprop Herbicide
In this work, the ability of AOPs to degrade MPs at lab scale, after 3 different secondary treatment
methods is tested. UV/H2O2 and solar photo-Fenton, as well as their three composing sub-processes (UV-
C at 254 nm, solar light and Fenton reaction), are considered as a final treatment step after Activated
Sludge (AS), Moving Bed Bioreactor (MBBR) or Coagulation-Flocculation (CF) treatment. 6 pollutants were
selected from the list of 12 indicators provided by FOEN, also contained in the WW from Vidy WWTP
(Lausanne, Switzerland). The degradation kinetics, the oxidation levels and the effect of the preceding
secondary treatment are given and the dependence of success as a function of the previous treatment
steps. Finally, considerations on the role of effluent organic matter (EfOM) are given.
56
2.2. Materials and Methods
2.2.1. Sampling campaign
In total, 4 sampling campaigns took place. The strategy was as follows: for two consecutive days, 2-L
samples were taken at 9am, 12pm and 15pm. The composite sample (12 L) was then mixed and
analyzed/treated. The physicochemical analysis was immediately performed, while the MPs were
analyzed the day after the creation of the composite (preservation at 4°C). The samples were collected
from the primary effluents (point 1, Figure 1) and at the output of the different secondary treatment
facilities in the WWTP of Vidy: Activated Sludge (AS), Moving Bed Bioreactor (MBBR) and Coagulation-
Flocculation (CF) (points 2, 3 and 4, Figure 2.1).
Figure 2.1 – Simplified overview of the Vidy WWTP and the sampling points used in the study.
2.2.2. Chemicals and reagents
All the chemicals for the experiments were used as received. Hydrogen Peroxide 30%, Iron Sulfate
Heptahydrate and Titanium Oxysulfate (1.9-2.1%) (for H2O2 determination) were acquired from Sigma-
Aldrich (Switzerland) and Sodium Bisulfite from Acros Organics (Switzerland).
Sand removal Screening Primary Clarifier
~20% MPs removal
Activated Sludge
Moving Bed Bioreactor
Coagulationon-n-Flocculation
2
~40% MPs removal
~25% MPs removal
1
3
4
Influent
57
2.2.3. Employed reactors
For the UV-C irradiation and UV/H2O2 treatment methods, two 300 mL double-wall, water-jacketed glass
batch stirred reactors were used in parallel. Each of them contained a 36-W, low-pressure amalgam lamp
(Model: UVI 40 4C P 15/300) from UV-Technik Speziallampen. These lamps have an emission irradiance
of 350 μW/cm² at 254 nm and 9 W output. During the experiments, the temperature of the reactors was
water-controlled at 22 °C with a Neslab RTE-111 recirculating thermostat.
For the Fenton experiments, 100-mL dark Pyrex reactors were used. Wastewater was continuously stirred
(300 rpm) with magnetic bars and the photo-Fenton reaction took place in the same conditions, although
transparent reactors were used. Light was provided by a solar simulator (Hanau, Suntest), with a detailed
description in de la Cruz et al., (De la Cruz et al. 2012). Light intensity was controlled and kept constant at
900 W/m2, by a Global and UV radiometer Kipp & Zonen (Models CM3 and CUV3, respectively).
2.2.4. Advanced Oxidation Processes specifics
2.2.4.1. UV-C and UV/H2O2 irradiation
A volume of 300 mL of the composite wastewater sample was introduced into each UV reactor and they
were exposed to UV-C irradiation during 10 min and 30 min, respectively. The pH was monitored and the
treated WW was stored at 4°C. For the UV/H2O2 treatment, hydrogen peroxide (30%) was added, reaching
an initial concentration of 25 mg H2O2/L in the reactor. The residual H2O2 was neutralized with sodium
bisulphite.
2.2.4.2. Solar irradiation, Fenton and photo-Fenton reaction
Wastewater samples contained in 100-mL brown bottles were treated with 25 mg H2O2/L and 5 mg Fe2+/L.
The iron source was FeSO4 •7H2O. Hydrogen peroxide dose was reached adding sufficient volume of 30%
H2O2 solution. WW samples contained in 100 mL Pyrex glass bottles were exposed to irradiation in the
Suntest solar simulator. For photo-Fenton, the same doses of H2O2 and Fe2+ used in Fenton experiments
were added. During the different treatment methods, pH, hydrogen peroxide and iron concentration
(when applicable) were monitored. Treated WW was stored then at 4°C until analysis.
Table 2.2 summarizes the treatment times and conditions of the AOP experiments. All experiments were
conducted with the MP content of the effluent WW (no spiking took place whatsoever). Assessment of
the MPs’ content before treatment was calculated as an average of 2 campaigns. Also, the results
concerning the MPs degradation (Figures 2.2 to 2.6) are a result of 4 campaigns, during which all
experiments were performed in duplicates, and each matrix (and AOP) was assessed in at least two
campaigns; the presented results are subject to approximately 5% standard error. The percentage results
58
were calculated with weighted arithmetic mean, rather than simple average of degradation %, according
to the following formula:
(2.1)
Where X% is the overall removal %, is the quantity of the pollutant (mol) and (i = 1 to 6) the removal
percentage of each MP. In this way, the quantity of the pollutants is taken into account in the calculations.
Table 2.2 – Summary of the advanced treatment methods applied.
Time
[min]
H2O2
[mg/L]
Fe2+
[mg/L]
UV-C irradiation 10, 30 - -
UV/H2O2 5, 10, 30 25 -
Solar irradiation 30, 60 - -
Fenton 60,120 25 5
photo-Fenton 30, 60 25 5
2.2.5. Physicochemical parameters
A pH meter (Mettler Toledo, GmbH) was used to measure pH values before and after each advanced
treatment method. A Perkin-Elmer UV/Vis Lambda 20 spectrophotometer was used in order to perform
the measurements of H2O2 at 410 nm (modified method: DIN 38 402 H15) and iron (Fe+2/+3) by the
Ferrozine method (De la Cruz et al. 2012). Calibration curves with respective WW effluents were made to
minimize spectral interferences. Total organic carbon (TOC) was measured by a Shimadzu TOC-V
CPH/CPN, while a digestion reactor and a spectrophotometer HACH DR/4000 were used to carry out the
COD measurements.
2.2.6. Analytical methods
For the MPs’ analysis, before and after the application of AOPs in lab scale, solid phase extraction,
followed by UPLC/MS-MS was employed. The analytical procedure applied is presented in detail in
previous works (De la Cruz et al. 2013, De la Cruz et al. 2012). In a summary, 300 mL of acidified samples
to pH=2.0 (32% hydrocloric acid) were filtered through 0.7 μm Whatmann glass fiber and spiked with 200
μL of a standard surrogate, containing the MPs in deuterated form. Solid Phase Extraction (SPE) was
performed automatically (GX-274 ASPEC, Gilson) onto Oasis HLB (200 mg, 6 mL) cartridges (Waters),
59
followed by nitrogen drying. After elution with methanol, the MPs were analyzed by UPLC/MS-MS
(Acquity Xevo-TQ, Waters). Multiple reaction monitoring mode with two transitions was used to detect
MPs and quantification was performed with internal standard calibration.
2.2.7. Secondary treatment systems specifications
The Vidy WWTP receives the municipal effluents from 16 different cities representing 220.000 inhabitants
and 40 million m3/year. It is composed mainly of a pre-treatment phase to separate suspended solids and
fats particles, followed by a primary decantation. Afterwards, the WW is mainly subjected to an aerobic
biological treatment followed by a sedimentation tank. The current secondary treatment consists of
activated sludge with a capacity of 1200 L.s-1. Finally, apart from the main line, the WWTP of Vidy accounts
with two secondary treatment installations: an MBBR and a coagulation-flocculation physicochemical
treatment.
2.2.7.1. Activated Sludge (AS)
It is the current biological treatment used at the WWTP of Vidy. The hydraulic retention time (HRT) is ~4
h and the sludge retention time (SRT) is ~2 days. The process does not include a nitrification step. It has a
reported MPs’ removal efficiency of 23%, as found by Margot et al. (Margot et al. 2011).
2.2.7.2. Moving Bed Bioreactor pilot plant (MBBR)
In this facility, MPs’ removal efficiency is about 44% which is higher than at activated sludge treatment
(Margot et al. 2013). The positive correlation among MP removal and nitrification could be attributed
either to the higher hydraulic residence time, or either to the higher microbial diversity of the nitrifying
bacteria; the latter have the ability to degrade many MPs, attributed to the co-metabolism due to the
ammonium monooxygenase enzyme (Fernandez-Fontaina et al. 2012). The treatment capacity is limited
to 5% compared to the AS unit.
2.2.7.3. Coagulation-Flocculation (CF)
This treatment method is based on chemical coagulation and flocculation processes in WW. The WWTP
of Vidy uses iron (III) chloride (FeCl3 - 40%) as coagulant agent.
2.3. Results
2.3.1. Initial conditions
After the three secondary treatment systems, the effluents recovered were found to differ in their
average physicochemical characteristics. Table 2.3 summarizes the main parameters controlled prior to
the application of advanced treatment. Among the three WW, the effluent of MBBR presents a series of
60
advantages. First of all, the pH is slightly lower than the AS and CF effluents. The organics content is
significantly lower as well, which can work as a precursor of the performance; since the AOPs rely heavily
on the HO● production, which non-selectively attack organics and MPs, less competition is provided for
the radicals produced. Alkalinity plays an important role, as it is an indicator of the (bi)carbonates content
of WW, and MBBR effluents contain 4 times less. Bi-carbonates are known to scavenge the hydroxyl
radicals, thus hampering the degradation efficiency (Carra et al. 2014). The suspended solids are
important for irradiation-based processes, since they cause shielding and pose a physical barrier between
the target and the photons. UV and solar irradiation are expected to perform very well both in AS and
MBBR effluents, since the difference is only 2 mg/L. Finally, the initial iron content in the effluents is an
indicator of the expected Fenton (side)reactions or the action as suspended solids, as far as UV light is
concerned; excess of iron, after a certain point can inflict an inverse effect, and pose a physical barrier in
the transmission of light within a wastewater sample (De la Cruz et al. 2013).
Table 2.3 – Initial physicochemical characteristics of the effluents of the different secondary treatment
units.
Parameter Unit
Wastewater previously treated with
Activated Sludge
Moving Bed Bioreactor
Coagulation Flocculation
pH - 7.8 7.4 7.9
TOC mg/L 37 20.2 57.2
COD mg/L 63 35 90
Alkalinity mg CaCO3/L 273 85 231
TSS mg/L 12 14 30
Total iron mg Fe/L 0.9 1.6 1.9
Comparing the three effluents, analysis has been performed to estimate the biodegradability of the
substances during the treatment in the different secondary treatment systems. Figure 2.1 shows the
evolution of the MP concentration during their presence in the WWTP. The treatment efficiency per
method was around: MBBR 40% > AS 25% > CF 20%, near to the values assessed by Margot et al. (Margot
et al. 2013). However, our estimation of removal percentage was approximated with 2 sampling
campaigns before treatment (Sampling point 1) and the average of 4 after the various secondary methods
(sampling points 2, 3 and 4), and was subject to (heavy) temporal variation for some substances (30-40%
difference).
61
Table 2.4 – Initial micropollutant concentration and limit of quantification (LOQ) for micropollutants in
the effluent of the different secondary treatment units.
Micropollutant (ng/L)
LOQ (ng/L)
AS (point 2) MBBR (point 3) CF (point 4)
[C] |Variation| [C] |Variation| [C] |Variation|
Carbamazepine 6 220 31 349 104 238 70
Diclofenac 18 1358 586 1254 328 1579 712
Metoprolol 6 579 134 793 166 855 317
Clarithromycin 6 490 132 363 52 479 153
Benzotriazole 14 4199 3633 7244 1566 7228 2366
Mecoprop 9 235 205 20 13 26 17
TOTAL* 7081 +4721 10023 -2230 10405 +3636
*The values in bold correspond to the values used for the experiments, the signed variation indicates the maximum value measured during the campaigns.
The 4 sampling campaigns results (at points 2, 3 and 4) on the initial MPs concentration are summarized
in Table 2.4. The MPs amount in the effluents of the three different secondary treatment methods slightly
differ from the estimation that derives from their removal efficiency during the secondary treatment
(described in Figure 2.1), because our (post-secondary)treatment experiments were conducted in
different sampling campaigns. Margot et al. (Margot et al. 2013) have mentioned the big variability of the
MPs content in the effluents, which makes the estimations complex. Also, AS presents a lower quantity,
due to the dependence of the average to Benzotriazole. In all cases, Benzotriazole consists of more than
50% of the monitored MP content. Hence, its variation highly influences the presented values. However,
it can be also attributed to high solubility in water (19800 mg/L) and low logkow (1.44); this specific
pollutant is very mobile in water and is not expected to sorb onto the sludge during treatment. Finally,
the total 6 MP content is on the order of 10 μg/L, at an average of 11, 10 and 13 μg/L, for AS, MBBR and
CF wastewater effluents, respectively. For micropollutant degradation in complex matrix such as
wastewater, this difference is not going to influence highly the results; if the initial COD and TOC contents
are considered, all the MPs monitored combined add up to 0.1% of the total organic load.
62
2.3.2. Efficacy of the various advanced oxidation processes
2.3.2.1. UV-C irradiation & UV/H2O2
The UV-C treatment method is based on direct photolysis of the persistent organic compounds by light
emitted at 254 nm. The main mechanism is the electronic excitation of the organic compounds, leading
to electron transfer from the excited state of the target compound to ground-state molecular oxygen or
homolysis to form organic radicals that react with oxygen (Legrini et al. 1993).
Figure 2.2 – UV treatment results. a) % degradation vs. time b) % COD & TOC reduction vs. time.
Figure 2.2a shows the removal efficiency of the 6 selected MPs at 10 min and 30 min of treatment, as well
as the evolution of COD and TOC (Figure 2.2b), for the three secondary treatment methods. After 10 min
of treatment, the removal efficiency was very similar, being 80, 85 and 79% for the AS, MBBR and CF
effluents, respectively. However, applying UV-C irradiation for 30 min, the three different effluents
demonstrated the following order of removal efficiency: Previously treated by MBBR (97%) > AS (93%) >
CF (92%).
Diclofenac and Mecoprop are already degraded 100% by UV-C irradiation alone, when the WW is treated
for a time as short as 10 min, for the three types of WW. This result verifies past evidence that these
compounds absorb well UV irradiation at 254 nm and can be easily photolyzed (De la Cruz et al. 2012).
Despite that Benzotriazole has shown low removal efficiencies against direct photolysis for pH > 7 in a
recent study (Bahnmüller et al. 2014), it showed relatively high efficiency in this case, achieving 100%
removal after 30 min of treatment. Furthermore, Clarithromycin showed a partial degradation after 30
min UV-C irradiation and only after MBBR treatment reached more than 80% removal. On the other hand,
Carbamazepine and Metoprolol remained below 80% removal after 30 min UV-C irradiation for the three
types of WW.
63
Finally, after 30 min of UV-C exposure, TOC was removed by 6.6%, 11.0% and 5.3%, while COD removal
rate was 47%, 71% and 27%, for the three types of WW (AS, MBBR, CF), respectively. The WW effluent
from Coagulation-Flocculation was the less favorable for organic compounds degradation.
Furthermore, UV/H2O2 is one of the most efficient AOPs, combining the immediate UV effect and the HO●
radicals produced from the homolytic disruption of H2O2. The initiation, propagation and termination
reactions involved are the following (Guo et al. 2013, Legrini et al. 1993):
2 ● (1.2)
● ● + (1.3)
● ● (1.4)
2 ● (1.5)
2 ● (1.6) ●+ ● (1.7)
After 5 min treatment, the order of MPs’ removal was the following: AS (99%) > MBBR (97%) > CF (96%).
After 10 min treatment, 100% removals of MPs removal was achieved, except for the WW previously
treated with CF, which showed 99% removal. 100% removal was already achieved in 30 min of exposure,
with the necessary time being calculated to 13 min. Figure 2.3a shows the removal efficiency for the 6
MPs at 5 min, 10min and 30 min of treatment, along with the COD and TOC removal (figure 2.3b) and the
remaining H2O2 content during treatment (Supplementary Figure S1).
Figure 2.3 – UV/H2O2 treatment results. a) % degradation vs. time. b) % COD & TOC reduction vs. time.
More specifically, Diclofenac and Mecoprop were 100% removed after 5 min of treatment. Benzotriazole
was also removed efficiently (over 80%) for the three types of WW. Clarithromycin was the only
compound not removed at 100% after 5 min treatment for the AS WW type. For the WW type
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corresponding to CF, even after 10min treatment, Carbamazepine and Metoprolol showed persistent
behavior reaching 73% and 95% removal, respectively. After 30 min treatment, all the selected MPs were
eliminated (figure 2.3a). Concerning the consumption of H2O2, a great reactivity is demonstrated.
Hydrogen peroxide is consumed almost at the same rate for the three different types of WW
(Supplementary Figure S1). After 30 min treatment, it was reduced almost completely (3 mg/L).
Concerning the global parameters, after 30 min treatment, TOC removal was 31.5%, %, 25.3% 12.0%,
while COD was removed ~100%, ~100% and 32% for AS, MBBR and CF effluents, respectively. The WW
types that were subjected to a previous secondary biological treatment reached higher TOC and COD
removal efficiency than the WW previously treated with CF. Finally, the two first types of WW achieved
almost 100% of COD removal; therefore, after 30 min UV/H2O2 treatment, extensive mineralization
process has started.
2.3.2.2. Solar irradiation, Fenton reagent and solar photo-Fenton treatment
Solar irradiation is anticipated to have the lowest impact against MPs, since the quantum yield of the
photons and the wavelengths reaching the organic compounds fall within less energetic bands of the light
spectrum. However, the experiments investigating effect of solar light were interesting, providing
information on the photo-transformation taking place in WWTPs and in natural waters, by indicating the
photo-sensible compounds. Figure 2.4a shows the MPs removal efficiency and 2.4b the COD and TOC
removal, respectively.
Figure 2.4 – Solar exposure results. a) % degradation vs. time b) % COD & TOC reduction vs. time.
After 60 min treatment, the order of removal efficiency was: MBBR (17%) > AS (11%) > CF (5%). Diclofenac
and Mecoprop had the most photo-sensible behavior; thus, they achieved more than 25% removal after
60 min treatment for the three types of WW. Carbamazepine, Metoprolol and Clarithromycin presented
65
more than 10% removal, except for the WW coming from the CF, where the Carbamazepine concentration
remained unchanged (0% removal). Benzotriazole was also very resistant to this treatment, and no
significant removal was found. Only the MBBR effluent demonstrated Benzotriazole removal (~15%).
Finally, as it was expected, the TOC and COD removal remained low after 60 min of solar exposure. After
60 min of simulated solar irradiation, TOC was removed of 9.5%, 3.7% and 5.1%, while COD decreased
18%, 21% and 11% for the three types of WW (AS, MBBR and CF), respectively.
The treatment by the Fenton reaction relies on the effect of the hydroxyl radicals produced by H2O2 and
Fe2+, and since this treatment is carried out in dark conditions, very slow regeneration of iron takes place
through the following reactions (Neyens and Baeyens 2003, Stasinakis 2008):
(1.8)
(1.9)
(1.10)
(2.2)
(limiting step) (2.3)
Figure 2.5 summarizes the MPs removal (2.5a), the H2O2 and iron concentration (Supplementary Figure
S2) along with the COD and TOC removal during the Fenton treatment (figure 2.5b). The fast oxidation of
Fe2+ to Fe3+ and the generation of a massive oxidative wave is followed by a steady Fenton cycle leading
to MP degradation. After 60 min of treatment, the order of removal efficiency was: MBBR (19%) > AS
(13%) > CF (3%), while after 120 min treatment, MPs removal of the WW coming from AS approached the
removal efficiency of the WW of MBBR, without significant increase in the CF water.
Figure 2.5 – Fenton process results. a) % degradation vs. time. b) % COD & TOC reduction vs. time.
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The most susceptible pollutant to treatment was Diclofenac, with 75% elimination rate in 2 h, followed by
Mecoprop (45%) and Carbamazepine (24%). Clarithromycin was almost unchanged (2% reduction), and
Benzotriazole and Metoprolol were mildly affected, demonstrating 12 and 15% reduction, respectively.
Despite that there is faster consumption of H2O2 for the WW effluents of AS and CF than for the one
resulting from MBBR, the MPs removal is higher in this last one (Supplementary Figure S2). This is mainly
attributed to the lowest pH among the others, acting beneficially as far as the Fenton process is
concerned, and the lower alkalinity of the MBBR WW type (85 mg CaCO3/L) compared to the one found
in the AS and CF WW (273 mg CaCO3/L and 231 mg CaCO3/L, respectively), since a lower bicarbonate
concentration was found. Iron concentration decreased accordingly to their initial pH. After 120 min of
treatment by the Fenton reaction, TOC removal was of 27.8%, 41.2%, and 16.0%, while COD decreased
27%, 83% and 19% for AS, MBBR and CF-treated WW, respectively.
Finally, the solar photo-Fenton has the advantageous synergistic action of light on the Fenton reaction,
regenerating Fe3+ back to Fe2+, thus limiting iron precipitation and enhancing further radical production,
through the following reaction (Pignatello et al. 2006):
(2.4)
Figure 2.6a shows the MP removal by the photo-Fenton reaction, 2.6b presents the COD and TOC removal
and the H2O2 and iron monitoring are present in Supplementary Figure S3. Although after 30 min the
removal efficiency is MBBR (21%) > AS (19%) > CF (7%), after 60 min treatment the difference increases,
the order of removal efficiency is: MBBR (31%) > AS (28%) > CF (11%).
Previous research, similarly to ours, has indicated the advantageous treatment against Metoprolol and
Carbamazepine (Klamerth et al. 2010, Prieto-Rodríguez et al. 2013). Diclofenac showed important
removal efficiency for the biologically pre-treated WW, while much lower removal efficiency for the one
coming from the CF treatment. Nevertheless, only Diclofenac achieved more than 80% removal for the
MBBR WW type. The rest of MPs were partially removed after 60 min treatment. Metoprolol,
Clarithromycin and Benzotriazole presented the lowest rate (less than 10% removal) for the CF WW type.
Concerning the organic matter, after 60 min of photo-Fenton treatment, TOC had removal efficiencies of
27.7%, 29.8%, 8.0%, while COD achieved removal efficiencies of 47%, ~100% and 10%, for the three types
of WW, respectively. H2O2 is consumed accordingly with the content of organic compounds (COD, TOC)
and the presence of inhibitors (carbonates and suspended solids) contained in each WW type. Dissolved
iron concentration remains almost constant during photo-Fenton treatment due to the Fe (II)
regeneration (Supplementary Figure S3).
67
The photo-Fenton treatment test was carried out during 60 min, and it could not reach the indicative 80%
MPs removal for any of the WW types. Consequently, it is suggested to extend the experiments residence
time until the removal goal is attained. However, if same degradation rates observed in the experiments
are followed, the estimated residence times would be: 116 min, 92 min and 185 min for AS, MBBR and CF
WW types, respectively. A summary of the degradation percentage per pollutant per process is given in
the Supplementary Material (Supplementary Figure S4).
Figure 2.6 – photo-Fenton process results. a) % degradation vs. time. b) % COD & TOC reduction vs.
time.
2.3.3. Degradation kinetics evaluation for the 6 different pollutants
The MPs chosen in this study were degraded by the different advanced treatment methods were fitted to
first-order degradation kinetics. Due to the limited sampling intervals these kinetics represent a common
ground for comparison only, described by the following equation:
(2.5)
or formulated as:
(2.6)
Table 2.5 summarizes the kinetic constants per AOP and (secondary) pre-treatment method. The
degradation rate constants k indicated by “nc” are the ones that could not be calculated due to the fact
that they were totally degraded before the minimal time span evaluated. For example, Diclofenac was
100% eliminated before 10 min of UV-C irradiation, or Mecoprop, which was also totally degraded before
5 min of UV/H2O2 treatment, for all three types of WW effluents. In addition, k values indicated by zero
represent the compounds that showed an insignificant (or not existent) removal. For example,
carbamazepine remained with the same initial concentration after 120 min of Fenton treatment for the
68
WW coming from CF. The degradation rate constants shown above are estimative values, and in order to
give more accurate kinetics, more and extended time spans (until complete degradation) should be
considered.
Regardless the type of WW analyzed, the order of degradation rates was the following:
Concerning the MP degradation, the degradation trends (the order indicates the increasing degradation
rate) and details on the Achilles’ heel of each pollutant are provided in the Supplementary Material
(Supplementary Table S1 and S2, respectively).
2.3.4. Evolution of the Average Oxidation State during the 5 different treatment processes
One of the most widely used parameters in WW degradability assessment is the Average Oxidation State
(AOS), which use the evolution of Total Organic Carbon (TOC) and Chemical Oxygen Demand (COD):
(2.7)
where COD and TOC values are expressed in mol O2/L and mol C/L, respectively. After each treatment
process, the following changes, summarized in Table 6, are observed.
As a common pattern, at the beginning of the highly oxidative process, the AOS increased rapidly, followed
by a stage when this increase decelerates, suggesting that the chemical nature of the intermediates
formed does not vary significantly. Nevertheless, the change of the AOS may not represent an important
impact on MPs removal, because MPs only represent a small part of the total organic compounds
contained in the WW (De la Cruz et al. 2012). In this study, only ~10 μg/L of the total organic load are the
6 MPs. Therefore, the degree of MP elimination is correlated with the change in AOS in treated WW. Since
the COD and TOC of a WW are relatively easy parameters to monitor, the AOS will predict the elimination
of the MPs.
Table 2.5 – Degradation kinetics of the 6 different pollutants during treatment in the different
effluents and treatment methods.
Degradation constant UV UV/H2O2
k (min-1) AS MBBR CF AS MBBR CF
Carbamazepine 0.027 0.046 0.021 nc 0.644 0.131
Diclofenac nc nc nc nc nc nc
Metoprolol 0.032 0.048 0.034 nc 0.599 0.3
69
Clarithromycin 0.035 0.061 0.024 0.563 0.354 0.277
Benzotriazole 0.23 0.281 0.204 nc 0.701 0.921
Mecoprop nc nc nc nc nc nc
Degradation constant Solar Fenton photo-Fenton
k (min-1) AS MBBR CF AS MBBR CF AS MBBR CF
Carbamazepine 0.004 0.003 0 0.004 0.002 0 0.006 0.01 0.007
Diclofenac 0.005 0.008 0.005 0.005 0.012 0.001 0.021 0.071 0.011
Metoprolol 0.003 0.001 0.002 0.001 0.001 0 0.003 0.01 0.001
Clarithromycin 0.001 0.003 0.002 0.001 0 0 0.002 0.003 0
Benzotriazole 0.001 0.003 0 0.001 0.001 0 0.003 0.003 0.001
Mecoprop 0.005 0.009 0.004 0.004 0.005 0.002 0.009 0.008 0.004
As a first step, the percentage of AOS change during treatment was calculated. The values are summarized
in Table 2.6. Afterwards, the correlation among the percentage of MP degradation per treatment method
(for all effluents) was estimated. The Pearson test was used to detect the correlation between the two
parameters, and the P-value indicating the verification of the hypothesis (that the parameters are
correlated) within the 95% confidence interval. The Pearson correlation values showing mild correlation
are among 0.6 and 0.8, while values among 0.8 and 1 indicate strong correlation among the parameters.
The accepted P-values are lower than 0.05.
Table 2.6 – Evolution of the Average Oxidation State (AOS) during treatment by the various methods
in the different effluents.
UV AS MBBR CF UV/H2O2 AS MBBR CF
0 min 1.45 1.4 1.64 0 min 1.45 1.4 1.64
10 min 1.8 1.95 1.75 10 min 3.43 2.16 2.16
30 min 2.55 3.17 2.18 30 min 4 4 2.18
Solar AS MBBR CF Fenton AS MBBR CF photo-
Fenton AS MBBR CF
0 min 1.45 1.4 1.64 0 min 1.45 1.4 1.64 0 min 1.45 1.4 1.64
30 min 1.48 1.58 1.75 60 min 1.6 1.77 1.66 30 min 1.96 1.6 1.65
60 min 1.51 1.86 1.79 120 min 1.77 2.36 1.71 60 min 2.14 ~4 1.67
70
As Table 2.7 indicates, there is correlation between the MP removal and the AOS, and is within acceptable
rates in the majority of the cases. For UV/H2O2, the fast kinetics pose difficulties in the calculation, since
100% removal is easily achieved; if none or up to 2 values corresponding to 100% efficiency are inserted
in the calculations, then the correlation can increase up to 0.949, while the corresponding P-value drops
to 0.014. Nevertheless, the AOS can offer, under conditions, a predictive value on the fate of MPs during
treatment. The total organic load is correlated with the concentration of the MPs, so the main effort will
be now focused on explaining its degradation pathways, according to the AOP applied.
Table 2.7 – AOS percentile change and correlation with % of degradation.
UV % 0 min % 10 min % 30 min Pearson Correlation
AS 0 59 80 0.819
MBBR 0 62 89 P-Value
CF 0 57 77 0.024
UV/H2O2 % 0 min % 5 min % 10 min Pearson Correlation
AS 0 99 100 0.665-0.949
MBBR 0 95 100 P-Value
CF 0 84 95 0.103-0.014
Solar % 0 min % 30 min % 60 min Pearson Correlation
AS 0 8 17 0.766
MBBR 0 11 22 P-Value
CF 0 5 11 0.045
Fenton % 0 min % 60 min % 120 min Pearson Correlation
AS 0 16 26 0.822
MBBR 0 23 29 P-Value
CF 0 4 7 0.023
photo-Fenton % 0 min % 30 min % 60 min Pearson Correlation
AS 0 20 32 0.819
MBBR 0 27 44 P-Value
CF 0 12 19 0.871
71
2.4. Discussion
2.4.1. Degradation of micropollutants in wastewater: characteristics, influence and role of
the Effluent Organic Matter
In order to further elucidate the mechanism of MPs and organics’ degradation by the various processes
involved in this work, the contribution of the organic matter present must be evaluated, since significant
removal of Effluent Organic Matter (EfOM) (and therefore, reduction in COD and TOC) has been found in
the previous section.
The composition of EfOM was recently reviewed by Michael-Kordatou et al., (Michael-Kordatou et al.
2015) and its main substances are organic contaminants, other non-degradable compounds, or products
of the biological treatment (Lee et al. 2013). One part of the EfOM contained is attributed to refractory
compounds (Barker and Stuckey 1999, Jarusutthirak and Amy 2007). Humic-like materials are found, and
their presence is linked with their existence in drinking water sources (Jarusutthirak and Amy 2007) or
their transfer through the non-separating WW collection systems. The EfOM also contains a series of
substances linked with the biological activity of the microorganisms, known as soluble extracellular
polymeric substances (EPS) and soluble microbial products (SMP). These substances are usually a product
of i) microbial metabolism or ii) released during cell degradation (lysis) (Barker and Stuckey 1999,
Jarusutthirak and Amy 2007). Some characteristics related to these substances are their specific UV
absorbance index (SUVA: UV absorbance/DOC) which is an indication of their humic behavior
(Jarusutthirak and Amy 2007) but more importantly, they form the majority of the COD of aerobic
effluents.
However, during physicochemical treatment, i.e. CF in our case, the EPS and SMP fraction is expected to
be less important, since the bigger organic molecules are expected to prevail. Decrease of the negatively
charged colloidal particles is expected in high rates (Shon et al. 2006), but no significant transformation
due to the addition of the coagulants. The removal of the flocs by settling is involved instead.
Nevertheless, the original sources of humic substances (i.e. at least from drinking water) are expected to
exist; this indicates some common reaction pathways involved in water and wastewaters, which will be
further analyzed later.
From the observations above, a differentiation can be made in the EfOM, compared with the organic
matter present in natural waters (NOM). Wastewater contains sensitizers not encountered or found in
lesser amounts in natural waters (Ryan et al. 2011). In EfOM, among others, these substances are
expected to participate in the active fraction during the photochemical reactions and the advanced
oxidation processes applied, while the rest of the organic matter plays the role of the target. Literature
72
does not indicate any participation of the EPS or SMP in the photochemical reactions that resembles the
NOM action mode and therefore we make the previous working hypothesis. Under this condition, the
removal of the MPs, compared to the amount of carbon eliminated by this effect is merely a side reaction,
and will be treated as such; the MP degradation is in fact facilitated by the organic load reduction within
the matrix.
2.4.2. Pathways of MP degradation in secondary effluent
At this point, we separate the UV-based and the solar/Fenton processes and examine the degradation
pathways separately. An accompanying overview of the mechanism is presented in Figure 2.7.
2.4.2.1. MP degradation by UVC-based processes
In principle, the effect of UV-C irradiation at 254 nm can be separated in two major categories, the direct
and the indirect pathway.
1. Direct UV-C photolysis: the direct action of UV-C light on OM in wastewater. If we consider a
sample receiving UV-C irradiation, theoretically the EfOM plays the role of screening filter, but
experimental proof accounted a 10% decrease due to this effect (Ryan et al. 2011). Literature suggests
that the application of solar UV light exerts fragmentation of large conjugated compounds in smaller,
lower molecular weight ones (Parkinson et al. 2001); we expect that this phenomenon is taking place in a
certain extent under UV-C irradiation as well. These targets can be either the MPs (action 1) that present
UV-absorption peaks near the emitted wavelengths (small contribution in the total DOC), as well as the
ESP and SMP contained in WW (action 2). The action of UV against proteins, lipids and sugars involves
protein degradation and lipid peroxidation (Nasibi and Kalantari 2005), protein carboxylation (Krisko and
Radman 2010) etc. Also, the direct effect on humic acids is to be considered (action 3), causing their
polymerization and dissociation of covalent bonds present in the molecule (Sławińska et al. 2002). The
production of free organic radicals (action 4) and electrons (actions 5a&b) can also initiate indirect
mechanisms. As a matter of fact, the direct UV-C effect is never acting alone, but carries with it all the
indirect pathways, further analyzed afterwards; this also explains not only the parent MP elimination, but
also the mineralization taking place during sole UV-C treatment.
2. Indirect UV-C photolysis: the action of excited compounds against the same targets. It has been
reported that UV can electronically excite the photosensitizing molecules (probably in triplet state) and,
in presence of oxygen, cause photolysis through electron transfer to molecular oxygen (action 6) or to
form organic radicals (action 7), which then will react with oxygen (Legrini et al. 1993). Important
parameters that are involved in this pathway are the presence of oxygen (aerobic conditions), the specific
UV absorbance (SUVA) and the ratio of absorbance at 254 to 365 nm (Sharpless et al. 2014).
73
2.i. The energy transfer to oxygen causes the formation of (more commonly found as )
which is responsible for interference to activated double bonds and facilitate electron transfer. By itself,
it reacts with lipids, proteins and acids, as well as other cellular targets. By one-electron transfer, the
creation of superoxide radicals is induced (action 8), and since it is a relatively weak oxidant, its
participation is expected to contribute lightly in redox reactions with metals, such as iron or copper
(Buettner 2013). In turn, these can initiate Fenton-like reactions in presence of H2O2 (which will be further
analyzed later).
2. ii. By two-electron transfer (action 9), and/or the participation of superoxide radicals and water,
H2O2 can be generated (Buettner 2013). In organic-free waters, no H2O2 is accumulated, but in WW, there
was a constant presence of H2O2 in the bulk (Buchanan et al. 2006). The simultaneous presence of H2O2
and dissolved iron in our WW induces the initiation of a Fenton reaction. Also, the dissociation of H2O2
causes further hydroxyl radical production and elimination of the organic content in the bulk, as it has
been suggested before (De la Cruz et al. 2012).
The mineralization extent observed by UV-C alone was limited to 10%. However, if hydrogen peroxide is
added into the bulk from the beginning, the equilibrium and the importance of these pathways is limited,
since the homolytic disruption of the HO-OH bond in H2O2 (action 10) induces the production of the highly
oxidative hydroxyl radical (HO●) (De la Cruz et al. 2013). The hydroxyl radical non-selectively attacks the
organic matter present in the solution, actively eliminating the COD and increasing the TOC removal up
to 30%, from 10% which was before. Finally, if H2O2 is present, as in all of our matrices (from 0.9 to 1.9
ppm), taking into account the iron in complexes present in the effluents, Fenton reaction can work in
parallel, further inducing the radical generation and the subsequent organic matter removal (from 60-
70% to almost 100% COD removal).
2.4.2.2. MP degradation by solar, Fenton and (solar) photo-Fenton processes.
The three processes of solar exposure, Fenton and photo-Fenton are inter-connected, with the action of
solar light alone proposed as a possible basis to facilitate the degradation of EfOM due to the other two
processes as well. Solar light has been long identified to initiate photochemical reactions, in presence of
NOM (Canonica 2007). Since EfOM contains a part of NOM, NOM-like substances or substances with high
SUVA values (as index of humic-containing waters), the action mode of light in natural waters is
extrapolated in our WW effluents.
Compared to UV-C light, the direct effects of solar light (UVA and UVB) on MPs and EfOM are relatively
limited (action i). However, this contribution is in order of some ng/L carbon elimination, does not take
place with all pollutants and therefore could be neglected. This contribution in the degradation of MPs
involves their excitation to singlet-excited state, and through intersystem crossing, to triplet state (Ryan
74
et al. 2011). After this point, the MP can either form products through side reactions or reacts with oxygen,
returning to ground state.
To explain the high mineralization percent in our experiments, we will extrapolate the reaction taking
place in natural water towards our effluents. In natural waters, there is considerable photosensitization
of the organic matter, or more specifically, humic, fulvic acids and other substances (action ii). The
substances involved in this process are either autochthonous or allochthonous, comprising the
chromophoric dissolved organic matter (CDOM), which is mainly responsible of participating in indirect
photoreactions (Canonica 2007). In a lesser extent, the light absorption leads to mineralization of the OM
to inorganic compounds, due to a direct pathway involving its disintegration to smaller constituents (Gao
and Zepp 1998). The main reaction pathway includes the excitation of OM and as an end-product, the
reactive transients participate in energy and electron transfer, as well as free radical reactions (Gao and
Zepp 1998).
The main transient products of the photosensitization are the HO●, ●CO3, 1O2 and triplet states of DOM
(3DOM*) (Vione et al. 2014). The production of 1O2 is associated with the photosensitizing ability of DOM
(Mostafa and Rosario-Ortiz 2013). The action of the singlet oxygen was analytically presented before (now
action iii) and now only the HO● contribution will be now assessed further. The humic and fulvic fraction
of the DOM is producing HO●, as it absorbs light better than the smaller compounds and some of their
triplet states are able to oxidize superoxide or hydroperoxyl to hydroxyl radicals (Vione et al. 2014). All
transient species undergo various pathways afterwards, including the reaction with natural organic
matter, (bi)carbonates, dissolved oxygen and more (Vione et al. 2014).
Extrapolating to the WW in our experiments, since EfOM is a combination of autochthonous (bacterial
metabolism related) and allochthonous organic matter (humic/fulvic acids of drinking water) a similar
behavior is expected (Ryan et al. 2011). The active part EfOM is excited to a triplet state from where it can
react with dissolved compounds by energy/electron or hydrogen transfer (Vione et al. 2014), with the
targets stated before, and return to ground state or react with oxygen and follow a pathway similar to the
one of natural organic matter (Ryan et al. 2011). The low-molecular weight fractions are the ones mostly
responsible for generating the hydroxyl radical as well as the humic fraction, because of their
chromophoric abilities (Lee et al. 2013, Vione et al. 2014). Also, compared to natural waters, WW with
same DOC levels have been suggested to produce hydroxyl radicals more efficiently (Ryan et al. 2011);
higher energy triplet sensitizers may increase the ability of energy/electron transfer than the respective
NOM-induced ones. Consequently, the HO● produced (action iv) are added to double bonds or to aromatic
compounds, abstract H+ or cause electron transfer (Wenk et al. 2011).
75
Other routes that are responsible for generating ROS in WW include H2O2-dependent systems, which
demonstrate Fenton-like behavior (Vione et al. 2014). The contribution of these reactions can be
considered in our work, when H2O2 is added to the system; (organically complexed) iron is already present
and for the Fenton experiments an additional 2.5 mg/L Fe (II) was added to the system. In natural systems,
the presence of iron is known to catalyze the oxidation of organic matter, as well as participate in the
production of reactive transient species (action v) (H2O2, HO●, HO2/O2●─) (Voelker et al. 1997); our reagents
addition ensures the Fenton reaction in the system in the most readily available form. Here, in an analogy
with the natural system, light is catalyzing the ligand-to-metal charge transfer in the Fe-EfOM system,
forming iron (II) and polycarboxylate radicals, which in turn create free radical intermediates (action vi)
(Voelker et al. 1997). At this pH, the contribution of the heterogeneous Fenton system of the solid iron
oxides has to be mentioned, but its action is neglected when compared with the homogeneous system.
Finally, the last possible pathway of radicals’ formation in our system is through the participation of
nitrites (in lesser extent) and nitrates contained in WW (action vii). Their presence is correlated with the
denitrification step after the MBBR, and their contribution to HO● formation should not be overlooked,
and their presence has been suggested as crucial when comparing the radicals’ production between
natural water and WW (Lee et al. 2013, Ryan et al. 2011, Vione et al. 2014). In WW, as in nature, the
concentration of nitrites is less significant than nitrates, but their quantum yield is higher (Vione et al.
2014). The comparison among the AS and the MBBR WW reveals similar levels of nitrites (0.2-0.3 mg N/L),
but the main radical producer, NO3 is 15.3 mg N-NO3/L in MBBR waters compared to 2.3 mg N-NO3/L in
AS effluents (Margot et al. 2011).
The effect and the intensity of the various effects is visible in Figures 2.2-2.6 (b), by the modification of
COD and TOC. The difference among our treated WW types lies in the difference in their physicochemical
features and composition. Firstly, there are physical characteristics that hinder the degradation process,
such as suspended solids, the pH and the alkalinity. Most of the unfavorable conditions are met in CF WW
(higher pH and suspended solids); the extra iron present cannot compensate with the action induced by
the parallel Fenton reaction. Secondly, the organic matter present in CF effluent is 1.5-2 times higher than
the respective aerobic processes and in less favorable forms, when it comes to sensitization, since the
colloids (and other low-molecular weight substances) have been removed. The EfOM present in this WW
forms a significant filter as well as causes self-scavenging of the reactive species produced (Ortega-Gómez
et al. 2014). Nevertheless, in absolute values, the carbon elimination was significant, as the percentage
was lower but the initial value was much higher than the aerobically treated WW; as it seems, the indirect
pathways are enhanced by the presence of EfOM, due to the similar photo-sensible content but the higher
target availability in CF water. The contribution of solar light alone is worth mentioning, as well as the one
induced by UV-C. There is almost 10% mineralization in both cases, strengthening the significance of the
76
multi-level solar light-induced reactions in WW, while adding the Fenton reagents lead to
complementarily increased radicals production in all the systems.
Figure 2.7 – Overall mechanistic interpretation for the action of UVC and solar light within the effluent
wastewater (adapted from (De la Cruz et al. 2012)).
2.5. Conclusions
The unambiguous necessity to adopt advanced treatment methods in municipal WWTPs in order to tackle
the MP issue was addressed by the implementation of 5 treatment techniques. High MP removal was
thereby achieved. In addition, the reduction of EfOM was identified as the main mechanism of organics
removal.
Regardless the type of advanced treatment applied, a previous biological treatment stage (AS or MBBR)
seemed to be more appropriate than a physicochemical one (CF). Moreover, the MBBR effluents had
better physicochemical characteristics (lower alkalinity, TSS, COD and TOC concentration), rendering the
water matrix more suitable to apply a further advanced treatment.
From the five different treatment methods applied: UV-C irradiation, UV/H2O2, solar irradiation, Fenton
reaction, and photo-Fenton, only the UV-based methods removed 80% of the selected MPs, for the times
spans tested. Furthermore, after 30 min treatment, the degree of oxidation was very high in terms of COD
and TOC removal. Thus, high levels of mineralization of the organic compounds could be achieved with
this technique. For the case of solar light, Fenton and photo-Fenton treatment methods, the degradation
EfOM
3PhOM*
PhOM •-
O2
1O2Fe3+-EfOM
EfOM • ox
O2-• /HO2
•
HH2HH2OOOO2
• OH
• OHEfOM
EfOMox
OxOM & MP
OxOM & MP
MP MPmod
(i)
(ii)
(iv)
(vi)
(iii)
(v)+H+
OxOM ox
O2
Fe2+-EfOM
EfOM
UV-C
R•
ROO•
O2OxOM & MP
OxOM ox
UV-C
UV-C
Abbreviations
EfOM: Effluent Organic
Matter
PhOM: Photo-sensitizablefraction of EfOM
OxOM: Oxidizable fraction
of EfOM
MP: Micropollutant
(i)-(vii): solar-induced
pathways
(1)-(10): UVC-induced
pathways
(5a)
(4)
(1)
(5b)
PhOMmod
OxOMmod
PhOM
(2)
(3)
(6)
(6)
(7)
(8)
(9)
(10)(10)
(10)
(ii)
(ii)
OxOM
(vii)
NO2/NO3
OxOM ox
(iii)
77
rates are slower. The photo-Fenton treatment has slower MPs’ degradation rates than the UV-based
treatment methods. However, solar-based processes achieved a (small) degree of overall organics
removal which is not negligible at all. Extending the residence times in future studies is suggested, in order
to verify their efficiency to remove the 80% of MPs. In general, the order of degradation rates was the
following:
This study presented an overview of the impact of different advanced treatment methods, coupled to
three different previous secondary treatment techniques. Promising results were gathered from the
fifteen different combinations assessed for the removal of the selected MPs and the EfOM. Nevertheless,
further studies should be carried out in order to optimize these processes; the main issues are located in
reducing residence time, changing H2O2 dose and feeding method, for the UV/H2O2 methods, and
changing Fenton’s Reagent ratio or extending the treatment time for the photo-Fenton treatment.
79
3. Chapter 3 - Micropollutant degradation, bacterial
inactivation and regrowth risk in wastewater effluents:
influence of the secondary (pre)treatment on the efficiency
of Advanced Oxidation Processes
Published work:
Stefanos Giannakis, Margaux Voumard, Dominique Grandjean, Anoys Magnet, Luiz Felippe De Alencastro,
and César Pulgarin. "Micropollutant degradation, bacterial inactivation and regrowth risk in wastewater
effluents: Influence of the secondary (pre) treatment on the efficiency of Advanced Oxidation
Processes." Water Research 102 (2016): 505-515.
Web link:
http://www.sciencedirect.com/science/article/pii/S0043135416305048
Supplementary material:
Appendix B
Doctoral Candidate’s contribution:
Main investigator and author.
80
3.1. Introduction
Throughout the years, urban wastewater treatment plants (WWTPs) have implemented strategies to
eliminate the organic load, chronologically followed by the inorganic one (phosphorus and nitrogen), and
presently, the current average treatment stops at the disinfection level. Chlorination was until some time
ago the most common disinfection method. However, its use has been connected with trihalomethane
(THM) production, a harmful disinfection by-product (DBP) of the reaction with organic matter (Krasner
et al. 2009). Hence, treatment at disinfection and decontamination level was turned towards safer
“greener” techniques (Michael et al. 2012).
Lately, ozone and ultraviolet light have been widely employed to tackle the issue of microorganism
elimination in wastewater (Drinan and Spellman 2012). UVC alone, combination with H2O2 and/or O3 are
some of the most studied and well-understood Advanced Oxidation Processes (AOPs) for this purpose.
The UVC-based processes have a well-established disinfection efficiency when applied in secondary
wastewater effluents (Rodríguez-Chueca et al. 2015), but the main concern of bacterial regrowth is yet to
be resolved. In overall, the AOPs gained supporters during the last two decades, mainly for their non-
selective character against organic matter and microorganisms (Moncayo-Lasso et al. 2012). However,
despite the interest gain, the limited number of full-scale applications engulfs the danger of over- or mal-
dimensioning of such units, since the pre-treatment process differs from plant to plant.
On the other hand, in less wealthy countries of the developing world, ozone and UV-based techniques are
far from applicable. Instead, the use of solar ponds has been widely applied (Von Sperling 2005), as a
simple, and quite efficient method of treating wastewater effluents. As this process has been successfully
applied, enhancing its performance with the photo-Fenton reagents could significantly increase the
removal of microbial and organic loads (Moncayo-Lasso et al. 2012). Iron and H2O2 are abundant and
environmentally safe, respectively, and the inactivation potential of photo-Fenton can improve the
effluent quality while reducing the residence times in such configurations (Von Sperling 2005) or in
Raceway Pond Reactors (RPRs) (Rivas et al. 2015).
In Switzerland, although special effort has been made to effectively remove (Giannakis et al. 2015c,
Margot et al. 2013, Margot et al. 2011), the recommended strategies have not included the
microorganism risk in the design, neither in the legislation. The upgrade of wastewater treatment plants
(WWTPs) affects the >10.000 inhabitant equivalent, thus leaving a large number of WWTPs without
disinfection units. For instance, the WWTP of Vidy (Lausanne, Switzerland) in its current reconstruction
planning, which focuses on the micropollutant removal after the secondary treatment of wastewater
(WW), involves the use of activated carbon, ozonation, followed by UVC light, but mostly for degrading
the by-products of the previous two installations.
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In this work, we take advantage of the simultaneous presence of 3 parallel secondary treatment systems
of wastewater treatment in the plant of Vidy, in order to study the effect of secondary pretreatment on
the efficiency of AOPs. More specifically, wastewater from Activated Sludge, Moving Bed Bioreactors and
Coagulation-Flocculation units (with primary wastewater effluent as control) has been subjected to
various oxidation methods. The UVC alone, UVC/H2O2, Fenton, solar light and (solar) photo-Fenton
processes (namely UV-based and Fenton-related processes) were tested on the (immediate) bactericidal
removal efficiency, as well as the post-treatment regrowth. Finally, to put things into the real wastewater
context, the evolution of 8 micropollutants were monitored, and insights were given on the comparative
order of removal of micropollutants (MPs) and microorganism (MO) regrowth risks.
3.2. Materials and Methods
3.2.1. Collection of wastewater samples and treatment plant specifications
For the needs of the microbial testing, 6 sampling campaigns were performed. During each visit,
wastewater from the following points was collected: i) before secondary treatment (after primary
decantation) (PT), ii) after secondary treatment by activated sludge and secondary clarification (AS), iii)
after secondary treatment by moving bed bioreactors (MBBR) and iv) after physicochemical treatment by
coagulation-flocculation (CF). The aforementioned points can be found in Figure 3.1. Each time, a 5-L grab
sample was collected and transported immediately to the laboratory for treatment. For the
micropollutants, the strategy has been analyzed in a previous work (Giannakis et al. 2015c).
Figure 3.1 – Schematic representation of the WWTP of Vidy, Lausanne (VD, Switzerland) and the
sampling points for this research.
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The AS unit has a hydraulic retention time (HRT) of 4h and sludge retention time (SRT) of 2 days,
approximately, without nitrification. The MBBR capacity is only 5% compared to the AS unit, but has a
longer retention time and includes a nitrification step. Finally the CF unit is based on chemical coagulation
and flocculation process by FeCl3 as coagulant. More details on the different units can be found in Margot
et al. (Margot et al. 2013).
3.2.2. Employed chemicals and reagents
For the experiments of bacterial inactivation H2O2 30%, FeSO4.7H2O and Titanium (IV) oxysulfate (for H2O2
determination) was acquired from Sigma-Aldrich (Switzerland) and NaHSO3 for H2O2 elimination from
Sigma-Aldrich and Acros Organics, respectively. Finally, the plate count agar (PCA) was purchased from
Sigma-Aldrich (Switzerland).
3.2.3. Experimental set-up: reactors and apparatus
The experiments are divided in two main groups, namely the UV-based and the Fenton-related ones. For
the UV-based experiments, two double-wall, water-jacketed merry-go-round reactors were used in
parallel, for the UVC and UVC/H2O2 experiments, respectively. The water recirculating in the glass reactors
was controlled at 22°C (for protection of the UVC equipment). UVC light was provided by 35-W low
pressure UVC lamps (Model: UVI 40 4C P 15/300), with an emission of 350 μW/cm2, acquired from UV-
Technik Speziallampen (see Supplementary Figure S1 for the reactor scheme). Among the Fenton-related
experiments, the solar only and solar-assisted photo-Fenton process were performed in 100-mL Pyrex
glass reactors, placed on magnetic stirrers and constantly agitated by magnetic bars (300 rpm). The Fenton
experiment took place in shaded reactors, in the dark, whereas the solar and the photo-Fenton
experiments took place in a solar simulator (Atlas, Suntest CPS+). This artificial solar light source was set
at 900 W/m2 global irradiance (~0.5% UVB, ~5% UVA and ~95% visible light) and has been analytically
presented in previous works, e.g (Giannakis et al. 2015b). The solar UV intensity and global irradiance was
monitored with a coupled CM3 – CUV3 UV radiometer and pyranometer (Kipp & Zonen, Netherlands).
3.2.4. Application of AOPs: details and specifications
A summary of the conditions is given in Supplementary Table S1, regarding the experimental times and
reagents addition. For each group of experiments, an analytical presentation follows.
3.2.4.1. UV-based experiments
For the sole UVC experiments, 300 mL of wastewater were added in the reactors and exposed to the
irradiation. In the case of UVC/H2O2 experiments, H2O2 was also added from a stock solution to reach the
desired initial H2O2 amount. The pH was monitored and the samples were immediately analyzed. Samples
were also kept in order to assess bacterial regrowth after the experiments.
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3.2.4.2. Fenton-related experiments
For the solar tests, 100 mL of wastewater were inserted in the reactors and placed in the Suntest for
simulation of solar exposure. The temperature of the water never exceeded 35°C. The remaining tests
were performed with the addition of Fe2+ and H2O2, either in the dark (Fenton experiments) or under light
in similar conditions (photo-Fenton experiments). In all cases, samples were also kept for regrowth tests.
3.2.5. Analytical methods, physicochemical and microbiological parameters
3.2.5.1. Analytical methods
The micropollutants presence in wastewater was followed by a UPLC/MS-MS method, used in previous
works (De la Cruz et al. 2013, De la Cruz et al. 2012) and analytically presented in (Giannakis et al. 2015c).
The removal percentage of the 8 micropollutants monitored in this study (Carbamazepine, Diclofenac,
Atenolol, Metoprolol, Venlafaxine, Clarithromycin, Benzotriazole and Mecoprop) was calculated by
weighted arithmetic mean, as follows:
(3.1)
In the graphs, the overall removal X% is given, wi is the micropollutant amount (mol) and xi the removal
percentage of each micropollutant (xi: i=1-8). Finally, we note that the work was effectuated by the
inherent micropollutant content of the collected wastewater; no spiking took place prior to testing.
3.2.5.2. Physicochemical parameters
For the pH monitoring throughout the experiments a Mettler Toledo pH meter was used. A UV-vis Lamda
20 spectrophotometer was used to monitor the evolution of H2O2, followed by the (modified) DIN method
38 402 H15 and the dissolved iron by the Ferrozine method (De la Cruz et al. 2012). The principal
physicochemical characteristics of the wastewater used in this work are summarized in Table 3.1.
Table 3.1 – Basic physicochemical and optical characteristics of the wastewater used in this study
(own measurements and (aMargot et al. 2013, bMargot et al. 2011)).
Parameter Unit Wastewater previously treated with Primary Activated Moving Bed Coagulation
Treatment Sludge Bioreactor Flocculation pH - 7.8-8 7.3-7.8 6.6-7.4 7.3-7.9
TOC mg/L 109.1±25.6 28.08±12.62 14.615±7.9 68.47±15.94 DOC (0.45μm) mg/L 89.32±26.42 20.40±1.41 6.39±1.71 29.98±0.88
COD mg/L 200±19 51±10 20±11 85±5 Alkalinity mg CaCO3/L 282.5±15 230±35 95±10 240±10
TSSa,b mg/L 35±10.4 12.1±2.8 14.2±1.4 28.5±5.7 Total Solidsa,b mg/L 59.5±5.4 54.6±4.1 25.5±4.3 58.2±3.3
Total iron mg Fe/L 2.5±0.55 0.95±0.05 1.75±0.15 5.5±1
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Dissolved iron mg Fe/L 0.25±0.05 0.04±0.002 0.02±0.001 0.33±0.06 UVAT % 37.78±5.78 87.58±4.95 86.10±5.51 62.22±7.09 UVBT % 22.45±3.32 75.77±2.24 74.07±1.57 44.45±4.09 UVCT % 11.42±0.97 65.59±2.34 67.47±3.23 31.27±6.55
3.2.5.3. Microbiological parameters
The microbial content of wastewater was monitored by cultivation on a non-selective agar (PCA). This
medium allows the enumeration of E. coli, Bacillus subtilis, Listeria monocytogenes, Staphylococcus
aureus and other bacteria contained in water and dairy matrices. The microorganism recovery rate, after
24h incubation at 35°C, is above 70% for a 1.000-100.000 inoculum (initial population). In such manner,
the disinfecting capabilities of the AOPs tested shall not be limited by selectivity on the medium and our
estimation will have the minimum error possible, given the particularities of the cultivation techniques
for inactivation estimation (Michael et al. 2012). The initial CFU/mL in the working matrices was 6.5x105,
6.5x103, 3.5x103 and 4x105, for PT, AS, MBBR and CF, respectively. No microorganisms were spiked in the
wastewater samples; the work was realized by the indigenous population. Samples were drawn at the
respective points (~ 5 mL) and were plated immediately. Appropriate dilutions were done, to achieve 15-
150 colonies per plate. Experiments were done in duplicates, in the different sample campaigns and at
least double plating was performed, enumerating 3 consecutive dilutions. Therefore, the average value is
presented in all the figures, subjected to <5% (max. 10% in few cases) standard deviation; measurements
with higher errors were not considered and error bars are not shown for clarity.
3.3. Results
3.3.1. Micropollutant elimination in the selected wastewater effluents
Figure 3.2 summarizes the degradation of the 8 selected organic micropollutants present in the effluents
of the secondary treatment facilities in the WWTP of Vidy. All the selected AOPs were tested (UVC,
UVC/H2O2, Solar, Fenton, photo-Fenton) against 8 MPs in WW (Carbamazepine, Diclofenac, Atenolol,
Metoprolol, Venlafaxine, Clarithromycin, Benzotriazole, Mecoprop), after treatment by AS, MBBR or CF.
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Figure 3.2 – Micropollutants’ degradation by AOPs after secondary treatment. a) UV and UV/H2O2
processes. b) Fenton, solar and photo-Fenton process. AS: blue trace, MBBR: red trace, CF: green trace.
Continuous lines and colored symbols show the measured evolution of the experiment, while the
dashed lines and open symbols indicate the projection of the experiment according to the measured
first order degradation rate constant.
In a previous study with 6 micropollutants, we have correlated the degradation of micropollutants with
the pretreatment method and the subsequent AOP (Giannakis et al. 2015c) with an order of increasing
efficiency of CF < AS < MBBR, for the pre-treatment methods and k (UV) < k (UV/H2O2) and k (Fenton) < k (solar
irradiation) < k (photo-Fenton), for the AOPs tested. This consistent behavior is also observed here. Although the
list of MPs has widened, including both photo-sensitive and “resistant” compounds, the effluents of MBBR
again facilitated the highest MP removal. More specifically, the micropollutant removal efficiency
dropped as we move from MBBR to AS and CF, in all types of AOP applied, attributed to the COD and DOC
content of the respective effluents. Furthermore, as far as the comparison among the tested AOPs is
concerned, only a relative order can be established, as the processes differ significantly. UVC/H2O2 and its
massive HO● production has a profound effect in MP elimination (2-10 min), whereas UVC alone requires
a mere 35-40 min for total removal of the parent compounds. The difference among the times in each
process is a function of the pre-treatment. These processes achieved also a very high degree of
mineralization (Giannakis et al. 2015c), therefore their application holds high potential.
On the other hand, solar, Fenton and photo-Fenton processes would require much longer times to fully
degrade the MPs. After 1 or 2h, when our experiments stopped and the apparent first order k constant
was calculated, a maximum of 50% elimination took place, in the photo-Fenton reaction after 1h in MBBR
effluents. The apparent k indicates minimum 2-h exposure to achieve 100% removal. As at the end of our
exposure period more than 75% of the oxidants was available (data not shown, available (Giannakis et al.
2015c), the assumption that the process would continue uniformly for an additional period holds true.
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Furthermore, an interesting observation takes place if the synergy among the constituents of the photo-
Fenton reaction is concerned. As it appears, the photo-Fenton process is more efficient than simply the
sum of its parts. The Synergy (S) is higher in the processes that were hampered in either way, solar or
organic load (see Supplementary Table S2). The reactivity of the organic pollutants with solar light is
limited and the enhancement of the process with the HO● generation could result in efficient removal in
relatively reasonable retention time.
3.3.2. Microorganism elimination in the different wastewater effluents, per AOP:
inactivation and post-treatment regrowth
3.3.2.1. UVC and UVC/H2O2 processes
Figure 3.3 showcases the bacterial inactivation after the application of UVC, with or without the addition
of H2O2. The effluents of MBBR, AS, CF and PT were exposed to monochromatic UVC irradiation (Figure
3a) or UVC and 20 mg/L H2O2. When UVC was applied alone, two distinct categories of kinetics were
observed, in either MBBR and AS effluents or in CF and PT. In MBBR and AS effluents the time necessary
to completely inactivate bacteria was similar (<1 min actual difference) while the 4-log reduction in CF
and PT effluents delayed significantly (10 min). The interpretation lies in the Achilles’ heel of UVC
applications. The two major drawbacks are the suspended solids and the organic content in the effluents.
The solids, apart from their physical barrier effect, they effectively shield microorganisms, and favor
aggregation. Hence, as the efficiency of the UVC irradiation relies in the transmittance of the medium, the
two effluents with lower SS content and therefore higher transmittance (UVCT in Table 3.1) presented the
lowest treatment times.
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Figure 3.3 – UV-based disinfection and respective regrowth of the indigenous bacterial population
after 24 h. A) UVC irradiation alone. B) UV/H2O2 process (20 ppm initial H2O2 addition). The shaded
part and the dashed lines symbolize the dark storage and regrowth after treatment, for 24 h.
The combined UVC/H2O2 process builds on the principles of the UVC disinfection, plus the homolytic
disruption of H2O2. The mechanism of UVC/H2O2 inactivation, is both external and internal. When H2O2 is
added into the bulk, the HO● attacks improve disinfection in all effluents; till now, there is no
microorganism found with resistance to the oxidation by HO●, contrary to damages by UVC irradiation
which is repaired instantly (Sinha and Häder 2002). For the aforementioned reasons, we naturally observe
decrease in all necessary treatment times in Figure 3.3b. The major enhancement observed in the CF and
PT effluents lies in the dependence of the disinfection efficiency in the transmission of UVC light. MBBR
and AS effluents contain significantly low organic content, which acts as a HO● scavenger (Ortega-Gómez
et al. 2014), and low SS; the improvement is of some minutes and the HO●-induced oxidation was proven
to affect the overall carbon content of the matrix (Giannakis et al. 2015c). In CF and PT effluents, since
the transmittance levels are lower, the benefit of the oxidative action was higher, with the HO● attacks
compensating the lower inactivation rates demonstrated when UVC alone is applied.
Finally, it should be noted that the wastewater effluents are far more complex to be dissociated only to
solids and organic scavenging, as many actors influence the degradation efficiency. For instance,
phosphorus moderately scavenges the radicals generated (Wu and Linden 2010) and UVC is absorbed by
nitrates, resulting to nitrite. Nitrite reacts with hydroxyl radicals, producing nitrite radicals, which are far
less oxidative, but on the other hand are more long-living (Vione et al. 2014). Margot et al. (Margot et al.
2011) measured high values of ions in MBBR effluents, due to the nitrification step, and their
participation cannot be overlooked. Finally, another dual mechanism is the scavenging of HO● by
carbonates (Carra et al. 2014), or the generation of carbonate radicals (Wu and Linden 2010). The high
alkalinity measured in AS and CF is an indication of high (bi)carbonate content, partially explained by the
lower pH values of the MBBR effluents, and the expected scavenging effect is higher than the beneficial
impact of the oxidation by the mildly oxidative carbonate radicals.
The shaded part of Figure 3.3 presents the regrowth assays performed for the UV-based processes. When
UVC irradiation is applied, the damage is mainly at the genome level, due to the high absorption by the
thymine and cytosine bases. The result is cyclobutane–pyrimidine dimers (CPDs), 6–4 photoproducts (6–
4PPs) plus their Dewar valence isomers (Douki et al. 2003). Within minutes of UVC exposure, the stress
induces responses of chaperones to repair the DNA damages, but soon this response is surpassed. As the
storage took place in the dark, the presented results are exclusively an effect of the base or nucleotide
excision repair, the mutagenic repair and other similar mechanisms (Sinha and Häder 2002). Similarly to
UVC disinfection, the regrowth is influenced by the dose of UVC received by the microorganisms. Hence,
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for similar treatment times, the different effluents result in a regrowth of increasing rate. After treatment,
the microorganisms that are present in the bulk can be categorized in some states, such as healthy (will
grow in WW), injured (which can regrow), apoptotic (which cannot regrow) and dead ones. The regrowth
presented here is the result of growth or regrowth from the first two categories. What is changing for
instance in MBBR effluents among 2.5 and 5 min, since the number of viable counts is the same, is the
regrowth potential and the shift towards the two last states. Finally, the differentiation among the various
statuses of cell conditions is more evident in CF and PT effluents. These received low UVC doses and the
higher final populations led to significant regrowth.
Concerning the UVC/H2O2 inactivation, the baseline damage is the UVC (common to the previous) adding
the oxidative action of HO●. If the damage was solely attributed to UVC, higher regrowth would be
demonstrated. The CF and PT effluents presented high regrowth rates, since they received low UVC doses
and suffered from high HO● scavenging. For the AS and MBBR effluents, when the inactivation process
was complete, no detectable regrowth occurred. The internal and external oxidative stresses posed by
HO● rendered the microorganisms unable to repair their lesions. Also, compared to the UVC alone, the
proportionality of residual concentration and regrown population was lower, attributed to the different
pathway brought by HO●. Finally, even for the non-favorable conditions met in CF and PT effluents, looking
the experimental process in retrospect, the regrowth was eliminated when the treatment was prolonged
beyond the necessary time for total inactivation. Hence in a field application, increasing the UVC dose
above the threshold for inactivation may ensure limitation of bacterial regrowth.
3.3.2.2. Fenton, solar and photo-Fenton processes
Figure 3.4 presents the results obtained when the Fenton reaction, solar light or the (solar-assisted)
photo-Fenton reaction were the inactivation driving forces. Concerning the Fenton reagents (Figure 3.4a),
H2O2 causes minor oxidation in outer cell wall layers, but also diffuses into the cell. The amounts of H2O2
used in this study are not bactericidal per se, and the modest inactivation achieved was the result of the
external Fenton reaction, by the addition of Fe2+ from our side, resulting to a massive oxidative wave. The
regeneration of ferric iron back to ferrous is very slow and difficult to recover since the Fe3+-dissolved
organic matter (DOM) complexes are very stable (Hakala et al. 2009); hence our low inactivation rates.
When H2O2 was doubled, the efficiency did not increase importantly. The HO● was partially scavenged by
the organic matter present in the solution. A positive effect though lies in the complexation of iron by
DOM after its conversion to Fe3+ and its reduced precipitation (Hakala et al. 2009). All effluents were in
the near-neutral region, in which the Fe3+ aqua-complexes are not soluble (Ruales-Lonfat et al. 2015).
Concerning the precipitated iron in the form of iron oxides, a small contribution of the heterogeneous
Fenton reaction is possible, with the iron oxides acting as iron source (Ruales-Lonfat et al. 2015), since all
effluents contain iron in lesser or higher amounts (Table 3.1).
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Figure 3.4 – Fenton-related disinfection and respective regrowth after 24 h. A) Fenton process (2:10
ppm initial Fe2+/H2O2 addition). B) bare solar light. C) photo-Fenton process (2:10 10 ppm initial
Fe2+/H2O2 addition). The shaded part and the dashed lines symbolize the dark storage and regrowth4
after treatment, for 24 h.
The exposure of the samples to solar only irradiation (Figure 3.4b) caused the bacterial inactivation in a
dual manner: UVB is documented to cause similar dimerization to the UVC-inflicted one, but in lower rates
(Cadet et al. 2005). UVA on the other hand initiates a chain of reactions in the bacteria, among which,
internal oxidative (Fenton-like) events are the most crucial (Imlay 2003, Spuhler et al. 2010). As it appears,
solar light demonstrated aspects similar to an indirect AOP. The nature of these actions initiated by UVB
and UVA explain the initial lag period (Giannakis et al. 2014b) visible in all graphs of Figure 3.4b and the
accumulation of this damage actually resulted to bacterial inactivation. UVB and UVA wavelengths are
also subjected to physical blocking and scattering by the suspended solids, and therefore their efficiency
was a function of the turbidity of the samples, as shown in Table 3.1.
As far as the photo-Fenton process is concerned (Figure 3.4c), within the time-frame studied, the
inactivation for any effluent was dramatically increased. In a recent review, we described the mechanism
of bacterial inactivation in water and wastewater (Giannakis et al. 2016a, Giannakis et al. 2016b). Briefly,
iron can complex with the organic matter and under light, a ligand-to-metal charge transfer (LMCT) results
to the sacrificial oxidation of the organic ligand (producing organic ligand radicals) and more importantly,
the regeneration of Fe3+ to Fe2+ (Spuhler et al. 2010). Furthermore, the simultaneous presence of iron,
DOM and solar light initiates photochemical cycles which can result in the production of ROS, such as HO●
and H2O2 (Canonica 2007, Ng et al. 2014). This cycle and its potential implications in wastewater effluents
(EfOM) has been previously analyzed (Giannakis et al. 2015c). Other sources of ROS are the nitrates and
carbonates (Vione et al. 2014, Wu and Linden 2010). As a result of the aforementioned actions, significant
microorganism removal took place in MBBR and AS effluents. In 3h the disinfection process was (almost)
complete, while even in CF and PT effluents the removal was important. The combined, multi-level
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damage inflicted by the photo-Fenton process can also be seen in the synergy calculated for these
experiments (see Supplementary Table S3).
The shaded part of Figure 3.4a summarizes the Fenton-related techniques regrowth. The Fenton process
was not efficient in inactivating the microorganisms present in the effluents. Only 1-2 log units of
inactivation represented the highest amount of bacteria removed from the bulk. Nevertheless, the
residual H2O2 and the iron present in solution (complexed or dissolved) efficiently continued the Fenton
process during the dark storage period. Furthermore, a bacteriostatic behavior is observed in all but the
PT effluents. As discussed before, this is a result of the excess of targets present in the solution. Also, the
final concentration of bacteria after 24 h was correlated with the number of leftover microorganisms at
the end of the “observation” period (since the same action continues for the whole 24 h). This fact is
promising, since this process could be used for suppressing any regrowth risk in treated wastewater,
during storage and before potential reuse.
Solar disinfection and its regrowth was previously studied by our group in synthetic, non-turbid effluents
(Giannakis et al. 2015b), where we correlated the exposure to solar irradiation with the regrowth, and
were able to identify the necessary solar dose for shifting from (post-irradiation) growth to a deterministic
decay phase. In Figure 4b, in all effluents, after 5 h of treatment, regrowth is demonstrated. Only after 6h
of exposure in MBBR effluents a bacteriostatic effect is observed. The main difference in the present work
is the presence of particles in WW which effectively aggregate and shield the microorganisms, thus
minimizing the received solar dose. Furthermore, the action mode of solar irradiation seems to be heavily
influenced by the UVA irradiation. If UVB was the main driving force, enhanced regrowth would be
demonstrated. In MBBR effluents, the bacteriostatic/decay phase observed after the exposure is an
indication of the internal oxidative damage occurring in the cell (Imlay 2003). Finally, the contribution of
the photo-sensitizable organic matter could influence the inactivation, by the production of HO● and H2O2
(Canonica 2007); iron is present in the effluents (especially in CF, Table 3.1), which in combination with
the small H2O2 accumulation could hamper the regrowth in the dark.
The application of solar photo-Fenton combines the benefits presented in the previous two processes.
Firstly, a decay phase is observed for the end-treatment phase in both AS and MBBR effluents, reaching
total elimination during the post-irradiation period. Most probably, the simultaneous exposure to solar
UV and the Fenton reagents limits the potential of recovery for microorganisms; this effect hinders their
growth in the minimal nutritional contents and the oxidative stress present in the WW effluents which
still contain H2O2 and iron (Giannakis et al. 2015c). The low organic content is probably the key point in
managing to effectively stop the growth. The PT effluents on the other hand still possess a great number
of healthy cells which continue to thrive. In conclusion, the short times of photo-Fenton by the exposure
under light and the continuous Fenton action have the best overall effect in inactivation and regrowth
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inhibition, which makes it a potentially attractive solution for WW treatment; possibly, if higher Fenton
reagent’s concentration was added to reduce the observed residence time, the process could be more
competitive.
3.4. Discussion
3.4.1. The major threat and treatment focus: micropollutants or microorganisms?
The previous chapters have dealt with the isolated problem of establishing proper disinfection or
decontamination in the wastewater effluents. Nevertheless, since the co-existence of MPs and MOs is the
actual situation, in this part we perform a combined approach and try to assess the treatment strategies
for ensuring both adequate MP removal and MO elimination, while suppressing post-treatment bacterial
regrowth. As thresholds, we have chosen the 3-log inactivation of microorganisms as minimum removal
(3 to 4-log for most reuse purposes; for instance (Liberti et al. 2003)) and the Swiss legislation limits for
micropollutants (80% elimination (Giannakis et al. 2015c)).
Figure 3.5 – UV-based disinfection and decontamination. A) UVC irradiation alone. B) UVC/H2O2
process. The lines indicate the microorganism inactivation, while the bars the micropollutant
degradation (%). The circles indicate the regrowth suppression points with the respective colors
indicating the secondary treatment method, while the horizontal lines indicate the minimal
micropollutant (brown line) and microorganism removal (orange line).
Figure 3.5 (a and b) presents in parallel the disinfection and the decontamination processes of the UV-
based processes. Concerning the UVC irradiation alone, we have noted the efficiency in the previous
chapters, and >99.9% MO removal can be achieved after 5 min of treatment. The immediate MP
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degradation does not satisfy the 80% threshold before 30 min of exposure except for the MBBR effluents.
Therefore, one could suggest that MOs are easier to remove and the design of the process has to be done
taking the MPs as reference. When bacterial regrowth is taken into consideration, different times are
reported to minimize this risk. For MBBR and AS effluents, 5 and 10 min were necessary, respectively. In
our samples, regrowth suppression was not achieved in CF effluents before 10 minutes but extrapolating
from the MBBR and AS effluents, in 30 min it is safe to believe that it would be no longer possible to
contain healthy or repairable microorganisms. Even so, 30 min of exposure is the threshold for MPs
removal and therefore, indeed the design needs to be implemented according to the MPs; their removal
means an already achieved acceptable disinfection level.
For the UV/H2O2 process, the necessary times were decreased. Only 2.5 and 5 min of treatment were
found necessary for MBBR and AS (and CF) effluents, respectively. The regrowth was completely
suppressed after 2.5, 5 and 10 min for MBBR, AS and CF as well. Comparing the necessary time for
minimum 3-log removal and regrowth inhibition, we observe that MPs were removed at least at 85% (up
to 99%) for all effluents. This means that if the design takes place for the minimal MP removal, then
effluents that have been subjected to biological treatment are also microbiologically safe. Only for the
physicochemical process a prolongation would be necessary, and a higher (but not complete) MP removal
was attained. If we take into account the higher oxidative conditions used for MPs removal (25 ppm H2O2
vs. 20 ppm and 5 ppm Fe2+ vs. 2 ppm), the micropollutants should definitely be the primary target.
Therefore, for both the UV-based processes, the reference for micro-contaminant and microbiological
safety is the removal of MPs.
For the Fenton and solar processes presented in Figure 3.6a, and 3.6b neither MPs nor MOs have been
successfully removed; after 6 h, moderate removal was achieved. In the Fenton process, if the k constant
remains quasi-linear, around 6 h would be necessary for efficient MP removal, therefore the exposure
times would be similar. After these exposure/treatment times, regrowth should not be an issue; after 6 h
of solar treatment, bacteria in MBBR effluents demonstrated stationary behavior and when the Fenton
process was used, the presence of the reagents efficiently suppressed regrowth.
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Figure 3.6 – Fenton-related disinfection and respective regrowth after 24 h. A) Fenton process. B) Bare
solar light. C) photo-Fenton process. The lines indicate the microorganism inactivation, while the bars
the micropollutant degradation (%). The circles indicate the regrowth suppression points with the
respective colors indicating the secondary treatment method, while the horizontal lines indicate the
minimal micropollutant (brown line) and microorganism removal (orange line).
On the other hand, the photo-Fenton process shows (Figure 3.6c) promising potential, as the order of
magnitude of bacterial decay is reduced to the hour range. More specifically, after 2 h of treatment the
MBBR and AS effluents are almost bacteriologically safe (99 and 97% removal, respectively) and above
the 80% threshold for MPs. Furthermore, after 3 h, apart from the attained disinfection, regrowth is
suppressed for biologically treated effluents and almost for all effluents decontamination is achieved
(~79% for CF). These results demonstrate that for the Fenton-related processes, a shift in the importance
takes place and bacteriological targets are gaining importance over the organic contaminant ones. We
believe that if similar oxidative conditions were to be used (higher were used in MPs experiments), after
2 h, complete disinfection could have been achieved and the only open question should be regrowth.
Nevertheless, the results indicate with a high level of certainty that MOs inactivation and regrowth could
be taken as reference, since >80% MP removal is estimated to precede the disinfection events.
3.4.2. Common events and dissimilarities in the treatment of different targets in
secondary effluents
Although we cannot possibly compare the two families of AOPs applied, i.e. UV-based and Fenton-related
ones, a separation can be made according to the effluents. MBBR effluents always allowed degradation
of the targets faster than AS, CF, and PT, in order of decreasing efficiency. However, an intriguing
controversy among the investigated effluents is the shift in the order of importance, when the family of
AOPs used is modified. When the UV-based technologies were applied, the MPs were the reference
target, while, in the Fenton-related processes the MOs disinfection and their regrowth risk are more
important. Even though this difference is marginal, it contradicts the clear importance of the MPs in the
UV-based processes (and MOs for the Fenton-related) and at this point we will try to assess the main
parameters behind this issue.
1) The nature of the target plays a key role.
The micropollutants are complex, high molecular weight (HMW) structures with the ones studied here
almost all exceeding the 200 g/mol. Sensitive LC-MS analyses have identified that the various attacks
against the molecules can be either photonic (UVC induced damage) or ROS-related. These mechanisms
can result to ipso, para, meta attacks, -OH addition, halogen scissions etc. for UVC light, while ketone
formation, decarboxylation, side chain breakage, H+ abstraction (and other) have been found for the HO●-
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induced attacks (Zhao et al. 2014). Even a moderate structural modification, such as short side-chain
breakage induced by e.g. a radical attack, modifies the micropollutant significantly, and the by-products,
even those structurally similar to the parent compound, are no more considered for the calculation of the
degradation percentage. However, these by-products continue to get degraded in the bulk, but compared
to the carbon content of the wastewater, their amount is negligible (Giannakis et al. 2015c).
Microorganisms on the other hand, seem to require significantly more attacks in order to get inactivated.
The influence of the light or the radicals in key structures (e.g. lipids in cell membrane) has a mitigated
effect, leaving the microorganism viable. As this damage progresses, the result could be bacterial death.
It is an intriguing question however, the effect of each process on bacterial viability, i.e. quantify the UVC
photons required to inactivate a microorganism, hinder its regrowth, or the ROS-induced attacks
necessary for membrane rupture etc. For the HO● effect alone and the necessary amount to inactivate a
single E. coli it has been found to be in the order of 109 (Marugán et al. 2008).
2) The heterogeneity of targets (number and size) acts in a dual manner.
The amount of each micropollutant in WW effluents is found most frequently in the ng/L and low μg/L
range. If a theoretical sum of all the contaminants of emerging concern is assumed at μg level, then in our
experiments, a g/mol is estimated and therefore at 300 mL of sample we get around of 1015
“pollutant targets”. Similarly, the maximum amount of bacteria encountered was of 105 CFU/mL, hence
~108 CFU are expected. It becomes clear that the micropollutants are in order of millions more than the
bacteria. However, the size of a molecule is Å to nm scale, while bacteria range around the μm range;
hence, the difference is in the order of thousands. All things considered, although there are far more MP
“molecules” to degrade, since the HO● radicals are limited by diffusion, it is probably easier to inflict
attacks on a big and rare-to-find microorganism, rather than reach a small and abundant pollutant.
Furthermore, the assumptions made in this study have to be re-considered when experimenting with
urban WW. For instance, bacteria are not the sole microorganism present (especially the monitored ones),
although our medium has optimal recovery for the spread plate method. Viruses, protozoa and others
compete for the oxidants generated, however in lesser extent than the EfOM. Also for MPs, we chose a
list of contaminants relevant to the research trends, but among the list, there are contaminants with
limited light reactivity (e.g. Atenolol) or high reaction rate constants with HO● (e.g. Diclofenac). As a result,
the percentage of removal is a relative measurement, and in future studies, the wider the list of
contaminants, the better approximation will be achieved.
3) Technical aspects related with the application of AOPs are implicated.
This study is a bench-scale simulation of a field application, using real WW effluents, but employing a
certain reactor geometry. The experiments were performed under a smaller optical path than the
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dimensions of, for instance, a UVC-based plant. This fact explains mainly the Figure 2.2 and the MP
degradation results, where although a linear change is observed, the difference among the pre-treated
effluents and the effect on degradation is lower than the respective one in microorganisms. Another
example is the efficiency of the UVC process after primary treatment only. Indeed, for a short exposure
time, with a short optical path, the difference is mitigated, but in a real application, the scale-up problems,
the effect of suspended solids, the cleaning of the quartz sleeves due to particle settling and
polymerization would make this application impossible. As UVC exposure requires low SS and high UVCT
waters (min. 35%), the PT effluents are rejected and the CF ones would be marginally accepted (see Table
1) to be treated by such a system. Therefore, although in some cases the results do not justify it
completely, a biological pre-treatment is necessary before AOPs application for disinfection.
4) Effluent characterization complexity hides the mode of action of the different AOPs.
Another controversial point comes at the attribution of the effect of AOPs to each effluents, as a direct
effect from the physicochemical characteristics presented in Table 3.1. As found for both microorganisms
and micropollutants, the order of degradation in all cases is MBBR > AS> CF > PT, for all AOPs used. One
could dissociate the two groups, of MBBR with AS (biologically treated effluents) and the CF with PT
(physicochemical processes). In the first group, the effluents present similar light transmittance, and
therefore, their optical-based effects are quite similar. The AS has higher alkalinity and organics content,
so the disinfection is slightly hindered. In the second group, the effluents present similar SS content, with
the CF effluents having been through a physicochemical removal of smaller (colloidal) particles.
Table 3.2 – Photochemical characteristics of the various effluents
Index PT AS MBBR CF
E2 (254 nm) 0.430±0.16 0.147±0.04 0.109±0.04 0.391±0.22 E3 (365 nm) 0.084±0.05 0.017±0.01 0.013±0.01 0.074±0.06
E2:E3 5.432±1.03 14.545±14.18 24.386±29.15 5.935±1.68
E4 (465 nm) 0.040±0.03 0.006±0.01 0.005±0.01 0.008±0.01 E6 (665 nm) 0.021±0.01 0.004±0.01 0.004±0.01 0.004±0.01
E4:E6 1.909±0.13 0.625±0.88 0.563±0.8 0.813±1.15
ε280 0.327±0.10 0.121±0.03 0.091±0.03 0.171±0.01 SUVA (DOC/E2) 273.15±15.88 168.59±3.21 70.22±4.66 178.32±5.52
Slope 275-295 nm 0.00250 0.00130 0.00055 0.00275 Slope 350-450 nm 0.00055 0.00015 0.00012 0.00051
SR (slope ratio) 4.697±0.78 10.472±5.62 8.750±8.84 5.413±0.11
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As a result, parameters with profound differences seem to merely affect the process (e.g. COD), as
ultimately, we assess the net degradation force at each effluent. To better investigate this effect related
with the organic matter, a look into the characterization of the organics content, which can act either as
(photo-) sensitizable or oxidizable matter, is useful (Giannakis et al. 2015c); to assess this possibility, a set
of photo-activity indices and measurements were applied to these effluents (see Table 3.2). The detailed
absorption spectra for the four effluents, are given in the supplementary material (Supplementary Figure
S2).
The specific wavelengths are used for photochemical activity evaluation purposes. The E2:E3 and the E4:E6
ratios, are measures of aromaticity, which indirectly imply photo-activity. The MBBR effluent presented
the highest E2:E3 ratio. The E4:E6 indicates higher colored dissolved organic matter (CDOM) presence; in
fact, higher E4:E6 ratio means low aromaticity (Fu et al. 2016). Since sometimes the absorbance at 665 nm
is zero, the ε280 (Helms et al. 2008) or SUVA (specific UV absorbance) were suggested as aromaticity
indexes. In our case, it corroborates with the rest of the findings. Also, the dimensionless slope ratio (SR)
(Helms et al. 2008) increased as we move from PT to MBBR (lowest to highest ratio) and suggested lower
molecular weight fractionated organic matter present in the effluent (Fu et al. 2016). Ultimately, since
LMW organic matter is proposed to act as photo-sensitizable organic matter (PhOM) rather than
oxidizable (OxOM) (Giannakis et al. 2015c, Vione et al. 2014), the possibility to participate in generating
ROS is higher. The generated ROS then participate in the controversial points 1 and 2, as analyzed before.
With this overview, it is safe to suggest that the physicochemical parameters followed in the effluents of
this work give only a view on some key factors influencing the process. This linear behavior is merely the
geometrical sum of the different actors present in WW water. In each effluent, the presence of
“secondary” parameters, such as the carbonates, or the organic matter, are vectors which can act either
synergistically or in an antagonistic manner.
5) Differences in the response between the two families of AOPs, for the different targets.
The UVC and UV/H2O2 processes were found to inactivate microorganisms and degrade pollutants rather
efficiently in all cases, whereas the Fenton and solar light (and less the photo-Fenton) require special
conditions (e.g. prolonged exposure) to ensure the success of the application. Apart from the obvious
differences in kinetics due to massive HO● generation in the UV/H2O2 process and higher energy in the
UVC photons (compared to solar UVB and UVA ones), there are other biological issues implicated in the
observed change in the reference and the importance attributed to each target.
When targeting micropollutants, the type and intensity of light applied, the addition of reagents etc. affect
the apparent 1st order degradation kinetics. However, in microorganisms, when light based processes are
involved, more issues should be considered. For instance, when UVC light is applied, the absorbance by
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the thymine and cytosine bases is much higher than the UVB supplied by (simulated) solar light (Cadet et
al. 2005). As a result, the time necessary to inactivate microorganisms is in order of minutes, compared
to hours, for UVC and solar light, respectively. On the contrary, if many hours are required for completing
a solar disinfection experiment, given that bacterial (E. coli) cell division takes place every ~30 mins, many
generations of microorganisms could be formed, thus constantly repopulating the sample. In conclusion,
the forces of inactivation and salvation of microorganisms are far from collinear. This delicate balance,
which depends on light irradiance, solar dose, temperature and more, may contribute significantly in the
change of order of importance among the chemical and microbiological contaminants observed in the
Fenton related processes.
3.5. Conclusions
The use of five AOPs against microorganisms and contaminants of emerging concern was assessed in this
work, focusing in the differences among the two broad categories tested here, the UV-based and the
Fenton-related ones. In combination, three effluents were treated, from which two involved biological
treatment (AS, MBBR) and a physicochemical one (CF), while presenting the primarily treated as control
(PT).
The quality of the effluents influenced the outcome of the experiment, for micropollutants and
microorganisms, both for immediate removal or regrowth suppression. In general, the order of effluent
quality was MBBR>AS>CF. The measured physicochemical characteristics of these three effluents
influenced in the same manner the application of the AOPs. Among the two AOP groups, the order of
efficiency for the UV-based processes was UVC<UVC/H2O2 for both targets, while for the Fenton-related
ones was solar<Fenton<photo-Fenton for micropollutants and Fenton<solar<photo-Fenton for
microorganisms. Even so, high levels of synergy where observed for the constituents of the photo-Fenton
process and its utilization in neutral pH was encouraged. The post-treatment events of bacterial regrowth
were monitored, and prolongation of the treatment beyond the required time for inactivation was the
solution for the UV-based processes, while the Fenton-related ones, as they employ different inactivation
mechanisms that can hinder regrowth, need optimization of the Fenton reagent’s addition.
Taking into account the levels proposed by the Swiss legislation for micropollutant removal and the
threshold for water reuse of treated wastewater, if a quaternary treatment unit based on UVC irradiation
(with or without H2O2) was to be considered, the removal of micropollutants is a better indicator of water
quality; the use of H2O2 reduces significantly the residence times but increases the operational cost and
design implications. In other contexts than Switzerland, i.e. sunny or developing countries, if the Fenton-
related processes are to be considered, the bacteria were (marginally) considered to be a better reference
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for depollution of wastewater, as for these higher residence times (compared to UV) the micropollutants
demonstrated faster degradation kinetics than the respective micropollutant ones. The variation
appearing among the two families of AOPs in the secondary effluents are a result i) of the structural
differences among the targets, ii) the degradation/inactivation pathway, iii) the reactor design
specifications, iv) the photochemical characteristics of the effluents and v) the biological implications of
the targets, such as bacterial growth and regrowth during treatment. As a result, apart from the
physicochemical data which can be easily monitored, photo-chemical indicators, design implications and
a battery of tests (microbiological, analytical) should be considered, in order to firstly well-characterize
the effluents and then refine the treatment strategies applied. Finally, although adequate MP removal
can be achieved, the degradation by-products and the potential toxicity problems related with the studied
processes are yet to be determined.
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PART 2
Hospital-derived microorganism inactivation in developing countries
by Fenton-related AOPs: mechanistic interpretation and underlying
mechanisms of the photo-Fenton process.
101
4. Chapter 4 - Effect of Fe(II)/Fe(III) species, pH, irradiance and
bacterial competition on viral inactivation in wastewater by
the photo-Fenton process: Kinetic modeling and
mechanistic interpretation.
Work accepted for publication in Applied Catalysis B: Environmental
Stefanos Giannakis, Siting Liu, Anna Carratala, Rtimi Sami, Michaël Bensimon, César Pulgarin (2017).
Effect of Fe(II)/Fe(III) species, pH, irradiance and bacterial presence on viral inactivation in wastewater by
the photo-Fenton process: Kinetic modeling and mechanistic interpretation.
Supplementary Material:
Appendix D
Doctoral Candidate’s contribution:
Main investigator and author.
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4.1. Introduction
Wastewater disinfection is of major importance to prevent the microbial contamination of downstream
water resources. Treatment strategies such as filtration, chlorination or UV-radiation for microbial
inactivation have been developed over the last decades and their efficiency against bacteria (McGuigan
et al. 2012), viruses (Carratalà et al. 2016) and parasites (Carter 2005, Weir et al. 2002) has been assessed
in a number of studies. Nevertheless, treatment strategies are turning towards greener and more
sustainable techniques, such as the Advanced Oxidation Processes (AOPs).
Among these techniques, the photo-Fenton process has emerged as a prominent solution to treat
chemical contaminants (Malato et al. 2009), but the number of studies focusing on microorganisms is
significantly inferior. This process has been found to inactivate structurally simple (Kim et al. 2010),
complex (Giannakis et al. 2016c) or resistant microorganisms (Karaolia et al. 2014), and is promoted
because of its simplicity, low cost and limited environmental footprint (Pulgarin 2015). In the Fenton
reaction, hydrogen peroxide reacts with iron generating hydroxyl radicals, which are the predominant
reactive oxidizing species (ROS) responsible for microorganism inactivation in AOPs, and effectively
oxidize microbial components, such as amino acids and nucleotides (Giannakis et al. 2016a, Giannakis et
al. 2016b). In this process, iron acts as a catalyst, is repeatedly oxidized and reduced. In wastewater, the
process becomes significantly more complicated, due to the chemical and biological complexity of the
matrix and the imminent iron precipitation due to the near-neutral pH (6-8). Also, the presence of effluent
organic matter (EfOM) in wastewater (e.g. humic acid, fulvic acid), can scavenge a significant part of the
generated HO●, leading to a weakened inactivation (Rincón and Pulgarin 2004). However, other reports
have pointed out that light radiation on EfOM components (i.e. the dissolved fraction of the organic
matter, DOM) can create intermediate radical species, which react with water to generate HO● (Kohn and
Nelson 2007), and partially compensate for the loss of HO● by DOM.
Furthermore, Fe ions form complexes with organic matter and these Fe-organo species not only absorb
light, but also stabilize at near neutral pH. This extends the application of the homogenous photo-Fenton
reaction with less pH dependency (Spuhler et al. 2010). Under solar light exposure, the organic ligands
that compose the DOM form complexes with Fe(III) and participate in a ligand-to-metal charge transfer
(LMCT) type reaction (Ruales-Lonfat et al. 2015). However, during the photo-Fenton process, both
organics degradation and microorganism inactivation would compete. DOM may scavenge ROS and
provide targets of degradation with protection sites (Pignatello et al. 2006).
Most of the previous works on the efficacy of photo-Fenton processes against microorganisms at near
neutral-pH were done targeting bacteria (e.g. (Giannakis et al. 2015d, Ndounla et al. 2014, Ndounla et al.
2013, Ortega-Gómez et al. 2014, Ortega-Gomez et al. 2012), either in pure water or simulated wastewater
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with NOM-like substances. To date, however, there is much less experimental information on the
efficiency and parameters governing the photo-Fenton inactivation of viruses (Kim et al. 2010, Kohn and
Nelson 2007, Nieto-Juarez and Kohn 2013, Nieto-Juarez et al. 2010, Ortega-Gómez et al. 2015). MS2
bacteriophage is a single-stranded RNA virus, which infects Escherichia coli thorough the pili and
resembles certain human enteric viruses in size (27.5 nm) and structural complexity. Also, it can be rapidly
cultivated in laboratory conditions up to the high concentrations needed for most inactivation studies, is
easily purified, not pathogenic to humans (Kuzmanovic et al. 2006, Templeton et al. 2006), which explains
its frequent selection as a model virus in microorganism inactivation studies (Bradley et al. 2011).
The main purpose of this work is to assess the overall efficiency of photo-Fenton inactivation against
viruses in wastewater, using MS2 bacteriophage as a model. Furthermore, the effect of major parameters
implicated in the process (namely Fe species and concentration, sunlight irradiance, initial pH and
bacterial competition) is also assessed, emphasizing the alterations inflicted by the presence of organic
matter in the matrix. The obtained datasets were used to propose a mathematical and a mechanistic
model to describe the pathways exerted during the photo-Fenton inactivation of MS2 bacteriophage in
wastewater.
4.2. Materials and methods
4.2.1. Chemicals and reagents
In the experiments, all the chemicals were reagent grade or above, and all the solutions were prepared in
water purified at analytical grade using a Millipore Elix 3 system combined with a Progard filter (Millipore
AG, Zug, Switzerland). The pH measurement was handled by a digital pH-meter (S220 SevenCompactTM
pH/Ion, Mettler Toledo).
4.2.1.1. Fenton reagents
Iron salts of FeSO4 7H2O (≥ 99.0%, Sigma-Aldrich) or Fe2(SO4)3 xH2O, (97%, Sigma-Aldrich) were used
according to the required starting iron species. The H2O2 stock solution in water was prepared with
PerdrogenTM (H2O2, 30% w/w, refrigerated, Sigma-Aldrich) and the quenching agent for H2O2 residuals was
aqueous solution prepared with a mixture of NaHSO3 and Na2S2O5, (99% Acros Organics).
4.2.1.2. Synthetic secondary wastewater
The synthetic wastewater was chosen rather than the secondary effluent from WWTP, for its ability to
provide an identical water matrix for every single experiment. The composition of the synthetic secondary
wastewater is shown in Table 4.1 (Muthukumaran et al. 2011). A concentrated stock solution (×10 times)
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was prepared and dilution to reach the levels of Table 4.1 was done. The dilution was regulated to neutral
pH (pH 6, 7 or 8 in different series of experiment with 0.1 M NaOH or HNO3) before use.
4.2.1.3. Fe(II)/Fe(III) determination
The Fe(II)/Fe(III) concentrations in experimental samples were measured by a modified Ferrozine method
(Viollier et al. 2000), in which Fe ions chelated with the organic ligand Ferrozine and the formed magenta
iron complex was determined by absorbance measurement at 562 nm. This modified method could be
applied to detect μM level of Fe ions in water samples containing DOM. ICP-MS was also used to monitor
trace Fe amounts during experiments. The FinniganTM ICP-MS 7-238- NU1700 used was equipped with a
double focusing reverse geometry mass spectrometer presenting low background signal and high ion-
transmission coefficient. The spectral signal resolution was 1.2×10^5 cps/ppb. Fe from the solutions was
digested in 69% nitric acid (1:1 ratio HNO3:H2O), ensuring organics removal in solution and ions adhesion
to the vial wall. MS quantification of Fe concluded the analyses.
Table 4.1 – Composition of synthetic secondary wastewater (Muthukumaran et al. 2011).
Substances Composition [mg/L]
Meat extract (Sigma-Aldrich) 1.8 Peptone from meat, peptic digest (Sigma-Aldrich) 2.7
Humic acid (Carl Roth) 4.25 Tannic acid (AppliChem) 4.18
Lignosulfonic acid, sugared sodium salt (Sigma-Aldrich) 2.4 Sodium dodecylsulfate (NaC12H25SO4, 98%, Abcr) 0.9
Arabic gum powder (Acros Organics) 4.7 Ammonium sulfate ((NH4)2SO4, ≥ 99.0%, Carlo Erba Reagents) 7.1
Potassium phosphate dibasic (K2HPO4, ≥ 99.0%, Sigma-Aldrich) 7 Ammonium bicarbonate (NH4HCO3, ≥ 99.0%, Sigma-Aldrich) 19.8
Magnesium sulfate heptahydrate (MgSO4 7H2O, Sigma-Aldrich) 0.71
4.2.1.4. H2O2 determination
During the photo-Fenton experiments, the H2O2 concentration in the system was monitored. By reacting
with 10 μL of titanium(IV) oxysulfate solution (TiOSO4, 1.9-2.1%, Sigma-Aldrich), the H2O2 concentration
in a 1 mL experimental sample was quantified by measuring the colorimetric absorbance of the produced
yellow-colored pertitanic acid (H2TiO4) at 410 nm (Eisenberg 1943).
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4.2.2. Sunlight source and reactors
4.2.2.1. Suntest solar simulator
The experiments were conducted using a solar simulator (CPS Suntest System Heraeus Noblelight, Hanau,
Germany) with infrared and UVC cut-off filters in order to simulate solar global radiation from outdoor
daylight and to prevent from the influence of UVC radiation and thermal heating (the emitted spectrum
can be found in the Supplementary material, Figure S1). The solar radiation intensities used in the assays
were 300, 600 and 900 W/m2 (global irradiance) which were monitored by the combination of a UV
radiometer and a pyranometer connected to a data-logger (CUV3 and CM6b respectively, Kipp & Zonen,
Delft, Holland). These values represent typical intensities achieved by solar light for different seasons,
latitude and/or time points within a day. According to previous experiments and own current
measurements performed under the same conditions, the temperature in the simulator never exceeded
38 °C (Spuhler et al. 2010).
An irradiance of 300 W/m2 was selected in the experiments concerning pH variations and different ratios
of Fenton reagents. At this relatively low light intensity, the MS2 inactivation was slower and the
inactivation kinetics could be better distinguished. However, the inactivation experiments in systems of
MS2 and host E. coli coexistence were carried out under the irradiance of 600 W/m2 in order to enhance
the E. coli inactivation rates.
4.2.2.2. Glass reactors
All the solar radiation experiments were performed in Pyrex, UVB-transparent glass vials of 100 mL, while
brown ones were used in the dark Fenton controls. Inside the solar simulator, a rectangular stirrer (MIX
15 eco, 2Mag Magnetic Motion, München, Germany) was used to place the reactors and the reaction
solutions were continuously stirred at 350 rpm. In order to avoid iron cross-contamination, after every set
of experiments, all glass reactors were soaked in 10% HNO3 overnight and then rinsed with deionized
water before heat-sterilization.
4.2.3. Microorganisms and quantification methods
4.2.3.1. Microorganisms
MS2 phage (DSMZ 13767) and the antibiotic-resistant (2 mg/L streptomycin) strain of bacterial host
Escherichia coli (DSMZ 5695) were obtained from Deutsche Sammlung von Mikroorganismen und
Zellkulturen (DSMZ, German Collection for Microorganisms and Cell Cultures, Braunschweig, Germany).
The propagation and purification of the coliphage was following the procedure described by Ortega-
Gómez et al. (Ortega-Gómez et al. 2015). The preparation of the bacteria for the co-culture experiments
followed a protocol similar to the one for E. coli K-12 (Giannakis et al. 2015b, Giannakis et al. 2014c).
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4.2.3.2. Phage and bacteria quantification
Infective MS2 Coliphage was measured by the double agar layer technique (DAL, EPA Method 1602, 2001).
Plates were incubated at 37 °C for 18-24 h in a CO2-controlling incubator (B 5060 EK-CO2, Heraeus
Instruments, Hanau, Germany) and then the plaque forming units (PFU) were counted manually. The
detection limit of these experimental methods was found to be 10 PFU/mL. E. coli were handled with the
spread plate technique and colonies were quantified by the standard plate count method and results were
collected similarly.
4.2.4. Inactivation experiments
At the beginning of each experiment, 50 mL of the spiked wastewater matrix in the glass reactor was
stirred in the dark for 10 min to get evenly mixed. By adding 50 μL of 109 PFU/mL MS2 stock in carbonate
buffer solution (CBS, 8.401 mg NaHCO3, Sigma-Aldrich, and 876.6 mg NaCl, Sigma-Aldrich, dissolved in
1000 mL of water, adjusted pH to 8), the initial concentration of infective MS2 was around 106 PFU mL-1.
The reactors were then spiked with Fe(II)/(III) from freshly prepared stock solutions (500 mg/L) to reach
the final concentration at 0.25, 0.5 or 1 mg/L. Lastly, H2O2 was added from a fresh stock solution (1000
mg/L) and the final concentration was 0.5 or 1 mg/L. Next, the Xenon lamp was turned on to photo-
inactivate viruses under continuous irradiation at constant intensity. Corresponding control experiments
containing MS2 and Fe ion or H2O2 alone, under solar light or in the dark, were also conducted. To monitor
MS2 inactivation in the presence of its host, experiments were conducted at the light intensity of 600
W/m2, using 1 mg/L of Fe and 1 mg/L of H2O2.
During the experimental process, samples of 0.5 mL were taken at certain time intervals and immediately
mixed with 10 μL NaHSO3 aqueous solution (100 mg/L) to scavenge exceeding H2O2. Inactivation of MS2
and E. coli caused by NaHSO3 and dilution solutions was negligible over the experimental period (Kim et
al. 2010). Finally, before use, all the materials and solutions were autoclaved at 15 psi, 121 °C for 15 min
(Fedegari FVG1, Vitaris AG, Baar, Switzerland) to achieve complete sterilization.
4.2.5. Data treatment and analysis
Experimental data were expressed as the measured plaque forming units over time (PFU/mL vs. time),
where the instant MS2 concentrations were presented as arithmetic means ± standard deviations
calculated from the last three serial sample dilutions. For experiments involving host E. coli, the same
operation was done in interpreting its colony forming units (CFU/mL).
From the slope of a linear regression of ln([virus]0/[virus]) vs. ln(time), the observed k was determined as
the first-order inactivation rate in each individual experiment. In the systems involving Fe(II), where the
inactivation was better approximated by a two-phase exponential approach (Kim et al. 2010), for each
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phase a first-order kobs was determined. The curve fitting for each series of experiment was conducted
with Maple 18 (Waterloo Maple Inc.) or Excel 2010 (Microsoft Corp.).
4.3. Results and Discussion
4.3.1. Isolated effect of the photo-Fenton constituents
First and foremost, all the experiments conducted in this work took place in a (simulated) secondary
wastewater matrix, therefore the inherent challenges encountered when stepwise constructing the
photo-Fenton process merit a separate mention.
4.3.1.1. Effect of the Fenton reagents in absence of light and the effect of solar irradiance
MS2 infectivity was well preserved in absence of light and Fenton reagents’ addition (see Supplementary
Figure S2). These results were similar to the viral survival curve obtained in CBS (Ortega-Gómez et al.
2015), although here at pH 7 and a complex dilution matrix. Adding 0.25 mg/L of Fe(II), Fe(III) or 0.5 mg/L
of H2O2 had a negligible effect within 60 min (<0.5-log inactivation). When both Fe ion and H2O2 were
applied simultaneously, the (dark) Fenton system with Fe(II) showed a 1.2-log inactivation while almost
no virucidal effect was observed for the Fe(III) system; this differentiation is also parallel (but lower) to
Kim et al. (Kim et al. 2010), where CBS served as the MS2 suspension medium. Although 1.2-log
inactivation is low, the higher efficiency compared to the other (milder or Fe(III)-driven) processes reveals
the potential of viral infectivity decrease in the complex WW matrix.
When samples were exposed to (global) irradiance of 300, 600 or 900 W/m2 for 60 min, the infectivity of
MS2 did not demonstrate a significant decrease, which indicated the relatively high resistance of MS2
towards UV/visible light, in accordance to previous findings (Nieto-Juarez et al. 2010, Ortega-Gómez et al.
2015). In addition, the wastewater matrix itself did not show a notable impact on virus inactivation under
solar radiation. The operating pH (initial pH: 7) and the presence of particles did not significantly affect
the infectivity of the viruses present in the matrix.
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4.3.1.2. Effect of sole H2O2 or Fe addition on MS2 sunlight inactivation
Figure 4.1 – Solar/H2O2 and Solar/Fe control experiments. a) Isolated effect of the operating H2O2
levels of this work. b) Addition of 0.5 or 1 mg/L Fe(II) or Fe(III) salts. DL: detection limit.
In Figure 4.1a, under 600 W/m2 of solar irradiance, H2O2 doses of 0.5 and 1 mg/L contribute at about 0.5
log MS2 inactivation further than the effect of solar radiation alone. This result contradicts what was
reported by Ortega-Gómez et al. (Ortega-Gómez et al. 2015) in buffered water, which showed a total
inactivation after 50 min by 1 mg/L of H2O2. The virucidal effect was explained as a consequence of solar
irradiation that made MS2 more sensitive to oxidants, rather than the impact of HO itself (Ortega-Gómez
et al. 2015). The apparent contradiction of low H2O2 efficiency here, however, could be interpreted by the
presence of NOM-like substances in the specific water matrix, which can act as efficient scavengers of
HO (Westerhoff et al. 1999) and non-selectively react with H2O2 in competition with MS2 particles.
As shown in Figure 4.1b, dissolved Fe ions in wastewater induced a more effective MS2 inactivation than
hydrogen peroxide under solar irradiation. The addition of 0.5 mg/L of Fe(II) resulted in a decay of 2.9-log,
while in the presence of 1 mg/L MS2 inactivation reached 3.5 log units. For Fe(III), the amount of 0.5 mg/L
had a decrease by 1.8 logs, and 1 mg/L led a 2.5-log inactivation. Nieto-Juarez et al. (Nieto-Juarez et al.
2010) observed that MS2 infectivity dropped by half over 30 min in their CBS matrix containing 0.056 mg/L
of Fe(III), and considered this degradation as either virus inactivation by Fe ion alone or virus aggregation.
The possibility of spontaneous aggregation of MS2 is unlikely here, as Fe-induced MS2 removal by
excessive aggregation was found negligible by filtering samples prior to plating as well (0.2 μm filtering)
and comparing the results with un-filtered ones (data not shown). Thus, it is implied that Fe ions serve as
the main actors of inactivation in the Fe/light system.
109
According to previous works concerning virus-metal interaction, the LMCT process would occur in the
iron- and MS2-spiked water matrix, where the iron-MS2 “complex” acted as a light sensitizer (Ortega-
Gómez et al. 2015). These iron-MS2 complexes resulted from the interaction of Fe cations and negatively-
charged MS2 virions (pI = 3.9) in the wastewater. However, in our experiments, the observation that Fe(II)
contributed to a higher MS2 inactivation than Fe(III) in wastewater contradicts the aforementioned
results, and implies an efficient electron transfer from iron first, most probably a direct reduction of viral
capsid elements with oxidation of Fe(II) to Fe(III). Afterwards, the events in the two iron systems follow
the same catalytic cycle. Nevertheless, the enhanced inactivation events observed, despite the
scavenging effects of DOM, suggest complexation possibilities of iron in this matrix, and higher
participation in MS2 inactivation than in the buffered waters (Kim et al. 2010, Ortega-Gómez et al. 2015),
and called for further experimentation.
4.3.2. Parametrization of MS2 inactivation by the photo-Fenton process in wastewater
The following section summarizes the experimental assays combining the main actors in wastewater
disinfection by the photo-Fenton reaction, namely irradiance, Fe:H2O2 ratio, Fe starting species and initial
pH.
4.3.2.1. Effect of solar irradiance and Fe species
Figure 4.2 – Effect of solar irradiance on the evolution of the photo-Fenton reaction. A) Fe(II) as
starting iron species. B) Fe(III) as starting iron species. A notable difference exists in the kinetic
families of Fe(II) or Fe(III). DL: detection limit.
Figure 4.2 shows that solar light significantly enhanced the virucidal effect of Fenton reaction. For Fe(II)
(Figure 2a), at initial concentrations as low as 0.5 mg/L Fe(II) and 1 mg/L H2O2, an increasing sunlight
110
irradiance caused a dramatic decay of MS2 titers (3-log) as compared to the inactivation observed in the
dark, reaching the detection limit (DL) after a 6-log decay in 10 min. In the Fe(III)-involving system (Figure
2b), only an irradiance of 900 W/m2 could achieve the same extent of inactivation after an exposure during
60 min, while exposure at 300 W/m2 and 600 W/m2 still improved MS2 inactivation by 2.4 and 3 log,
compared to the Fenton process alone, respectively. The dependence of inactivation efficiency on light
intensity in presence of Fe(III) implies a photonic limitation of the system and dependence of the solar-
driven actions in order to achieve viral inactivation. This effect suggests that while the Fe(II) photo-assisted
process is not light intensity- dependent, it has a direct HO●-related inactivation, but for Fe(III), the Fe(III)
complexes are indeed photo-active and the light-assisted LMCT process is the driving force of the
inactivation process (Eqs. 1-3) (Giannakis et al. 2016a, Giannakis et al. 2016b):
● (4.1)
● (4.2)
(4.3)
4.3.2.2. Effect of Fe:H2O2 Ratio and Fe starting species
Figure 4.3 – Effect of the Fe:H2O2 ratio on the evolution of the photo-Fenton process. a) Fe(II) as
starting species. b) Fe(III) as starting species.
Increasing the initial concentration of Fe ions in the experimental water matrix led to an improved MS2
inactivation effect in both Fe(II) and Fe(III) starting form (Figures 4.3a and 4.3b, respectively). Using Fe(II)
at low concentrations (0.25:0.5) required 30 min for total inactivation and after doubling, the necessary
time reached the 2’ experimental limitation (minimum time from sampling to plating). On the contrary,
only the high ratios, employing 1 mg/L of Fe(III) and 1 mg/L of H2O2 under 300 W/m2 of sunlight, 6-log
111
inactivation was achieved, in 50 min. In the meantime, lower concentrations of Fe(III) (0.25 mg/L and 0.5
mg/L) ended in only 1- and 2.2-log inactivation. The inactivation rate showed a dependency on the initial
Fe concentration, as well as verifying the dependence of the starting iron species. Ortega-Gómez et al.
(Ortega-Gómez et al. 2015) interpreted that the formation of Fe-MS2 complex was favored by the
increasing amount of Fe ion, resulting in the generation of oxidants close to virus particles, crucial for their
efficient inactivation (Nieto-Juarez et al. 2010).
The variation of inactivation effects by different initial concentrations of H2O2 was also displayed in Figures
4.3a and 4.3b. In sunlit Fe(III) (0.25 mg/L) systems, 1 mg/L of H2O2 increased the proportion of inactivated
MS2 by 0.5 log, when compared with the employment of 0.5 mg/L. When reacting with 0.25 mg/L of Fe(II),
by applying more H2O2, time used to reach complete inactivation was shortened from 30 min to 15 min.
Clearly, the difference due to varied H2O2 concentrations exhibited in a second phase (after 2 min) of
inactivation. As mentioned before, since the second period was driven by the regeneration of Fe(II) from
Fe(III), a higher concentration of H2O2 helps accelerate the overall inactivation process by the produced
ROS (Giannakis et al. 2016a, Giannakis et al. 2016b).
● ( ) (1.8) ● ( ) (2.2) ● ( ) (4.4)
● ( ) (4.5)
( ) (4.5)
( ) (4.6) ● ( ) (4.7)
● ( ) (4.8) ● ( ) (4.9) ● ( ) (4.10)
Because of the interaction between Fe(II)/Fe(III) and negatively-charged DOM (e.g. the pI of humic acid is
around 2) (Kohn and Nelson 2007), H2O2 was more efficiently used in the inactivation by photo-Fenton
process with Fe-DOM complexes than having its ROS quenched by it (Giannakis et al. 2016a, Giannakis et
al. 2016b).
Facilitator: (4.11)
Antagonist: ● (4.12)
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This explanation might be confirmed by the colorimetric H2O2 measurements during the experiments,
where the concentrations of H2O2 in the system can be considered constant (data not shown). Our findings
agree with (Timchak and Gitis 2012) who assumed that H2O2 regenerated constantly in HO2 and HO
radical reactions, through the following reaction (Giannakis et al. 2016a, Giannakis et al. 2016b):
● (4.13)
The MS2 survival curves in photo-Fenton systems containing Fe(II) or Fe(III) have different shapes. The
Fe(II)-induced photocatalysis performed a sudden decrease and all viruses were inactivated in 5 min;
comparing to the curve of 0.25 mg/L of Fe(II) and 0.5 mg/L of H2O2, which showed a distinction of two
inactivation phases, the proposal was put that the Fe(II) performance includes two distinct phases,
although due to its relatively high ability of disinfection, the second phase was only observed as a tailing
pattern under low concentrations (<0.5 mg/L). Tailing in UV-inactivation studies has been attributed to
recombination of viruses (Olsthoorn and Van Duin 1996) which requires that multiple (inactivated) MS2
virions to infect the same host cell (Mattle and Kohn 2012). However, the onset of a tailing in MS2 decay
was not observed for Fe(III). In this case, the overall inactivation rate was lower, and the decrease of MS2
infectivity followed a logarithmic curve without phase distinction. At a ferric dose of 0.5 mg/L, it was not
able to inactivate MS2 beyond 2.5 logs in 60 min. The second phase in the Fe(II) system at low
concentrations is correlated with the dependence to the Fe(III) presence, whose inactivation kinetics are
slower.
4.3.2.3. Effect of the starting pH
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Figure 4.4 – Effect of the starting pH on the evolution of the photo-Fenton process. a) Fe(II) as starting
species. b) Fe(III) as starting species.
The influence of pH on the photo-Fenton system is shown in Figure 4.4. The pH of applied water matrices
was measured before and after each experiment, with negligible drop noticed after 60 min of
experimental time. Although all the experiments were handled at near neutral pH, the variation of the
starting pH from 6 to 8 created a remarkable difference between inactivation rates. In photo-Fenton
experiments driven by Fe(II), when pH was 6 or 7, a complete inactivation was achieved in less than 5 min;
at pH 8, in 60 min the inactivation of MS2 was no more than 3.5 logs. When the starting Fe ion was
trivalent, the results of pH 6 and 7 were even more different. At pH 6, viruses were all inactivated in 10
min, at pH 7, the inactivation was completed in 50 min at a ferric dose of 1 mg/L and a pH of 8 did not
favor the photo-Fenton reaction, with inactivation of 0.8 log being attained.
4.3.3. Effect of bacterial competition on MS2 inactivation in wastewater
The experiments mentioned until now were all performed in sterile synthetic wastewater spiked only with
MS2. Normally in wastewater, a number of different microorganisms (bacteriophages, their bacterial
hosts and other microorganisms) co-exist and may play an important role in each other’s life cycle; certain
bacteria can grow and reproduce in the environment, while virus are capable of infecting them. To verify
if the proposed conditions of the photo-Fenton reaction could also apply to a more realistic situation in
which different microorganisms coexist, experiments were conducted in reactors simultaneously spiked
with MS2 bacteriophage and its bacterial host E. coli (Figure 4.5). Since no significant increase of MS2
titers was observed during the course of these experiments the effect of phage infection to the host could
be ignored.
When E. coli alone were exposed to the treatment conditions (figure 4.5a) at which we achieved total
MS2 inactivation (1:1 ratios and 600 W/m2 solar intensity), the viability of E. coli slightly dropped in 60
min, comparing to a 0.5-log decrease when MS2 was present (figure 4.5b). Naturally, viruses consume
oxidants in competition with bacteria. However, since a virion is one or two orders of magnitude smaller
than a bacterium and has a simpler structure, in the photocatalytic system an identical amount of
generated ROS could kill more individual viruses, while E. coli inactivation requires multiple ROS hits to
damage a single cell, and is subjected to endogenous inactivation events. Even among virus strains, the
ones with thinner capsids are more susceptible to inactivation by ROS (Carratalà et al. 2016), therefore
the analogy with bacteria is compelling. In both Figures 4.5a and 4.5b, Fe(II) was again proven to
contribute significantly to bacterial inactivation when MS2 were absent. A noteworthy change was
observed when MS2 were present in the solution, lowering the already small bacterial inactivation with
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the same reagent concentration. This difference is mitigated when higher reactants’ addition was assayed
(0.5:10 and 1:10).
Figure 4.5 – Bacterial competition tests: Inactivation of MS2 and E. coli by the photo-Fenton process.
a) Bacterial inactivation with increasing Fe:H2O2 ratios, in absence or presence of MS2. b) E. coli
inactivation in presence of MS2 and MS2 inactivation in presence or absence of the bacterial host
(Fe:H2O2 ratio 1:1). Higher Fenton reagents addition than 1:1 resulted in <2-min inactivation.
Finally, Figure 4.5b demonstrates the effect the bacterial presence has on MS2 inactivation. The time
necessary for total inactivation was prolonged from 5 to 10 min for MS2 with the presence of E. coli, since
viruses and bacteria are in competition by the generated ROS in the system. Under the condition of steady
stirring, the microbes were homogenously distributed in the water matrix and had random contacts with
systemic ROS. Nevertheless, the viruses could still be totally inactivated in a short period. Furthermore, in
this experiment, 1 mg/L of Fe(II) and 1 mg/L of H2O2 were introduced into the tested system and the
simulated irradiance was set at 600 W/m2. Recent disinfection approaches (Ortega-Gómez et al. 2014,
Ruales-Lonfat et al. 2015) of Fenton reagents application in the micro- to milli-molar range have been
reported so far, while (Spuhler et al. 2010) and (Giannakis et al. 2016d) observed the efficiency of bacterial
inactivation at neutral pH by 0.6 mg/L Fe(II) or Fe(III) and 10 mg/L of H2O2 under 550 W/m2 of solar
radiation. Based on the results above, it can be assumed that a general dose of the Fenton reagents and
115
sunlight exposure for bacterial disinfection is also sufficient for a fast viral inactivation in the wastewater
matrix.
4.3.4. Iron cations solubility in wastewater
Normally, effluents that have been subjected to a biological (or other secondary) treatment, are good
candidates for applying AOPs, such as the photo-Fenton process. Nevertheless, there are some
characteristics that often hinder the process, such as the presence of organic matter, the alkalinity, the
suspended solids and the quasi-neutral pH, among others. However, the organic matter is often
considered acting in a dual manner, with capabilities of complexing metals not only antagonizing the
process, but also able to facilitate the photo-Fenton process (Giannakis et al. 2016a, Giannakis et al.
2016b).
Similarly, the simulated wastewater used in this study was adjusted to neutral pH, at which normally iron
precipitates. We studied the evolution of the photo-Fenton process, in presence of MS2 and Fe(II) or
Fe(III), comparing Milli-Q (MQ) water with the studied wastewater. Over the course of two hours, there
is a slight decrease in the UV-vis absorbance of the bulk in each of the iron additions in MQ (see
Supplementary Figure S3). The reference absorbance belongs to MQ water and 1, 2 and 5 mg/L of Fe(III)
were added for further analyses. Additionally, WW forms more photo-absorbing, and therefore, photo-
active complexes. During a 2-h test, there was practically no decrease in the absorbance, indicating the
stability of the Fe-DOM complexes.
In order to verify the observations, a similar test was performed for 1 hour in WW, with 1 mg/L of either
Fe(II) or Fe(III). The goal of the test was to dissociate the dissolved and total iron (by 0.2 μm filtering)
during an experiment at pH 7 in presence or absence of light. The main two general trends can be
summarized in Figure 6 under the higher values of dissolved iron of Fe(II) (Figure 4.6a) than Fe(III) (Figure
4.6b) as starting iron species, and the slightly lower precipitation rates in the dark tests. On one hand,
Fe(II) readily reacts with the H2O2 in the matrix and then passes to Fe(III), which precipitates faster in near-
neutral values, hence the fast losses in total iron presented with Fe(III) as starting iron species. The
presence of organic matter helps complex the iron, efficiently perform an LMCT, and then possibly re-
complex the iron. This could possibly explain the high iron availability during the tests. Finally, TOC
measurements (data not shown) verify the degradation of the organic matter, however in negligible rates
when low Fenton reagents’ concentration was used. In conclusion, iron, even at small amounts is available
to react and plays an important role in the MS2 inactivation in wastewater.
116
Figure 4.6 – Iron evolution during (dark) Fenton or photo-Fenton process followed by ICP-MS analysis.
A) Fe(II) starting salts. B) Fe(III) starting salts. The dashed lines indicate the dark Fenton experiments,
closed trace symbols indicate dissolved iron and open trace symbols the total iron.
4.3.5. MS2 inactivation modeling
Various kinetic models have been proposed in the literature for microbial inactivation (Marugán et al.
2008). According to Hiatt (Hiatt 1964), the virus survival data can be plotted as ln c/c0 vs. ln t, obtaining
straight lines which are curvilinear for ln c/c0 vs. t. Here c/c0 is the reduction in the infective MS2
concentration and t refers to the treatment time.
Thus, the relationship between c/c0 and t is described as the following function:
(4.14)
where kobs behaves as the observed “relative velocity constant”, corresponding to a pseudo-first-order
kinetic. This model was applied to fit experimental data of the photo-Fenton inactivation at pH 7 under
different conditions (Table 4.2 and 4.3).
However, as seen in before, the curves of MS2 photo-inactivation with Fe(II) and H2O2 proceeded a sudden
decrease at the very beginning of the whole process, and then changed to a tailing pattern if MS2 had not
been totally inactivated. These “biphasic” survival curves can be drawn as two linear components (Hiatt
1964, Kamolsiripichaiporn et al. 2007):
The first stage: (4.14)
117
The second stage: (4.15)
where m is the intercept of the second function on the y-axis.
Table 4.2 – Effect of photo-Fenton treatment [Fe(II)] on MS2 inactivation.
LLight [[W/m22]
Fe(II) [mg/L]
H2O2 [mg/L]
T999.99% [min]
k1,obs [min-1]
r12
t1 [min]
k2,obs [min-1]
m r22
t2 [min]
0 0.5 1 - 2.4152 0.5770 0-5 0.3806 3.6564 0.9903 5-40 300 0.25 0.5 10 7.1218 1 0-2 1.3106 5.9716 0.9146 2-20 300 0.25 1 7.5 7.1218 1 0-2 2.3580 5.0404 0.9686 2-10 300 0.5 1 4 7.1218 1 0-2 300 1 1 3 7.7527 1 0-2 600 0.5 1 2 8.4208 0.9969 0-2 600 1 1 2 20.2658 0.9986 0-0.5 2.818 7.0741 1 0.5-1 900 0.5 1 1.5 9.8486 1 0-2
For different iron starting species of Fe(II) and Fe(III), klight can be determined from the slopes of kobs vs.
[intensity].
Table 4.3 – Effect of photo-Fenton treatment [Fe(III)] on MS2 inactivation.
Light [W/m2]
Fe(III) [mg/L]
H2O2 [mg/L]
T99.99% [min]
kobs [min-1] r2 t
[min] 0 0.5 1 - 0.1606 0.9561 0-60
300 0.25 0.5 - 0.3746 0.9142 0-30 300 0.25 1 - 0.7197 0.9094 0-60 300 0.5 1 - 1.4366 0.9653 0-40 300 1 1 33 2.4794 0.9772 0-30 600 0.5 1 32 1.8140 0.9698 0-60 900 0.5 1 30 2.2894 0.9258 0-30
Ultimately, the three investigated parameters light intensity, Fe(III) and H2O2 concentrations can be
linked together as a single function, within the boundaries of the experimental space, i.e. Intensity [I] =
300-900 W/m2, [Fe(III)]ini = 0.25-1 mg/L, [H2O2]ini = 0.5-1 mg/L), solving the Eqs. 4.14-4.15 and by non-
linear regression fitting we get:
(4.16)
Here klight,Fe(III) corresponds to 0.0016 m2 W-1min-1, kFe(III) to 2.310 L mg-1min-1 and to 0.7996 L mg-1
min-1.
As Eq. 4.16 shows, klight and kFe can be directly applied in the multi-parameter function in Fe(III) systems.
However, in Fe(II)-induced systems cannot be calculated due to the fast inactivation and relatively
118
long sampling time from which the obtained kobs were the same. The correlation between experimental
data and the function is acceptable in the majority of the sets (Tables 4.2 & 4.3). However it must be noted
that during the first two minutes of the experiments, the inactivation was so fast that it was possible to
have already inactivated all the viruses or entered the second phase of disinfection.
4.3.6. Integrated proposal for the inactivation mechanism of viruses in wastewater
Based on our experimental findings, the inactivation presented in one of our previous works (Ortega-
Gómez et al. 2015) and the relevant literature, a modified framework for wastewater is suggested in
Figure 4.7, displaying the possible pathways occurred in virus inactivation, driven by the photo-Fenton
process in wastewater. This framework postulates a modified inactivation pattern in close vicinity to the
virus, also suggested as a caged mechanism by previous works (Nieto-Juarez et al. 2010). Concerning the
MS2 inactivation (Figure 4.7, events 1-6):
1. Sunlight directly affects the viral genome, decreasing its infectivity. Other direct actions involve
the damages to the coat protein, as well as considerable A protein decay (Wigginton et al. 2012).
2. Oxidative stress exerted by H2O2 on the virus is not significant, due to its low oxidation potential,
while under light, due to both its poor photolysis and the presence of DOM that scavenges reactive
hydroxyl radicals the expected contribution is limited. Only by combination with UVA important damages
have been reported (Nelson et al. 2008, Romero et al. 2011).
3. Irradiation of the DOM present in WW generates a small amount of H2O2, O2-, 1O2 and other ROS.
The superoxide radical anion is always generated in lower steady-state concentrations than other ROS.
Also, the presence of these trace metals is reported to enhance its production (Voelker and Sedlak 1995).
As it was reported, O2- has minor contribution in direct MS2 infectivity decrease. On the other hand,
singlet oxygen significantly affects viral infectivity (Kohn and Nelson 2007).
4. In a dark Fenton reaction, Fe(IV) species participates predominantly in the inactivation of viruses;
however, an implementation of solar light greatly enhances the production of HO , which is more
effective in virus inactivation (Nieto-Juarez et al. 2010). When high organic matter concentrations were
involved in previous works, the steady state concentrations and the use of specific HO● quenchers proved
that the HO● contribution of the bulk is low (Kohn et al. 2007). Later works based on caged mechanisms
of inactivation (Chevion 1988, Kocha et al. 1997), suggested that HO● plays a role only when generated in
the vicinity of the virion (Nieto-Juarez et al. 2010).
5. In the wastewater matrix, Fe ions form aquo-complexes by hydrolysis and organo-complexes with
the DOM present. As indicated by Rose and Waite (Rose and Waite 2002), the reaction rate of Fe
complexes towards ROS is the same as for the free ions. The complex formation allows the photo-Fenton
reaction to proceed at neutral pH where Fe(III)-organo complexes are generally stable in particular. They
show higher absorption in the visible range of solar light than aquo-complexes, favoring LMCT reaction
119
that generates ROS under sunlight (Spuhler et al. 2010). The resulting ROS (HO , O2-) have been analyzed
before and the oxidized ligand could possibly proceed with further ROS production (Cieśla et al. 2004,
Šima and Makáňová 1997).
6. Finally, Fe(II) and Fe(III) may directly interact with any of the amino acids in MS2 capsid, forming
organo-complexes. In this case, the Fenton reactions can proceed on the MS2 surface (Kim et al. 2010),
facilitating an LMCT reaction with the viral capsid as sacrificial ligand.
Figure 4.7 – Proposed MS2 inactivation pathway by the photo-Fenton process in wastewater at near-
neutral pH. The events 1-6 are further analyzed in the text.
Fe(II) Fe(III)
Fenton,Photo-Fenton LMCT, Fenton,
Photo-Fenton
ssRNA
Fe(II)Aqua-complex
Organo-complex
Fe(III)Aqua-complex
Organo-complex
,
Lox- & other ROS
Produces
Importantif in
proximity
Dissolved Organic Matter
6 6 1 3 5
4
Fe(IV)
Sunlight (280 – 800 nm)
2
ssRNA
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120
4.4. Conclusions
The use of μm concentrations of Fe and H2O2 has been proven, under certain conditions, enough to
enhance the viral model inactivation in simulated wastewater. The photo-Fenton process in near-neutral
conditions under the presence of scavenging DOM has proceeded to effectively reduce MS2 infectivity,
and the effects of the key parameters of the process were further analyzed.
The photo-Fenton reagents’ concentration was kept at <1 mg/L level, in order to facilitate easier kinetics
studies. Even so, it proves the feasibility of removing MS2 from wastewaters. Fe(II) proven was more
efficient than Fe(III), as its interaction with key components of the capsid enables the ROS production in
the vicinity of the virus. Lowering the ratio among Fe:H2O2 (increasing iron concentration) improved the
disinfection process indicating the importance of iron presence for efficient disinfection. Similar trend was
observed for the pH, which improves iron solubility and therefore its participation to the photo-Fenton
process. Nevertheless, the most important contribution derives from the DOM complexation of iron,
which, apart from the additional ROS production, also mitigates precipitation and facilitates the
maintenance of the initially added amounts. Furthermore, a simple model describing the MS2
inactivation, including the implicated parameters, was effectively constructed.
In conclusion, we identified iron and organic matter as the key factors playing a role in the process when
a complex, multi-target matrix was involved, proposing an inactivation scheme, as well as presenting the
indicative difference of the needs for addition of oxidants. As in actual applications the levels of Fe and
H2O2 addition are higher, the MS2 removal is normally expected sooner than the corresponding bacterial
inactivation. Finally, further work concerning human pathogenic viral strains and other public health
related microorganisms is required before establishing a relative order of removal (compared to other
pathogens) and asserting the efficacy of photo-Fenton.
121
5. Chapter 5 - Castles fall from inside: Evidence for dominant
internal photo-catalytic mechanisms during treatment of
Saccharomyces cerevisiae by photo-Fenton at near-neutral
pH
Published work:
Stefanos Giannakis, Cristina Ruales-Lonfat, Sami Rtimi, Sana Thabet, Pascale Cotton, and César Pulgarin.
"Castles fall from inside: Evidence for dominant internal photo-catalytic mechanisms during treatment of
Saccharomyces cerevisiae by photo-Fenton at near-neutral pH." Applied Catalysis B: Environmental 185
(2016): 150-162.
Web link:
http://www.sciencedirect.com/science/article/pii/S092633731530299X
Supplementary material:
Appendix C
Doctoral Candidate’s contribution:
Main investigator and author.
122
5.1. Introduction
Historically, one of the biggest side-effects of urbanization, was the high concentration of inhabitants in
relatively small areas, which in turn created massive flows of wastewater. It was not until after the
Industrial Revolution that the these wastes started to become a threat against the environment, since up
to that point, the self-cleaning capacity of natural water bodies was able to regulate the incoming nutrient,
organic and inorganic pollution. The last decades, apart from the chemical constituents, a systematic
effort to upgrade the wastewater treatment plants has been undertaken, in order to eliminate
microbiological contaminants contained in wastewater. As first approaches, chlorination, peracetic acid
and other chemical methods were employed (White 2010), gradually replaced by more eco-friendly
methods (such as UV or ozonation) due to the lower harmful by-products connected with their
application.
Moreover, hospital wastewater has been categorized as a main contributor of chemical substances (drugs,
wastes) (Verlicchi et al. 2012) and microbiological agents normally not encountered in municipal
wastewater, such as high concentration of antibiotic resistant bacteria, viruses, yeasts or fungi (Li et al.
2007, Prado et al. 2011, Schwartz et al. 2003). The similar origin of wastewater in health facilities led the
practitioners to apply one sterilization step before leading the treated wastewater in the municipal
wastewater treatment plants (Emmanuel et al. 2004). During the last years in Europe, there is an
increasing demand of treatment plants specifically designed for hospitals, taking into account the special
form of pollution contained (Lienert et al. 2011). Nevertheless, in less favorable regions of the world, these
wastewater treatment plant facilities are either a luxury, non-existing or have never operated properly.
As a result, the wastewater is directly discharged into nature and the natural water bodies are
transformed into disease carriers. Bacterial induced illnesses, such as diarrhea, viral or fungal-related
infections have been encountered, problems craving a simple, cheap and sustainable solution (Gibson
2014, McGuigan et al. 2012).
The advanced oxidation processes (AOPs) have emerged during the last years as a practical and in some
cases, easily applicable solution, as a barrier to stop pollution in contaminated drinking water sources. As
a common denominator, the extremely oxidative hydroxyl radical is produced, and secondarily, other
reactive oxygen species (Ruales-Lonfat et al. 2014). Ozonation (at basic pH), heterogeneous photocatalysis
by TiO2, UV-induced production of HO● by the homolytic disruption of H2O2 and the iron-catalyzed radical
induction are some of the most popular AOPs in decontaminating water or wastewater (Comninellis et al.
2008, Poyatos et al. 2010). Especially the Fenton reaction, and its photo-enhanced version, gained much
merit during the last decade, after the proof of its considerable effectivity at near-neutral pH (Rincón and
Pulgarin 2006); in the past, its acidic pH-bound character acted as a limiting step towards its application
123
against microorganism removal. Its low cost and easy application has proven itself a powerful ally in sunny
regions around the globe (Ndounla et al. 2014, Ndounla et al. 2013).
A significant number of studies discuss the efficiency of the Fenton reaction as an antibacterial agent,
using most commonly E. coli, but also Enterococci, and Salmonella (Ndounla et al. 2013, Ortega-Gómez et
al. 2013, Ruales-Lonfat et al. 2015, Spuhler et al. 2010). The efficiency of the Fenton reaction was lately
tested for the inactivation of viruses, such as MS2 Coliphage and Echovirus (Ortega-Gómez et al. 2014).
Although prokaryotic unicellular microorganisms have been more studied, due to their omnipresence in
the environment and their impact on health, expanding works on other groups of microorganisms is
necessary. The impact of eukaryotic microorganisms on environment and human health is not negligible.
The effects of photocatalysis on fungal cell survival has been showed for environmental species, like
Penicillium, Fusarium, and Aspergillus that are frequently recovered from water and soil (Brinkman et al.
2003, Park et al. 2015, Pigeot-Rémy et al. 2012) and for yeast species like Candida closely associated to
human opportunistic infections (Thabet et al. 2014).
In eukaryotic cells, there are significant structural modifications compared to prokaryotes which may
facilitate difference in interesting traits, disinfection-wise, such as resistance, higher stress responses and
repair mechanisms (Temple et al. 2005). A series of photocatalysis studies using TiO2 have focused on F.
solani as a model of multicellular microbial structure (Sichel et al. 2009, Sichel et al. 2007b), and at the
unicellular level on Saccharomyces cerevisiae as a model for oxidative response (Thabet et al. 2014,
Thabet et al. 2013). It was proven that there is limited penetration of TiO2 nanoparticles into the yeast
cell, and that photocatalysis induces the establishment of an intracellular oxidative environment (Thabet
et al. 2014). In bacteria, the effect of an internal Fenton mechanism has been brought to surface (Ruales-
Lonfat et al. 2014), complementing the external pathways but yet, it is still unclear how it would act, when
yeast cells are the target of the Fenton reaction.
In this work, we have used S. cerevisiae, as a model of eukaryotic microorganisms, and photo-Fenton as
the antimicrobial AOP. The mechanisms of yeast inactivation by photo-Fenton process at near-neutral pH
were investigated. The reactions were fueled by different iron sources, namely iron sulfate and iron
citrate, in presence of H2O2, under simulated solar light. The different inactivation pathways were
interpreted by using flow cytometry, and assessment of the damage at both DNA and protein level was
also performed. DNA and cell wall protein damages were depicted by electrophoresis, to elucidating the
photo-Fenton mode of action.
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5.2. Materials and Methods
5.2.1. Chemicals
Ferrous sulfate heptahydrate (FeSO4˙7H2O) (Riedel-de Haën 99-103.4%); Ferric chloride (FeCl3) (98% carlo
erba), Trisodium citrate dihydrate (Na3C6H5O7.2H2O) (99% Merck); Sodium hydrogen carbonate (NaHCO3)
(analytical grade, Merck); Hydrogen peroxide (H2O2) 30% w/v (Riedel de Haën); Titanium (IV) oxysulfate
(TiOSO4) (Fluka); Sodium hydroxide (NaOH, 98%) and hydrochloric acid (HCl, 36.5%), were purchased from
Sigma-Aldrich, Switzerland. The spin-trap, 5,5-dimethyl-1-pyrroline-N-oxide (DMPO), was purchased from
Enzo Life Sciences (ELS) AG (Switzerland). All solutions were prepared immediately prior to irradiation
with the use of Milli-Q water (18.2 MΩ-cm).
5.2.2. Fe–citrate complex and Goethite preparation
Fe–citrate complex was prepared according at modified patent European from Bayer (Antonini and Vidic
1994). Ferric chloride (4.1 g) and sodium hydrogen carbonate (3.0 g) were dispersed in 50 mL of distilled
water and dissolved therein by stirring. This solution was degassed under vacuum for 2 hours followed by
constant stirring and Trisodium citrate dihydrate (4.0 g) was added. The color of the solution turned to a
pale brown. The solution was stored in the dark for 24 h. Then, 40 mL of methanol was added to the
brown solution under constant stirring at 25 °C and a brown precipitate was formed. The resulting solution
was centrifuged (5 min at 5000 rpm) to remove the precipitate, and the clear supernatant suspension was
separated by filtration. The precipitate was washed with methanol at least three times and dried under
vacuum at room temperature. Goethite preparation and characterization was analytically presented in
previous works of our group (Ruales-Lonfat et al. 2015).
5.2.3. Yeast strains and growth media
The laboratory strain S. cerevisiae (BY4742) was used for all yeast inactivation experiments. The strain was
maintained on YPD medium (1% yeast extract, 1% peptone, 2% glucose, 2% agar for plates). Yeast cells
were grown in liquid YPD overnight under aerobic conditions with constant shaking at 28 °C. The yeast
culture growth was checked by measuring optical density at 600 nm using a spectrophotometer. For all
experiments, cell samples were collected at the beginning of the exponential growth phase (OD600 = 1,)
washed twice and suspended in the photoreactor in 20 mL of sterile ultra-pure (UP) water (Simplicity™,
Millipore), resulting into a concentration of 107 cells/mL.
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5.2.4. Photo-inactivation experiments
All yeast inactivation experiments were performed in Pyrex reactors (4 cm x 9 cm, 100 mL). The Pyrex
reactors containing the yeast suspension in Milli-Q water (approximately 107 CFU/mL) were placed in the
dark at 25 °C under magnetic stirring for at least 30 min to let the yeast adapt to the new matrix and to
allow the die-off and equilibration of the most stress-sensitive species.
The following systems were analyzed for the inactivation effect on yeast. (i) photo-Fenton process
mediated by Fe–citrate (0.6 mg Fe/L) at pH: 6.0 or 7.5; (ii) photo-Fenton process mediated by FeSO4 (0.6
mg Fe/L) at pH: 5.5 and 7.5; and (iii) control experiments: H2O2/dark; light alone and H2O2/light. Goethite
addition (0.6 mg Fe/L) was assessed complementarily, to assess the function of the iron after its
precipitation in the near-neutral environments. In the experiments iron was added to a yeast suspension.
Then, the pH was adjusted depending on the experiment. Neighboring near-neutral values were assayed
to better investigate the behavior of a system which partially permits soluble Fe and compare with realistic
pH. Finally, H2O2 (10 mg/L) was added to the reactor as the last component.
Experiments were carried out using a solar simulator CPS Suntest System (Heraeus Noblelight, Hanau,
Germany). This solar simulator was equipped with a basic uncoated quartz glass light tube, a filter E and
an IR screen (neither UVC nor IR is reaching the sample, the intermediate wavelengths are a simulation of
the solar radiation); more information can be found at (Giannakis et al. 2015a, b). The irradiance was
measured by a spectro-radiometer, Model ILT-900-R (International Light Technologies) and corresponded
to 820 W/m2 of light global irradiance (from which ~0.5% UVB, ~5% UVA is emitted). Temperature was
monitored and always remained <38°C.
5.2.5. Cultivability assays
Samples were collected at regular intervals during yeast inactivation reaction. Serial dilutions were
immediately made in liquid YPD medium and spread onto YPD agar plates. After 2 days of incubation at
28 °C, the colony forming units (CFU) detected on appropriate dilution plates were counted, in order to
determine the concentration of surviving cells. Triplicate plating was performed for each dilution of the
samples. All experiments were performed in triplicates and the results presented in the graphs are the
average value (<5% statistical error).
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5.2.6. Analytical methods
5.2.6.1. Optical epifluorescence microscopy
Microscopy observations were performed using Axioscop 2 plus Zeiss optical microscope equipped with
AxioCam MRm camera. Data were collected using AXioVision software.
Cell viability was investigated using PI (Propidium iodide, Invitrogen, ex/em 490/635 nm) and CFDA-AM
dye (Carboxyfluorescein diacetate- acetoxymethyl, ROCH, ex/em 492/517 nm). PI enters only cells with
damaged cytoplasmic membranes, whereas CFDA-AM enters all cells and is non-fluorescent until it is cut-
off by active cytoplasmic esterases. CFDA-AM reflects cell metabolic activity. Treated cell samples (100 μL)
were diluted in PBS to 106 cells/mL. After addition of dyes (1 μg/mL PI and 5 μg/mL CFDA-AM), the mix
was incubated for 20 min at 37 °C.
5.2.6.2. Flow cytometry
Flow cytometry was carried out using FACS CantoII instrument (BD Biosciences) fitted with three lasers:
blue (488 nm, aircooled, 20 mW solid state), red (633 nm, 17 mW HeNe) and violet (405 nm, 30 mW solid
state). Diffracted light (related to cell surface: Forward scatter FSC) and reflected light (related to
granularity: Side scatter SSC) of blue laser, as well as CFDA-AM and PI, were collected. Data from
10,000 cells were collected using FACSDIVA software (6.1.2 version, BD Biosciences).
5.2.7. Biochemical methods
5.2.7.1. DNA extraction and analysis
Yeast chromosomal DNA was extracted from 2 mL of stationary phase YPG culture at 28° C and 150 rpm.
Cells were collected by centrifugation 30 s at 16000 g, washed in 0.5 mL of sterile water and suspended
in 0.2 mL of lysis buffer (2% Triton X-100, 1% SDS, 100 mM NaCl, 10 mM Tris-HCl pH 8,0, 10 mM EDTA pH
8.0). Glass beads (0.5 mm diameter, 0.4 g) and phenol chloroform isoamylalcool (0.2 mL) were then
added. Samples were vortexed for 5 min and 0.2 mL TE pH 8.0 (10 mM Tris-HCl pH 8.0, 1 mM EDTA, pH
8.0) was added. After centrifugation (10 min, 16000 g) at room temperature, the supernatant was
transferred into a new tube and 0.4 mL chloroform was added. After centrifugation for 2 min at 16000 g,
the aqueous phase was transferred and 4 μL of 10mg/mL RNAse were added. Samples were incubated at
37°C for 15 min and DNA was precipitated with 1 mL 100% ethanol and incubated for 10 min at -20°C.
After centrifugation (10 min, 16000 g), the pellet was solubilized in 0.4 mL TE pH 8.0. The samples’ DNA
was quantified using a nanodrop spectrometer at 260 nm. DNA was loaded on a 0.8% agarose gel and
separated by electrophoresis according to (Sambrook et al. 1989) and visualized under UV irradiation after
staining the gels with ethidium bromide (1μg/mL).
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5.2.7.2. Protein extraction and analysis of protein profiles
To analyze the proteins, the protocol described by Thabet et al. (Thabet et al. 2014) was followed. SDS-
PAGE, was performed with 10% (wt/vol) polyacrylamide gels as decribed by Laemmli (Laemmli 1970). 100
μg of proteins were loaded in each well. LC/MS (HPLC Ultimate 3000; Dionex coupled with LTQ Velos;
Thermo Scientific) was used to identify the proteins, followed by discoloration of the bands of interest (by
trypsin digestion). A second MS was undertaken for the 10 most significant peaks, and analysis through
Proteome Discoverer software (Thermo Electron). The Mascot software (v2.3) was finally used to perform
a UniP_Sacchar_cerev search, with the following criteria applied: MS/MS ion search, electrospray
ionization (ESI-TRAP), trypsin (digestion enyme), carbamidomethyl and oxidation (modifications), max 2
missed cleavages, peptide and fragment mass tolerance ±1.5 and ±0.6 Da, respectively, ion scores > 37,
P<0.01 (statistical identification significance).
5.2.8. Experimental Planning
The strategy for unveiling the complex inactivation mechanism was as follows. In principle, the photo-
Fenton process was stepwise constructed: first light only, then addition of H2O2 and finally addition of the
iron source. This construction was evaluated in three levels: i) inactivation efficiency measured by
cultivability, ii) localization of the damage (internal, external) and iii) identification of the targets deriving
from the various processes.
5.3. Results and Discussion
5.3.1. Preliminary assays in simulated wastewater
Initially, the efficacy of the photo-Fenton process in S. cerevisiae inactivation in simulated wastewater was
assayed (recipe and conditions identical to Chapter 4), and the results are presented in Figure 5.1.
Although solar light exposure in a 3-h period failed to decrease the viability significantly, the addition of
H2O2 inflicted a 2 to 3-log decrease as the addition increased from 10 to 25 mg/L. The addition of both Fe
(di- and tri-valent starting iron species) and H2O2 under illumination inflicted a 4 to 6-log reduction in the
population, indicating that the photo-Fenton process is a prominent technique towards the elimination
of this specific pathogen, even in the presence of organic matter and ROS scavengers (see chapter 4 for
composition and simulated WW characteristics). However, the focus of this work is to elucidate the
underlying mechanisms of S. cerevisiae inactivation, hence for simplification and interference avoidance
purposes, the following detailed study was conducted in MQ water.
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Figure 5.1 – Overview of the photo-Fenton tests in simulated wastewater.
5.3.2. Cultivability assays – Efficiency of treatment in MQ water
Figure 5.2 summarizes the various photocatalytic inactivation tests carried out in the framework of this
work in MQ water. Figure 5.2a contains the heterogeneous and homogeneous photocatalytic systems
with the respective blank tests, while Figs. 5.2b and 5.2c depict the effect of pH on the efficiency of the
(homogeneous) photo-Fenton action.
More specifically, in Figure 5.2a the boundary conditions, concerning the oxidative stress applied to S.
cerevisiae are shown first ( trace). Hydrogen peroxide at high concentrations has been reported to have
detrimental effect on the survival of S. cerevisiae (Oyane et al. 2009). Normally, H2O2 acts on its cell wall
and plasma membrane, causing carbonylation and thiolation of surface proteins (Cabiscol et al. 2000,
Costa et al. 2002, Grant et al. 1999). The fungal wall is suggested to protect from diffusion of H2O2 into
the cell of F. solani (Sichel et al. 2009), with increasing thickness and efficacy as the cell ages (Sousa-Lopes
et al. 2004). Here, the control test was performed at 10 mg/L initial H2O2 concentration. As a result,
negligible inactivation was observed during the monitoring period (2 h).
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Figure 5.2 – Overview of the photocatalytic inactivation tests and their respective controls. a) The
plots describe the cultivability evolution over time. b) Comparison between pH 5.5 and 7.5 for the
FeSO4-assisted photo-Fenton system. c) Comparison between pH 6.0 and 7.5 for the iron citrate-
assisted photo-Fenton system. Standard deviation < 5%.
When light was introduced to the system, significant inactivation of yeast cells was initiated ( trace).
The fungal kingdom is known to be affected by solar (Sichel et al. 2007a) or pulsed light (Takeshita et al.
2003), which essentially has similar mode of action, but higher intensity. After 30 min of minor
inactivation, resembling the shoulder period of inactivation found for E. coli (Giannakis et al. 2015a, b), a
linear (at log-scale) pattern was observed, without significant tailing. The necessary dose to initiate the
linear inactivation was 72 kJ/m2 and 288 kJ/m2 were required for total inactivation, respectively;
compared to other (multicellular) fungi, this is 40% less (Sichel et al. 2007b). The emitted light from the
solar simulator includes wavelengths at both UVB and UVA regions. Although UVB is notably less than the
UVA (0.5% compared to 5%) its biological effects are significant (Giannakis et al. 2014a, b). UV light affects
both external sites (cytoplasmic membrane) and internal ones, such as the enzymatic activity and the
genomic structure (Schenk et al. 2011). Pfeifer et al. (Pfeifer et al. 2005) have shown that artificially
irradiated cells present a higher percentage of UVB-induced lesions, namely CPDs (cyclobutane pyrimidine
dimers), rather than (6-4) photoproducts from type I or II reactions, that UVA is held usually responsible.
However, UVA can i) produce H2O2 (under certain conditions) by activating oxidases (Hockberger et al.
1999) ii) or, release iron from ferritins (Pourzand et al. 1999) and Fe/S clusters (De Freitas et al. 2003); this
ends up in initiating an internal (photo)Fenton process. Although DNA has low absorbance in the UVA
a)
b)
c)
130
region (maxima around 260) (Lindberg and Horneck 1991, Schenk-Meuser et al. 1992); strand breaks have
been reported, supporting this hypothesis, and guanine to cytosine transversions (Pfeifer et al. 2005).
Finally, apoptotic responses have been reported, and are initiated as a result of disrupted or altered yeast
life cycle or UV sensitivity (Chen et al. 2014, Del Carratore et al. 2002).
The last control test of the system assessed the combined action of simulated solar light and hydrogen
peroxide ( trace). Compared to the simulated solar light test, the required time for 6-log inactivation
has decreased almost in half (75 min instead of 120) and the shoulder length has also been decreased to
10 min from 30. In this experiment, notable consumption of H2O2 was observed compared to the dark test
(see Supplementary Figure S1). Since it is known that the cleavage of H2O2 with the subsequent formation
of hydroxyl radicals is unlikely to be achieved within the solar spectrum (Zapata et al. 2010), the possible
inactivation mechanism is as follows: the action of H2O2 and UV on the external proteins affects the
composition and stability of the membrane, and subsequent regional changes in permeability occur. Since
the H2O2 can now enter the cell, the internal Haber-Weiss reactions are enhanced (Spuhler et al. 2010).
The first step of the catalytic cycle involves reduction of ferric ion to ferrous (Eq. 5.1):
● (5.1)
The second step is the Fenton reaction (Eq. 1.8):
(1.8)
Net reaction (Eq. 5.2):
● ● (5.2)
This hypothesis is reinforced by data acquired by F. solani, where notable decrease of H2O2 occurred,
during UVA irradiation (Sichel et al. 2009), and entrance of H2O2 in the spore was highly probable. The
second action mode suggests a damage in the oxidative stress regulation mechanisms in the cell by the
action of UV light, such as SOD or CAT, followed by accumulation of ROS into the cell. If the SOD, the
responsible for regulation of superoxide radical ● inside the cell is no longer functional, it can lead to
the accumulation of ● . Superoxide radicals attack the DNA (Keyer and Imlay 1996), lead to the
accumulation of H2O2 and lately, ● has been suggested that in aqueous environments can lead to the
formation of hydroxyl radicals ( ●) (Ruales-Lonfat et al. 2015, Xu et al. 2013). CAT is also strongly
affected by light (Imlay 2008) and suspending its functions can cause internal stress by over-accumulation
of H2O2. Once the internal regulation mechanisms have been dropped, the cells cultivability is decreasing
dramatically, succumbing to the internal and external stresses initiated by UV and H2O2.
The remaining inactivation curves describe the photo-assisted Fenton processes undertaken in this study,
marked with the square traces. Iron in the form of FeSO4 ( trace), iron citrate ( trace) and iron oxides,
as goethite ( trace), were added to the solution 30 min prior to illumination, and H2O2 addition (and
131
light supply) indicated the initiation of the experimental assay time. According to the different starting
forms of iron in the solution, different responses were expected and subsequently monitored in the
system. In general, contrary to solar only or solar/H2O2 systems, an hour or less was required to achieve
total inactivation. In addition, apart from the goethite-powered photo-Fenton process, no significant
delay (shoulder) was measured; almost constant inactivation kinetics were observed. An estimated order
of efficiency according to the initial iron source was as follows: Goethite < FeSO4 < Citrate.
Goethite: Goethite is one of the most abundant forms of iron in nature (Ruales-Lonfat et al. 2015) and
can play a significant role in S. cerevisiae inactivation as heterogeneous catalyst in presence of H2O2
(Ruales-Lonfat et al. 2014). At near-neutral pH, when iron salts (such as the ferrous sulfate used here) are
added in presence of H2O2, zero-charge ferrous complexes [Fe(OH)2] are formed, which are very sensitive
to oxidation and rapidly form solid ferric (hydr)oxide compounds, such as goethite and lepidocrocite
(Ruales-Lonfat et al. 2014). Therefore, according to the process described in our previous work, goethite
was prepared (Ruales-Lonfat et al. 2015) and used in this study. It is necessary to differentiate the actions
attributed to iron oxides, at least for the cultivability assays, as their formation in near-neutral
environments is ubiquitous. As explained below, goethite contribution is divided to action as a photo-
excited semiconductor with the cells, or a heterogeneous photo-catalyst.
Goethite, in absence of H2O2 has demonstrated semiconductor properties, towards bacterial inactivation
(band gap: 2.1 eV). Even more, photo-activity has also been reported (Leland and Bard 1987). Hence, HO●
radicals can be formed only by presence of light, and the particles that could adsorb onto the yeast surface
due to negative charging (Dunlap et al. 2005, Polo-López et al. 2010) may contribute to surface holes and
aid in inactivation. Furthermore, apart from the oxidative damage from the holes, the iron oxides can lead
to damage on the cell surface through another semiconductor action mode. The goethite particles bound
in the surface of the yeast cell are illuminated and electron excitation is following. Oxygen plays the role
of electron acceptor, leading to superoxide radicals ( ● ) and subsequent reaction with water locally
produces hydroxyl radicals (Ruales-Lonfat et al. 2015). In our experiments, a stronger electron acceptor
(H2O2) is present and the heterogeneous (Fenton with Fe-oxide as iron source) action mode is more likely
to affect the inactivation process. Nevertheless, we cannot neglect the possibility of semiconductor
pathways’ contribution to cell damage.
In presence of H2O2, the following action modes are more prominent. Firstly, radicals’ production is
expected, through the excitation of electrons on the surface of the oxide, and transformation of H2O2
through the following reaction:
→ ● (5.3)
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The other pathway includes a heterogeneous photo-Fenton mechanism for hydroxyl radical production,
where H2O2 is responsible for initiating a series of reactions, leading firstly to HO2● when in contact with
Fe3+ from iron oxides’ surface, reducing it to Fe2+. Fe2+ participates in the Fenton reaction and a cycle is
initiated, described by the following reactions (Ruales-Lonfat et al. 2015) (>Fe corresponds to the iron in
the surface of the goethite particle).
● (5.4)
● (5.5)
● ● (5.6)
● (5.7)
Finally, Fe3+ could form complexes with organic compounds in the cell wall (Polo-López et al. 2014, Polo-
López et al. 2013, Spuhler et al. 2010). Through ligand-to-metal charge (LMCT) transfer, Fe3+ is reduced,
leading to Fe2+ and initiating the Fenton reaction anew, in presence of light.
● (5.8)
Iron sulfate: FeSO4 was used as a starting source of iron, where Fe2+ is available to react with H2O2,
according to the following reactions:
(1.8) ● (5.9)
● (5.10) ● (5.11)
The treatment here takes place under (simulated) solar light. Hence, regeneration of the iron catalyst is
taking place according to the last two equations (Eqs. 5.10-5.11). Equation 5.11 takes into account the
possible complexes with organic by-products (R) deriving from the initial yeast cell wall attack, which can
maintain the iron available in solution for the reaction, as follows:
Fe2+ feeds the photo-Fenton cycle outside the cell, damaging the external membranes by the ROS
produced, in the same way the HO● radicals do due to heterogeneous photocatalysis with iron oxides.
133
However, after addition of FeSO4 at neutral pH, Fe2+ has a half-life of minutes before its oxidation in Fe3+,
and the subsequent precipitation as iron oxide (Barona et al. 2015). It also has been reported to diffuse
through cell walls (Polo-López et al. 2014, Spuhler et al. 2010), increasing the inactivation efficiency
through radicals’ production. Contrary to bacteria, S. cerevisiae do not produce any siderophores to
facilitate this transport, but there are i) surface binding mechanisms, ii) opportunistic use of siderophores
from other microorganisms (in real water samples) as well as reductive and non-reductive iron transport
mechanisms reported in literature (Gaensly et al. 2014, Lesuisse et al. 2001, Stearman et al. 1996, Yun et
al. 2000).
After diffusion, although iron does not affect the carrier proteins per se, it blocks their synthesis and the
transport energy resources (Khansuwan and Kotyk 2000); as a result, halving of the ATPase was observed.
Fe2+ is also proposed to bind to internal membranes to participate in the internal (photo-Fenton) process
and further promotes the superoxide radical production, ultimately increasing HO● radical production
(Sigler et al. 1998). The free iron inside saccharomyces is in Fe3+ form (Srinivasan et al. 2000), so reduction
to Fe2+ (and further HO● production) by LMCT or by the superoxide radical is also expected (Temple et al.
2005).
Finally, since the iron is not likely to remain in solution for long (Barona et al. 2015), the heterogeneous
action mode due to the formation of iron oxides is highly likely to be the driving force, after a certain
point. For simplicity reasons, we do not repeat here the heterogeneous and the semiconductor action of
the iron oxides as explained before; nevertheless their participation cannot be neglected.
Iron citrate: The experiments with complexed iron (by citrate ligand) simulate the mild chelating
properties of naturally available iron in natural conditions. These tests presented the fastest inactivation
rates for the operated pH region (pH = 6.0). In principle, the optimal efficiency for the photo-Fenton
reaction is found at pH = 2.8. If the experiments with FeSO4 were performed at that pH the efficiency
would have significantly improved. However, the acidification costs for treatment and the subsequent
neutralization necessary for use of the water after treatment demands viable solutions at the neutral pH.
Iron citrate has been successfully used in high pH (up to 8) for pollutants’ degradation (Katsumata et al.
2006, Trovó and Nogueira 2011) and bacterial inactivation (Ruales-Lonfat et al. 2016), therefore its
success is promising also for drinking water disinfection, since its related toxicity is very low (Silva et al.
2007). Here, the citrate complexes lead to higher solubility and stabilization of iron cations in the solution.
In general, the action mode of citrate can be categorized as a homogeneous Fenton promoter. The
generation of HO● radicals is induced by photoactive [FeOH-cit]– complex, which is the main species
formed at neutral pH (Chen et al. 2011); first a LMCT transition and then a Fenton reaction take place. The
(photoactive) [FeOH-cit]– complex will generate a ligand radical (HGA2●─) and Fe2+, which will in turn result
134
to superoxide radical anion and HO● production, respectively. This Fe2+ can also participate in the photo-
Fenton cycle mentioned before for Fe2+ from FeSO4.
pH dependence: In order to test the efficiency of the two processes initiated by FeSO4 and Fe-cit and
verify the extent of homogeneous, heterogeneous action mode and side-effects of iron addition, assays
in higher pH (7.5) were initiated. In Figs. 2b and 2c, the results for FeSO4 and Fe-cit are summarized. As a
rule of thumb, increase of the pH leads to faster precipitation of Fe3+, and lower inactivation rates are
expected. Nevertheless, for FeSO4 the reaction duration was not affected and 45 min were necessary to
completely inactivate the Saccharomyces. In pH 7.5, the oxide forms of iron are favored, and since the
overall inactivation rate was not affected, it indicates the significance of the heterogeneous process in
yeast inactivation.
The iron citrate inactivation was more affected by the pH increase. Since the iron and the citrate complex
were synthesized by a 1:1 ratio, after the ligand to metal charge transfer and citrate’s sacrifice, iron is
more likely to precipitate at neutral pH, rather than re-complexing with another citrate ligand. Therefore,
the homogeneous action is not affected. The difference in the inactivation rates could also probably a
consequence of the side-reactions influenced by the citrate ligand, which acts as an extra target for the
non-selective oxidative species generated. Our overall suggestion is that the reactions initiated by extra
iron intake are limited by the pH increase, and the subsequent oxide formation.
5.3.3. Flow cytometry results – Localization of damage
Very often, the viability assay through cultivation, works on the assumption that viable cells are the one
able to reproduce. Hence, cultivability is the required measurement. However, Davey in her recent review
emphasizes on the problematic dependence on these measurements, since microbial cells are not
classified only as “live/dead”, but cryptobiotic, dormant, moribund and latent states have been suggested
throughout the years (Davey 2011). Therefore, flow cytometry combined with CFDA/Propidium Iodide
staining has also been used in this study, for an assessment of the type and the extent of damage at yeast
cells. Indicative results of one process, are presented in Figure 5.3.
The staining protocol used allows the identification of living cells (appearing green in P2 quadrant) dead
cells (red in P4 quadrant), as well as the unlabeled and intermediate states in quadrants P1 and P5
respectively (Figure 5.3i). The green staining is an indirect indication of a living cell, since an acetoxymethyl
ester of the 5-carboxyfluorescein diacetate (CFDA) added is entering the cell through the membrane, and
once inside, gets hydrolyzed into acid and alcohol by non-specific enzymes (esterases) resulting in a
fluorescent green stain. On the contrary, the Propidium Iodide (PI) test indicates the non-viable cells. The
propidium ion is excluded from permeating the membrane and the loss of this ability suggests a loss of
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viability. Even so, literature suggests cases that this is not definitive (Davey and Hexley 2011) and live cells
can get the red staining while maintaining their viability; up to 7% of these cells can still perform repair.
Figure 5.3 – Control tests and an indicative presentation of the flow cytometry results evolution,
during photo-Fenton reaction, at pH = 5.5.
Figure 5.3ii demonstrates the evolution of cell state in 30 min of exposure to light and the addition of the
photo-Fenton reagents, at pH = 5.5. This case is presented as an indicative test, and the results of the
other tests will be summarized instead (Figure 5.4). At time 0, 99% of the cells fall within the live state,
and 1% to the other states; we remind that 30 min have preceded all experiments before illumination, to
allow die-off of the most sensitive cells and acclimatization time for the rest of the cells. The intermediate
cell state appearing in quadrant P5 in Figs. 5.3ii-b and c, indicate vital cells but with compromised
membrane. As the exposure time passed and cells were subjected to the actions induced by the photo-
Fenton reaction, viability, as it is defined in this test, diminished within 30 min. For the rest of the tests,
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the conventional graphs will be presented instead. By processing the data (number of cells) on CFDA and
PI staining for the first 30 or 45 min of the treatment, a correlation was found among the classic
cultivability assay and the flow cytometry results (more information can be found in the Supplementary
Material, Figure S2 and Table S1).
In our work, for each different test (hv, hv/H2O2, photo-Fenton with FeSO4 and Fe-cit as iron sources), flow
cytometry has been performed and the results were always juxtaposed with the cultivability assays
presented before, for comparison. An overview of the CFDA decrease and the PI increase during the
various experiments: hv, hv/H2O2, photo-Fenton (FeSO4 - pH = 5.5 & 7.5, Fe-cit – pH = 6.0 & 7.5) can be
found in the Supplementary Figure S3, while the analytical data will be presented in Figure 5.4. Following,
an analytical explanation of the results of CFDA, PI and the intermediate cell state is presented, with
suggestions on the inactivation mechanisms for each case. As this process is constructed in a step-wise
manner, the explanations and the mechanisms suggested in the first steps (solar degradation and H2O2
oxidation), will not be repeated in the more complex systems.
Simulated solar light: During exposure of S. cerevisiae to simulated solar light, the changes in esterase
activity and membrane permeability were recorded and summarized in Figure 5.3a. Firstly, we compared
the time necessary for 50% and 90% reduction of the initial microbial load. As it appears, the cultivability
assays indicate a required time somewhat higher than 30 min. However, CFDA and the PI-stained cells are
almost in agreement (6% intermediate state cells) at 50 minutes. For 1-log reduction there is a small
convergence between the two methods, with 10 min difference instead. Nevertheless, the remaining
population is consistently underestimated by the cultivability assays, and viable cells that are not able to
form colonies are left out of the estimation.
A critical point in this study is the timeframe of 45 min (Figure 5.4a), where the number of viable cells, but
with compromised membranes is the highest (11.5%). Therefore, the principal mechanism of light-
induced inactivation is an internal process. More specifically, the proposed mechanism is as follows:
1) If we consider either CFDA or PI staining as the accurate viability assay, and not cultivability, the
inactivation presents a shoulder, a latency (in linear scale). Therefore, there should be either an
accumulation of damage before inactivation or the specific type of damage can be repaired.
2) The low accumulation of purple stains during flow cytometry (11.5% versus 26% PI-stained or
generally 37.5% esterase inactive), suggests that lipid peroxidation is limited, and external
proteins are rather intact. Also, it could signify that the cells are inactivated through a failure in
their internal functions.
3) The above indicate that this result is probably, the effect of the actions of UVB and UVA light on
(nucleic/mitochondrial DNA and internal enzymes, respectively.
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hv/H2O2: The flow cytometry results for the hv/H2O2 treatment of S. cerevisiae are summarized in Figure
5.4b. In principle, the shapes of the curves are very similar to the ones already shown during the solar-
only exposure. The cultivability decreases rapidly in time, and the 4-log reduction time dropped to 30 min
(instead of 60). However, the CFDA/PI staining levels presented the same lag in the beginning, with
different time to reach >99.5% (30 instead of 45 min). Also, the intermediate cells were at the same
percentage with the solar-only process. The main difference that modifies the inactivation mechanism
lies in the higher levels of non-viable cells:
1) The latent character of inactivation indicates the necessity to accumulate damage prior to
inactivate the cells. The shoulder length is again around 30 min, indicating similar accumulation
of photo-induced damage.
2) The low number of intermediates could mean a low peroxidation-related killed cells. Hence, there
are not many vital cells with compromised membrane.
3) In 45 min, there were significantly more inactivated cells compared with the solar-only process,
with the same number of intermediate cell-states. Therefore, there is a synergy in the action of
light and H2O2.
4) Since the suggested mechanism is the CPD-formation in DNA and enzymatic failure (CAT, SOD),
the mutations and enzymatic activity loss could increase the permeability of the membrane, thus
enhancing the H2O2 diffusion into the cell.
5) The entry of H2O2 in the cell enhances the oxidative damage, now unable to be controlled by SOD,
or even more, enhancement of the internal Fenton process taking place into the cell.
Photo-Fenton with FeSO4, at pH = 5.5 and 7.5: Figs. 5.4c and d summarizes the evolution of cultivability,
plus CFDA and PI staining through time. The photo-catalytic process is profoundly more efficient than
solar, or hv/H2O2. The time mark of 15 min offer a solid ground for comparisons. At pH 5.5, the level of
viable cells is 86%, compared with the 94% of the higher pH. Also, 4-log of cultivability loss occurs at 20
min (here recorded at 30 min for pH 7.5 due to sampling interval settings) and total inactivation takes
place at 30 min.
For the samples treated at pH = 5.5, there is a latent period marked with CFDA staining but probably the
levels of viability are similar (Figure 5.4c); the cultivability is almost equal but the marked difference is at
the intermediate cells, were 5% and 40% yeasts with compromised membranes appear, for pH 5.5 and
7.5, respectively. At 20 min, the peak of intermediate cells appear for pH 5.5, reaching 30%, and 67% dead
cells (PI stain) but the striking difference at pH 7.5 is that even 5 min earlier, the peak of intermediate cells
is reached, almost double in quantity (55%) and only 6% dead cells (Figure 5.3d). Also at 30% where the
inactivation is almost complete, the number of vital but membrane-compromised cells is higher. Hence,
the proposed inactivation mechanism is as follows:
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1) Although a shoulder appears in the beginning, and a build-up in damage is required, the PI stain
indicates similar death rates. Therefore, at the early stage the inactivation is similar, and probably
attributed to the same mechanism, of the homogeneous photo-Fenton action mode.
2) The markedly high difference after 15 min of treatment (40-50% live intact cells) but the notable
difference of compromised membranes shows that the action mode is probably the external
photo-Fenton, and the production of reactive oxygen species is responsible for membrane
peroxidation.
3) At pH = 5.5, total inactivation is achieved faster than at pH 7.5 (>99% of PI stained cells). This
result is logical if the main mechanism is the external photo-Fenton, which is more profound at
lower pH due to favorable form of iron and higher dissolution levels. However, the maintenance
of iron as Fe2+ and its soluble form explain the difference in intermediate cells. The diffusion of
iron in the cell is higher, and the internal photo-Fenton process is enhanced. For this reason,
inactivation is not heavily dependent on the external ROS action, marked by the higher red
staining levels and lower membrane-compromised, compared to the process at pH 7.5.
4) At pH = 7.5, iron is either participating in heterogeneous photo-Fenton reaction in form of oxides,
whose efficacy is lower, or by attachment to the cell surface. The notable difference in cell
integrity, due to the inflicted damage can be explained by reactions taking place at the cell
surface, such as LMCT between iron forms and yeast cell wall, due to local contact-related
promotion of photo-Fenton and subsequent damage at the proximity of a surface.
Iron citrate-driven photo-Fenton reaction at pH = 6.0 and 7.5: Figs. 5.4e and f summarize the results of
the iron-citrate assisted photo-Fenton processes. As seen also in the previous section, the inactivation
measured by cultivability, among the Fe-citrate-fueled experiments did not differ significantly. In Figure
5.3e, at around 20-25 min of treatment, up to 4-log reduction has been achieved and at 30 min, almost
complete loss of cultivability. The viability assay differs significantly from the cultivability once more.
Initially, there is a lag period, 15 and 30 min for the experiments at pH 6.0 and 7.5 respectively, as
measured by the loss of esterase activity, due to the similarities in the absorption spectrum among yeast
and the citrate complex (Robertson et al. 2013, Ruales-Lonfat et al. 2016, Ułaszewski et al. 1979). Even by
monitoring the PI staining, an initial 10-min vs. 15-min period of latency was followed by rapid increase,
to lead in 30 vs 45 min period for >99% viability loss. The peak of the intermediate states was noted at 15
minutes for pH = 6.0, whereas at 30’ for the 7.5 pH experiments. Finally, there is a notable difference at
these last time points, where for pH = 6.0, at 15 min, the composition is 25% viable, 15% dead and 60%
viable, but with compromised membranes. If this point characterizes the maximal damage point, for pH
7.5 at 30 min (Figure 5.4f), the corresponding composition was 32%, 22% and 45%, respectively. This
indicates that the damage made was rather internal, and less related with cell membrane lesions.
However, this 15-min delay has to be taken into account in the mechanism suggestion that follows:
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1) The lag is explained by the competition of yeast cells and the citrate complex, as they absorb in
the same wavelengths. Hence, a delay in the ROS production is expected, and lower peroxidation
of membranes.
2) At pH = 6.0 (compared to 7.5), the solubility of iron (Fe2+) is higher and therefore, a higher fraction
is expected to participate at the homogeneous Fenton reaction. Consequently, higher ROS
production and higher damage is recorded.
3) Also, the fast inactivation and the concomitant increase of dead and injured cells indicates a
notable participation of the internal mechanisms of inactivation (through Fe2+ penetration).
4) At pH = 7.5, the delay expressed alters the proportions of the dead cells compared to the live
ones; at the point where the intermediates reaches its maximum, more PI-stained cells appear. A
heterogeneous action mode is probable as well.
5) Generally, there is less iron intake compared with the processes initiated by FeSO4. This is
probably attributed to the initial form of iron (complexed Fe3+, compared to free Fe2+). The
importance of damage as depicted by the dead fractions and the time achieved is appearing to
be more dependent on the internal, and less in the external photo-Fenton reactions.
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Figure 5.4 – Flow cytometry results. Control tests: a) Simulated solar light only. b) hv/H2O2 system.
FeSO4–assisted photo–Fenton processes: c) pH = 5.5. d) pH = 7.5. Fe-cit–assisted photo–Fenton
processes: e) pH =6.0. f) pH = 7.5. Standard deviation < 5%.
e) f)
c) d)
a) b)
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5.3.4. Identification of targets – Nuclear DNA, cell wall and cytoplasmic protein damage
In order to further shed light in the suggested mechanisms of S. cerevisiae inactivation, an assessment of
the damage on nuclear DNA and the proteins of cell wall and cytoplasm, was performed. The analysis of
DNA fragmentation was monitored by gel electrophoresis, and the results are summarized in Figure 5.5,
while Figure 5.6 a) and b) show the results of the cell wall and cytoplasmic protein damage, respectively.
Protein damage is analyzed by SDS-PAGE and Coomasie blue staining. Simulated solar light only or
combined with H2O2, and the two main photo-Fenton systems were compared.
Figure 5.5 – Nuclear DNA damage in the four different systems. Comparison of the pH effect in FeSO4-
assisted photo-Fenton systems.
In the case of simulated solar light, as it is clearly depicted (Figure 5.5), DNA damage progresses over time,
showing a dose-dependence with exposure. After 120 min of treatment, the fragmentation levels were
too high (trace disappears). The change among the state at 60 and 120 min corroborates with the acute
loss of viability recorded via the CFDA and PI staining. The cell wall proteins pool profile appears intact
(Figure 5.6a), and negligible degradation is was detected; the intermediate cell state was also very low, as
measured by flow cytometry in Figure 5.3a. Nevertheless, after 120 min there is a notable reduction of
cytoplasmic proteins, which was not high until 60 min of exposure (Figure 5.6b). Therefore, a double
action is the probable pathway where i) DNA is damaged severely, no repair/defense mechanisms are
able to be deployed against the (mild) internal photo-Fenton action (whose damage becomes later
significant), or ii) concomitantly with the DNA destruction, the internal photo-Fenton action is becoming
profound.
0’ 30’ 60’ 120’ 0’ 60’ 120’30’ 45’ 0’ 60’ 120’30’ 45’ 0’ 60’ 120’30’ 45’
hv only hv/H2O2 hv/FeSO4/H2O2at pH = 5.5
hv/Fe-cit/H2O2at pH = 6.0
Nuclear DNA damage Comparison:pH 5.5 & 7.5
hv/FeSO4/H2O2at pH = 5.5
Nuclear DNA damage
hvh /F/FeSOSOvv 4/H/H2OO2 hv/FeSO4/H2O2at pH = 7.5
0’ 60’ 120’30’ 45’ 0’ 60’ 120’30’ 45’
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Figure 5.6 – Cell wall (a) and cytoplasmic proteins damage (b) in the four different systems. (i-ii):
Comparison of the pH effect in FeSO4-assisted photo-Fenton systems.
Cytoplasmic Protein Damage
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hv/Fe-cit/H2O2at pH = 6.0
hv/FeSO4/H2O2at pH = 5.5
hv/FeSO4/H2O2at pH = 7.5
Comparison: pH 5.5 & 7.5
Cell wall proteins
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hv/Fe-cit/H2O2at pH = 6.0
hv/FeSO4/H2O2at pH = 5.5
hv/FeSO4/H2O2at pH = 7.5
Comparison:pH 5.5 & 7.5
a)
b)
ii)
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The addition of H2O2 in the system resulted in similar DNA damages (Figure 5.5). The presence of
intermediates cells cannot really be linked to DNA and protein damages visualized by electrophoresis. The
results of the cell wall proteins’ damage presents the first notable, but limited damage (Figure 5.6a), which
probably does not lead to loss of viability, but is presented only as 3% increase of intermediate cell states.
However, the results of the cytoplasmic protein damage indicate the participation of H2O2 to the internal
mechanisms, as the staining is less intense and more bands disappeared completely (Figure 5.6b). Hence,
the increased inactivation kinetics are a result of DNA damage, combined with limited cell wall
peroxidation and increased internal photo-Fenton action, after the regulatory mechanisms fail to cope
with the high accumulation of H2O2 and the rest of the ROS in the cell.
Adding iron to the system has a detrimental effect in all levels. First of all, DNA damages were extensive,
with disappearing bands at 45 and 60 min, for FeSO4 and Fe-cit respectively (Figure 5.5). These time frames
are significantly lower than the ones recorded for the solar and hv/H2O2 systems. Probably there is an
increased loss of membrane integrity (as seen in Figs. 5.4c-f) and oxidative damage inside the yeast cell.
As it appears on the damage of the cell wall proteins, even at time 0 the staining has a different, lighter
pattern, compared with the previously presented systems. This disappearing pattern is deteriorating
slowly (until 60 minutes) and accelerates afterwards (Figure 5.6a). However, since the cytoplasmic
proteins are actively getting degraded after 60 min for FeSO4 and Fe-cit, the strong dependence on the
internal contribution is verified (Figure 5.6b).
Cultivability is lost even before the damage (at any level) is highly accumulated. Furthermore, flow
cytometry suggested that the loss of viability was accelerated after 15-20 min for the iron assisted systems
(Figs. 5.4c-f), but the protein damage is highly notable after 30 minutes. For the iron-supported systems,
the order of events in the form of a suggested timeline can be found in Table 5.1. The loss of cultivability
is related with the first and direct oxidative stress conditions that the cell is faced with. The simultaneous
damage of DNA and cytoplasmic proteins, verify our initial hypothesis that the driving force in S. cerevisiae
inactivation is the internal photo-Fenton process. For the two iron salts, the difference in the appearance
of this effect is related with the ROS production in the system; FeSO4 at pH 5.5 presented significantly
higher activity. Then, as these electrophoresis processes are quantitative, the cell wall proteins appear as
the last to degrade because they comprise a very big part of the total mass of the cell. This is also explained
by the fact that in all figures depicting the protein damage, the bigger ones (highest kDa values) are
targeted first. Finally, in order to notice oxidative damage inside the cell, only a small part of the
membrane must be breached, enabling the introduction of iron into the cell (extra amount added to the
diffusing one). The fact that the flow cytometry data indicate more than 50% viable but compromised
membrane-cells, is the signature of the breach and the subsequent internal action.
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Table 5.1 - Timeline of the inflicted damage in the corresponding targets of the different iron-assisted
systems
Event FeSO4 Fe-cit Loss of cultivability 10-20 min 15-20 min
Loss of viability (by CFDA or PI) 10-30 min 10-30 min
DNA damage 30-45 min 45-60 min
Cytoplasmic proteins damage 30-45 min 45-60 min
Cell wall proteins damage 60-120 min 60-120 min
At a higher pH for the FeSO4 system, where solid Fe-oxides (goethite) is present, weaker, less active
systems are involved. The DNA damages were delayed, compared to the corresponding system at 5.5 pH.
However, a possible contribution of the iron oxides is noted, when the internal and external protein
damage is compared. When the pH of the solution promoted the oxide formation, increased cell wall
degradation was observed. Accordingly, lower internal protein damage has been recorded. The
combination of these two events indicate a contribution of the iron oxides at the degradation of the cell
membrane, either by promotion of local oxidative species at the surface of the (attached to the cell) iron
oxide, by the oxide itself acting as a semiconductor and causing local damage to the structure, or by
heterogeneous photo-catalysis in presence of H2O2.
5.3.5. Holistic proposal for the inactivation mechanism of S. cerevisiae
Having analyzed the cultivability and flow cytometry results, as well as the DNA and protein damages,
together with an extensive literature review, a mechanism proposed for the inactivation of S. cerevisiae
is given in Figure 5.7. The four sub-figures represent distinct actions, as before: a) simulated solar light
alone (here, direct action), b) hv/H2O2 (+indirect light actions, important at this stage), c) FeSO4-assisted
(including oxides) and d) Fe-cit-assisted photo-Fenton systems. Once again, the step-wise construction of
the complex photo-Fenton mechanism is not repeated; the actions of the solar-only system and the
hv/H2O2 are present in the photo-Fenton actions, but not presented again, for simplicity. Also, the
references that support our observations and the subsequent suggestions are not repeated again in this
section, as they were discussed before. A brief explanation on the different actions per sub-figure follows:
a) (Direct) Solar light: (1) Simulated solar light induces mutations at DNA level (e.g. CPDs, (6-4)
photo-products, guanine to cytosine transversions) at both nucleic and mitochondrial genome (2). Also,
mainly UVB and in a lesser extent UVA induce damage at the external cell surface (3). The cell structures
suffer damage at external and internal level (4): internal groups and structural functions (enzymes,
clusters, proteins etc) are physically affected by the direct illumination. Cell death can be the final
outcome of the loss of viability.
145
b) (Indirect) hv/H2O2: Light affects internal enzymes, such as superoxide dismutase (SOD) and
peroxidases, such as catalase, oxidase etc. (1) and (2). As a result, the internal respiratory chain is affected,
with subsequent H2O2 and ● accumulation. Since Fe/S clusters are affected, release of iron is expected,
and an internal Fenton mechanism is initiated with the hydroxyl radicals damaging internally the cell. H2O2
plays both the role of oxidant for Fe2+ and the reductive for Fe3+, and since light is present, internal photo-
Fenton is taking place. The superoxide radical also participates in iron reduction and the internal oxidation
actions. As far as the external actions are concerned, mild peroxidation of the external cell wall proteins
at small extent is expected (3) and possible penetration of H2O2 into the cell (4). These actions further
enhance the internal photo-Fenton actions.
Figure 5.7 – Mechanistic proposition of the pathways towards yeast cell inactivation. a) (direct)
Simulated solar light. b) (Indirect) hv/H2O2. c) FeSO4–assisted photo–Fenton process. d) Fe-cit–assisted
photo–Fenton process.
c) FeSO4-assisted photo-Fenton: The addition of FeSO4 in the solution provides (for a limited period
of time) Fe2+, which produces radicals externally (1). Fe3+ complexes are reduced by light, further
producing hydroxyl radicals and Fe2+. The rupture of the cell wall can allow the penetration of Fe2+ and
Fe3+ into the cell, enhancing the Fenton reactions taking place inside the cell (2). Also, the iron transport
mechanisms carry Fe2+ and Fe3+ into the cell, to maintain homeostasis, with the same effect as before (3).
However, the presence of dissolved oxygen in the sample and the near-neutral pH cause the oxidation of
iron to goethite and lepidocrocite; the heterogeneous Fenton action is initiated (4). The attachment of
146
the (positively charged) iron to the (negatively charged) cell wall induces local damage to the cell through
either (5) a photo-assisted reduction of Fe3+ (LMCT) on cell wall and the initiation of a photo-Fenton action
(since H2O2 and light are present and Fe2+ is produced) or (6) semiconductor action mode by the iron oxide,
which includes oxidative damage from the hole (h+) and the excitation of electrons (e-). These electrons,
in presence of oxygen or H2O2, acting as electron acceptors, generate ROS that cause extra oxidative
damage in the exterior of the cell.
d) Fe-cit-assisted photo-Fenton: Iron citrate is stable in water, in absence of light (equilibrium 1).
Light on the Fe-citrate, on the other hand, induces another pathway, involving LMCT and a [Fe2+─cit2─●]
product. Its dissociation gives Fe2+ and cit2─●, which can participate in the Fenton reaction (2) and
formation of superoxide radical anions (3), respectively. Alternatively, the cit2─● can react with H2O2
(4).The end-product is a hydroxyl radical, which inflicts external damage to the cell.
5.4. Conclusions
A eukaryotic, unicellular microorganism (S. cerevisiae) was subjected to a multi-level, systematic
investigation on its inactivation mechanisms. The contribution of photo-Fenton and its constituents were
put under study, and light was shed on the separate or synergistic pathways participating in yeast
inactivation.
The cultivability results indicated the best conditions and starting iron forms, to achieve the best
inactivation rates. Furthermore, flow cytometry data coupled with the electrophoresis data on DNA and
protein suggested the pathways towards inactivation. A significant contribution of the internal photo-
Fenton process was measured, in addition to the external oxidative stress by the ROS produced.
In principle, the action of light was monitored to affect mainly the DNA, and secondarily, the internal
proteins. The sequence of events suggests a photocatalytic-like induction of damage. When H2O2 was
added to the system, the non-viable cells were a result of increased internal photocatalytic reactions,
when compared with bare light. The addition of iron greatly enhanced the process, reducing the
inactivation time significantly. The generation of ROS inside and outside the cell reduced the viability by
destroying DNA and internal proteins, and when the process was prolonged, total destruction of the cell
was monitored.
According to the pH levels, iron oxides participate in heterogeneous pathways. Efficient photo-Fenton
inactivation was observed at pH 7.5, and in cellular level, a mixed mode between the diffusion of iron into
the cell and the damage caused from iron particles attached to the surface of the cell. Finally, iron citrate,
a relatively cheap organic complex was investigated, to increase the applicability of the process. The
significant inactivation measured indicates promising application potentials.
147
In overall, a wide view into the pathway of S. cerevisiae inactivation was given, helping understand the
inactivation of more complex microorganisms. Nevertheless, its complexity did not offer great resistance
against the photo-Fenton reaction, but can offer great insight on the function of eukaryotic cells when
present in similar oxidative stresses.
149
PART 3
Degradation of hospital PhACs by AOPs, as a point-source treatment
option in HWW and urine: treatment optimization and degradation
pathway elucidation
151
6. Chapter 6 - Iohexol degradation in wastewater and urine by
UV-based Advanced Oxidation Processes (AOPs): Process
modeling and by-products identification.
Published work:
Stefanos Giannakis, Milica Jovic, Natalia Gasilova, Miquel Pastor Gelabert, Simon Schindelholz, Jean-
Marie Furbringer, Hubert Girault, and César Pulgarin. "Iohexol degradation in wastewater and urine by
UV-based Advanced Oxidation Processes (AOPs): Process modeling and by-products
identification." Journal of Environmental Management (2016), pp. XXX - XXX
Web link:
http://www.sciencedirect.com/science/article/pii/S0301479716304418
Supplementary material:
Appendix E
Doctoral Candidate’s contribution:
Main investigator and author.
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6.1. Introduction
During the last decades, research in wastewater (WW) treatment has focused on the elimination of
emerging contaminants. Having efficiently tackled the classical WW issues of macro-pollution (organics,
phosphorus, nitrogen etc), combined with the leaps in analytical chemical capabilities, micropollutants
are the hottest topic in WW treatment for the last 15 years. These substances are comprising an increasing
list of anthropogenic contaminants, which include among others, pharmaceuticals, personal care
products, steroid hormones, industrial chemicals, pesticides and many other emerging compounds (Luo
et al. 2014). The polymorphism and the diversity of the chemical pollutants, state this topic as high priority
for the treatment facilities.
A distinctive category of micropollutants are the Pharmaceutically Active Compounds (PhACs), and
especially the ones that are exclusively administered from hospitals. Verlicchi et al. (Verlicchi et al. 2012)
analyzed 73 PhACs from 12 different therapeutic classes, and they concluded that most compounds are
found in consistently higher concentrations in HWW than in urban WW. The antibiotics, analgesics and
lipid regulators were the most concentrated, and 9 compounds posed a high risk at the concentrations
detected in hospital effluent and 5 in urban WWTPs influent and effluent. Ort et al. (Ort et al. 2010)
analyzed 59 PhACs in HWW, from which 2 had a contribution higher than 15% of the total of WWTP
influent. Within the “Pills-Project” (Pills-Project 2012) 16 key substances out of eight substance groups in
different hospitals were studied, concluding that 5 of these groups are exclusive contributors in 10 to 60%
of the load found in urban WWTPs, and are attributed to hospital use.
Among these categories, the Iodinated Contrast Media (ICM) are identified as a major threat. In a recent
research in a University hospital in Lausanne, Switzerland, contrast media contributed in 59% of the total
PhAC load. Globally, the consumption of ICM is 35.000 tons/year (Sprehe and Geissen 2000), from which
95% are excreted unchanged from the human body. Their use in Germany has been estimated at 500 tons
of ICM per annum (Haiß and Kümmerer 2006), while in Switzerland, the total consumption per year of
ICM is estimated at 35 tons (McArdell et al. 2011). In the case of a standard Swiss University hospital, the
consumption is of 1149 g/day and 725 g/day only for Iohexol (Weissbrodt et al. 2009); half of the
consumed amount is rejected in HWW. This amount is reached because the individual dosage in imaging
treatment is up to 300 g (Haiß and Kümmerer 2006). ICM are non-biodegradable and only partially
removed in WWTP, so their concentration in surface and drinking water is increasing, with the
concentration of Iohexol in Lake Leman, Switzerland being 0.03 μg/L (Chèvre 2014), or Iopamidol, which
was found in groundwater up to 2.4 μg/l (Ternes and Hirsch 2000).
Since the proven incapability of the existing WWTPs to handle ICM is established, their discharge to
natural water bodies will contain the aforementioned amounts (Pérez and Barceló 2007, Putschew et al.
153
2000, Ternes and Hirsch 2000). Advanced Oxidation Processes (AOPs) have long been suggested as an
alternative in treating non-biodegradable compounds (Herrera et al. 1998, Pulgarin and Kiwi 1996) and
many works have demonstrated the efficiency of AOPs against ICM. For example, for various ICM, such as
Iopamidol, Iomeprol, Iohexol and others, very good removal was attained at basic pH (Seitz et al. 2008),
or exposure to gamma irradiation (Jeong et al. 2010), while UV/TiO2 although it requires higher treatment
times, is a treatment that can achieve high removal rates (Borowska et al. 2014, Doll and Frimmel 2004,
Sugihara et al. 2013). Nevertheless, the works that have addressed the removal in matrices as hospital
wastewater or urine are scarce.
In this work, Iohexol has been chosen as a model non-ionic ICM, and has been subjected to extensive
investigation concerning the various UV-based processes (UV, UV/H2O2, UV/H2O2/Fe2+). In order to assess
the feasibility of the treatment by UV-based AOPs, an engineering approach has firstly been made, where
the investigation focuses on the matrices that Iohexol can be potentially found and measure the effect of
the operational parameters in achieving 90% degradation of the initial amount in water, wastewater and
urine. Also, in the view of treatment optimization by these AOPs, a modeling approach has been made for
the reactants addition and pH. Finally, in order get insights on the structures affected by the different
components of the process, the degradation pathway is studied for the three AOPs applied.
6.2. Materials and Methods
6.2.1. Chemicals and Reagents
Table 6.1 presents the composition of the synthetic urine and synthetic wastewater employed in most
experiments; the chemicals were used as received. Iohexol (Histodenz), hydrogen peroxide (30%) and iron
sulfate heptahydrate, used for the degradation experiments, as well as KCl, Peptone, CaCl2·2H2O and
MgSO4·7H2O were purchased from Sigma Aldrich (Switzerland), NaCl, Na2SO4, Meat Extract and NH4Cl
were acquired from Fluka (Switzerland), KH2PO4 and K2HPO4 from Merck (Switzerland), while urea and
creatinine from ABCR (France). Finally, titanium oxysulfate for the colorimetric determination of H2O2 and
Ferrozine for iron detection were purchased from Fluka.
Table 6.1 – Synthetic matrices composition.
Synthetic Urine Synthetic Wastewater Name Chemical
formula SUR
composition [g/L]
Name Chemical formula
SWW composition
[mg/l]
154
Urea CH4N2O 25 Peptone - 160 Sodium Chloride
NaCl 2.925 Meat Extract - 110
Sodium Sulfate Na2SO4 2.25 Urea CH4N2O 30
Potassium chloride
KCl 1.6 Dipotassium Phosphate
HK2PO4 28
Potassium phosphate monobasic
KH2PO4 1.4 Sodium Chloride NaCl 7
Calcium Chloride
dihydrate
CaCl2·2H2O
1.103 Calcium Chloride dihydrate
CaCl2·2H2O
4
Creatinine C4H7N3O 1.1 Magnesium Sulfate
Heptahydrate
MgSO4·7H2O
2
Ammonium chloride
NH4Cl 1
6.2.2. Reactors and experimental apparatus
Three “merry-go-round” reactors were used for the Iohexol degradation experiments, presented in
Supplementary Figure S1. These double coated glass vessels recirculate water at 22°C (Neslab RTE-111
thermostat), for the protection of the UV-C equipment. UV-C light at 254 nm (5x10-3 mW/cm2) was
supplied to the system by low pressure (LP) mercury discharge lamps (Philips TUV 11W/G11 T5 UV). The
lamps were placed in the interior of quartz glass and then submerged in the solution inside the reactor.
Mixing is ensured by a magnetic bar at the bottom of the reactor and the placement of the apparatus on
a magnetic stirrer.
6.2.3. Analytical methods
6.2.3.1. Iohexol determination
The determination of Iohexol concentration was achieved through HPLC analysis (HP Agilent 1100 Series),
including a G1315A diode array detector, set at 254 nm. The HPLC method was as follows: The mobile
phase was held at an isocratic mode during all the analysis and consisted in the mixture of 95 % ultrapure
(Mili-Q) water with 0.1 % of formic acid (phase A) and 5 % of methanol (phase B). The flow was 1 ml/min
and the temperature of the column is 40 °C and the injection volume was 50 μL. This configuration led to
a retention time of 10.15 min, with a C18 reverse phase column (Merck Lichrospher 100 RP-18, 5 μm, 250
· 4 mm).
155
6.2.3.2. H2O2, Fe, COD and TOC measurements
A Shimadzu UV 1800 spectrophotometer was used for the colorimetric determination of H2O2 and iron.
H2O2 was quantified by adding 10 μL of Ti(IV) oxysulfate in 1 mL of sample and subsequent measurement
at 410 nm (DIN 38402H15 method). In some experiments, due to color interferences, Merck Milipore
peroxide detection strips were used for semi-quantitative measurement of H2O2 (measurement ranges:
<1. 1-3 and 3-10 or <1, 1-5 and 5-10 ppm). They were employed to detect residual (<10 ppm) of H2O2 in
real WW samples and H2O2 in high concentrations of Iohexol (color interference). Dissolved iron was
followed with the Ferrozine method, as described elsewhere (Viollier et al. 2000). Briefly, after filtration
of a 5 mL sample (0.22 μm), 0.2 mL of hydroxylamine hydrochloride, 0.2 mL of acetate buffer at pH 4.65
and 0.1 mL of 10 mM Ferrozine solution were added in the bulk. The iron determination took place by
spectrophotometric measurement of the magenta color formation at 562 nm.
Pre-acquired COD (HR/LR vials, HACH Lange) were used to determine the chemical oxygen demand, and
the corresponding colorimetric methods were used, measured by a HACH DR3900 Spectrophotometer.
Total organic carbon and inorganic carbon of the samples during treatment were followed by a Shimadzu
TOC-VCSN analyzer, with an ASI-V automatic sampling module. Finally, pH was measured with a Seven
Easy pH meter (Mettler-Toledo).
6.2.3.3. Orbitrap MS analysis for determination of the degradation pathway
The products of Iohexol degradation were analyzed by HPLC-HR-MS. Prior to the analysis the samples
were desalted using C18 SPE spin columns (Pierce Biotechnology, Rockford, IL, USA) following the
manufacturer protocol. Desalted samples were separated using Dionex UltiMate 3000 UPLC system with
Nucleodur C18 Gravity-SB precolumn (4 x 2 mm, 1.8 m) and Nucleodur C18 Gravity-SB separation column
(4 x 2 mm, 1.8 m, Macherey-Nagel, Düren, Germany). The solvent A was composed of water with 0.1 %
FA, while solvent B contained acetonitrile with 0.1 % FA. The flow rate of the mobile phase was set to 250
l/min. The gradient consisted in the linear increase of solvent B percentage from 3 to 60 % within 11
min. The sample injection volume was set to 35 l. The order of events were i) column activation:
MeOH/TFA 50%/0.01%, ii) column equilibration: 5% ACN 0.5% TFA, iii) sample binding: 150 μL sample, iv)
washing: 5% ACN 0.5% TFA and v) elution: 80% ACN 0.1% TFA.
The MS was performed using a Q Exactive-HF-Orbitrap MS instrument (Thermo Scientific, Bremen,
Germany) in positive ion mode within 200-1000 m/z. For all LC-MS runs survey scans were acquired with
15000 resolution (at 400 m/z), automatic gain control (AGC) value of 3E6 and maximum injection time of
100 ms. Dynamic exclusion duration for the precursor ions was set to 30 s. Top 5 data-dependent MS/MS
scans were recorded also with 15000 resolution (at 400 m/z), AGC value set at 1E5 and maximum injection
time of 50 ms. The isolation width for the precursor ion was set to 1.8 m/z. Higher-energy collision induced
dissociation (HCD) was used for the fragmentation of isolated precursor ion with normalized collision
156
energy (NCE) of 26 % and minimum signal threshold for MS/MS triggering was fixed to 20000 counts. The
obtained data were processed using Xcalibur software (3.0.63 version, Thermo Scientific, San Jose, CA,
USA).
6.2.4. Water matrices and treatment conditions
All experiments were carried out in triplicates (3 reactors) and in different categories of matrices, i.e.
water, wastewater and urine. The systematic studies took place in ultrapure water (MQ), synthetic
wastewater (WW) and synthetic urine (UR). The graph data represent the average, with <5% standard
deviation in the majority of cases (error bars not shown). The operational parameters tested were the
following: i) Specific matrices investigated: Mili-Q water (MQ), synthetic WW, diluted synthetic WW,
untreated (biologically) WW, secondary WW, synthetic urine, real urine and diluted real urine, ii) initial
Iohexol concentration 10 – 1000 ppm, iii) initial H2O2 concentration 0 – 1000 ppm, iv) initial Fe2+ addition:
0 – 50 ppm, v) Dilution factor: undiluted, x10 diluted, x100 diluted and vi) starting pH: 3 – 11.
Table 6.2 – Physicochemical characteristics of the real wastewater matrices (Giannakis et al. 2015c,
Margot et al. 2013, Margot et al. 2011).
(mg/L) WWTP Influent Activated Sludge Effluent Total Suspended Solids (TSS) 30 13.9
Dissolved Organic Carbon (DOC) 91 7.9
Chemical Oxygen Demand (COD) 256 30.2
Total Nitrogen (in NH4, NO3, NO2) 30 19.1
Total Phosphorus 5.8 0.55
Alkalinity (CaCO3) n.m. 273
pH 8 7.5 n.m: not measured,
The composition of the synthetic WW and UR matrices was presented above. The real WW experiments
involved i) the sampling from the influent and ii) the sampling after biological treatment and secondary
clarification, from the WWTP of Vidy, Lausanne, Switzerland, whereas the real UR experiments succeeded
the collection of urine from healthy individuals. Their main characteristics are presented in Tables 6.2 and
6.3, respectively. Finally, spiking with Iohexol to the desired level took place before each experiment.
Table 6.3 – Physicochemical characteristics of real urine matrices (own measurements and (Beach
1971)).
Parameter low high unit TDS 24.8 37.1 g/L pH 6.2 8.3
157
COD 6.1 10.6 g/L TKN 4.8 7.9 g/L TOC 3.6 6.7 g/L
Average
Inorganic salts 14.2 g/L Urea 13.4 g/L Organic compounds 5.37 g/L Organic ammonium salts 4.1 g/L Total solutes 37.1 g/L
6.2.5. Statistics, modeling and data treatment
For the statistical and modeling part of the investigation, the collected data were organized under
separate designs of experiment. Their treatment was achieved through MINITAB software for Windows
including the ANOVA and the proposed models for the first order degradation constant k. The evaluation
of the models is performed through the standard error (S) and the coefficient of determination (R2).
i) Quadratic model
The model is formulated as follows:
(6.1)
where k is the (first order) reaction constant, xi are the model parameters and aij the respective weights.
For each experiment the first-order k constant was determined (dependent variable) and was described
as a function of initial Iohexol concentration [I], H2O2 addition [H2O2], starting iron addition [Fe2+] and the
pH (independent variables).
ii) Multiplicative model
The second model presented here is formulated as follows:
(6.2)
k refers to is the reaction kinetics, xi are the model parameters, γi the corresponding weight, while c is a
numerical constant.
Given that all the parameters can be expressed in logarithmic terms (as concentrations), the model can
be written as above. The independent variables assume 0.01 instead of 0 in the Iohexol, H2O2 and Fe2+
concentrations, and the pH of the solution is expressed as –log[H+]. Therefore, the equation 2 is expressed
as follows:
158
(6.3)
With the aforementioned transformation, the model takes a rather simple form of a product between the
independent variables, directly connected with the reaction constant k.
6.3. Results and Discussion
6.3.1. Engineering approach – investigation on the operational parameters
6.3.1.1. Iohexol, H2O2 and water matrix effect on t90%
In the first part of this study, the operational parameters involved in the UV/H2O2 AOP process were
investigated, namely the concentration of Iohexol, the addition of H2O2 and the matrix containing the
contaminant. Figure 6.1 depicts the influence of concentration of the drug (I) and the oxidant (H2O2), in
Mili-Q (MQ) water. As it has been previously reported (Pereira et al. 2007), Iohexol is rather susceptible
to UV treatment alone. The high molar absorption coefficient of Iohexol at 240 nm (Borowska et al. 2014)
makes the treatment by the high energetic UV-C photons effective. According to the level of drug addition,
the time necessary to degrade the pollutant starts from a matter of minutes (10 ppm) and exceeds 10 h
(1000 ppm) for this relatively low light intensity used in our experiments. The good linear profile of the
fitted lines in log Y scale (R2>99%) indicate that the degradation follows pseudo first order kinetics. The
threshold of 90% degradation is set to ensure elimination of the compound and offer a ground of
comparison among the various processes that will follow, which is calculated as t90%=-(ln0.1)/k.
In the former experiment, H2O2 was also added in a log-stepwise manner. The homolytic disruption of the
HO-OH bond results in the release of the second most powerful oxidant, the hydroxyl radical (HO●) (Guo
et al., 2013). In the past, adding small quantities of H2O2, when LP UV was used, has not sufficiently
improved the degradation of Iohexol in water matrices (De la Cruz et al. 2013, De la Cruz et al. 2012,
Pereira et al. 2007), but the concentrations never exceeded the “economic” range.
159
Figure 6.1 – UV photolysis and UV/H2O2 experiments in Mili-Q water. Note that the results in the 10-
1000 mg/L range are plotted in double-logarithmic scale and axis breaks for clarity purposes only.
Here, we reached up to 1000 ppm H2O2 initial addition, and the results are presented in the different color
traces of Figure 6.1. Iohexol is mostly affected by the hydroxyl radical addition to the aromatic ring, as
hydrogen abstraction or electron transfer are either slower or less common pathways (Zhao et al. 2014).
Nevertheless, it appears that the process is mildly affected in its totality, since the t90% is moderately
improved. Also, since the first order models also fit well this process, we can corroborate with previous
findings (Pereira et al. 2007, Sharpless and Linden 2003) that most probably, the efficiency of direct
photolysis is very high.
Table 6.4 – t90% evolution (min) in varied Iohexol (10-1000 ppm) and H2O2 (0-1000) levels
Iohexol/H2O2
1000/0 1000/10 1000/100 1000/1000
Mat
rix MQ 324 320 311 268
WW 371 360 329 291
UR 535 523 501 461
100/0 100/10 100/100 100/1000
Mat
rix MQ 33 28 26 19
WW 35 29 27 22
160
UR 204 184 141 122
10/0 10/10 10/100 10/1000 M
atrix
MQ 7 5 4 3
WW 10 7 6 3
UR 168 154 139 122
Similar investigation also took place in (synthetic) wastewater (WW) and (synthetic) urine (UR) matrices.
These matrices represent the main conditions in which Iohexol is encountered, and the effect of the
matrix is here investigated. Table 6.4 summarizes the t90% calculated in the different experiments, varying
the initial Iohexol and H2O2 amount, as a first step. A marginal improvement is observed as the ratio of
Iohexol/H2O2 is modified, as found in the MQ matrix before. However, although t90% times for WW
remained close to the observed ones for MQ, synthetic urine values did not drop significantly for low (10
ppm) Iohexol content, but were rather similar to the 100 ppm ones. The explanation lies in the
competition for the HO● radicals generated by the process. In wastewater, the oxidizable organic and
inorganic components are significantly less than in urine, which makes the degradation of mg/L quantities
easier. Normally, for compounds that are highly photo-oxidized, the effect of the organic matter is usually
not very profound (Canonica et al. 2008). Hence, a parameter which could greatly affect the application
of the process and would need further investigation is the possible dilution of the concentrated WW and
UR, and then treatment with AOPs.
6.3.1.2. Effect of matrix dilution and Fenton-initiated enhancement of the process on t90%
Figure 6.2 showcases the wastewater and urine experiments plus the comparison between undiluted and
diluted (x10 times) matrix, while featuring the addition of Fe2+ in the system and the drop of the pH up to
3. For WW (Figure 6.2a), dilution had an effect on the degradation efficiency, decreasing as the initial
Iohexol content is decreasing. The diluted matrix now presents less competition for the HO , effectively
targeting the contaminant. However, for the same reason, milder effect on the addition of iron now
occurs, as, along with the antagonistic nature, the synergistic metal complexing effects of the organic
matter, leading to a higher Fe3+ solubility and consequently a more efficient Fenton and photo-Fenton
cycle, are now mitigated. Nevertheless, the dilution plays an important role and ~20% improvement in
degradation is measured. This suggests confidently that reducing the organic matter of the water, for
instance with an activated sludge process could enhance the efficiency of the downstream UV/H2O2/Fe2+
AOP applied, the participation of the matrix, but also the recalcitrance of the compound while treated,
since the improvement is not impressive.
161
Figure 6.2 – Effect of pH, dilution and Iohexol, H2O2 and Fe2+ amounts. Dotted lines represent the
undiluted matrices, continuous lines indicate the x10 times dilution experiments, and for Figure 3b, the
x100 times diluted UR experiments are signified with long dashed lines. Note the mixed axes scales.
Furthermore, in Figure 6.2b we observe a similar improvement in UR treatment when x10 dilution is
applied in the system. In average, the improvement is higher than the respective one in WW, with almost
~40% minimum increase in the efficiency. The new matrix composition absorbs less UV inefficiently (nitro-
, amino- and phosphoric compounds from the synthetic recipe), thus efficiently targeting Iohexol, and also
the generated radicals target the contaminant without being overly wasted. Technically, using a
secondary water from other sources in a hospital could be feasible; for example water from deionization
units, or even greywater (having considerably lower organic and inorganic content than urine) could be
used for the dilution. Of course, hydraulic optimization of the reactor and construction costs will play an
important role, which is beyond the scope of this research.
6.3.1.3. Experiments in real wastewater and urine matrices
i) Real wastewater
In municipal wastewater, we tested the lower two concentrations assayed in the synthetic matrix, before
and after secondary treatment of the WW inflow, varying the Iohexol spiking, the H2O2/Fe2+ addition levels
and the pH in the beginning of the experiment.
162
Figure 6.3 – Real wastewater and urine experiments: UV/H2O2/Fe2+ process. A) Iohexol in untreated or
biologically treated WW, and B) diluted/undiluted urine, H2O2 added in 0, 10 or 50 ppm, iron was
added in 0, 1, or 5 ppm, and changing of the initial pH value (3, 5 or near-neutral). The two main
groups of Figure 3a data are separated by continuous (10 ppm Iohexol) or dashed lines (100 ppm). The
respective groups in Figure 3b are designated by color. The vertical bars show the variation in
efficiency when pH was changed. Note the mixed axes scales.
Figure 6.3a suggests that, as a rule of thumb, acidification increased efficiency and moving towards the
natural pH, the removal is hampered. The initial physicochemical conditions differ significantly among the
two matrices with suspended solids, which block light transmission, being double before treatment.
Secondly, the organic content removed in the activated sludge unit greatly benefited the process
demonstrating 50% reduction in the removal of Iohexol (10 ppm) and almost 20% in the 100 ppm
experiments. The reduction of the organics content permitted the redirection of the HO● radicals against
the contaminant, which is less effective when high amounts of Iohexol were added.
However, the degradation in WW is a complex system, with various forces which aid or act antagonistically
either to the photolysis or the production of hydroxyl radicals. Other parameters that influence the
efficiency are the nitrogen, phosphorus and carbonate-related compounds. Nitrate exposed to UVC at
254 nm has been shown to undergo photo-transformations. With the participation of peroxynitrite and
peroxinitrous acid, either nitric acid or nitrite is produced (Mack and Bolton 1999). The nitrite, reacts with
the hydroxyl radicals, producing nitrite radicals (Vione et al. 2014). Phosphorus on the other hand
moderately consumes hydroxyl radicals, but precipitates by the iron salts, which actively reduces the
available iron for the complementary photo-Fenton action. Finally, (bi)carbonates are known not only to
scavenge the hydroxyl radicals, but also to form the carbonate radicals, which have mild oxidative action
(Wu and Linden 2010).
163
ii) Real urine
For the experiments involving real urine, the initial COD values ranged between 2.8-9.5 g/L and DOC 2.5-
7 g/L, corroborating with the literature suggesting similar values, previously presented in Table 6.3.
Treatment Iohexol in urine (Figure 6.3b) revealed only two different families of graphs, i.e. the diluted and
undiluted urine experiments. Firstly, pH modification and the addition of the Fenton reagents did not
enhance significantly the degradation rate. The vertical bars indicating the improvement are smaller than
the respective wastewater ones. Secondly, when treating Iohexol in undiluted urine, almost regardless of
the method or reactant addition, both 100 and 1000 ppm experiments required a significantly elevated
time to complete. Apart from the suspended solids, the reactants involved in wastewater, concerning
nitro-, phosphoro- and carbonate-compounds here are in higher amounts, compared to wastewater, and
the implications are expected to make the degradation scheme more complex.
Also, urine contains large amounts of proteins, such as urobilin, serum albumins, transferrins etc, some
of which contain groups which absorb in the UV region. On the other hand, transferrins can bind the iron
(Davis et al. 1962), which limit the participation in the Fenton reaction (Papoutsakis et al. 2015a). This
hypothesis is further strengthened when examining the diluted urine matrix. If x10 dilution is applied, the
need to acidify and add the Fenton reactants is lower, as they marginally contribute to the degradation.
Although a bigger reactor theoretically would be necessary, the economical and operational costs are
considerably lower than the ones necessary for improving the process in undiluted urine.
6.3.2. Statistical approach – modeling and mathematical optimization of the treatment
A general finding of the previous part was that there were no significant differences between the results
found in synthetic and real WW and UR matrices, therefore the laboratory tests can be extrapolated in
the real context. Also, it means that in two different matrices, we could predict the time necessary for
degradation (t90%), based only on broad indications about the target matrix and the order of magnitude
of Iohexol concentration. For the aforementioned reasons, we attempt to model the degradation process
(first order degradation constant k), based on the laboratory experiments already presented in the
previous chapter.
The models, to which the data will be fitted, have been presented in the Materials and Methods section.
For identifying the coefficients of these models, we have completed the experiments presented in the
previous section with additional experimental points, to constitute a Central Composite Design (CCD),
which summary is as follows:
Iohexol was kept constant, at 100 mg/L,
H2O2 and Fe2+ values were kept in a low amounts, in all matrices
164
pH was tested among 3 and 5 (to better take advantage of the conditions that favor the Fenton
reaction).
Table S1 of the Supporting Information presents the data points and the levels of the parameters used in
the CCD. The experiments added from the previous section bring different Iohexol and Fenton reagent
amounts, as well as alternative pH values (near neutral and basic, only for WW).
As a general strategy for both matrices, a step-wise construction of the model took place, as follows: After
removal of the outliers and through regression, different models were fitted. Their expressions are
presented in Table 6.5 for WW and Table 6.6 for UR. For the multiplicative model, the logarithmic values
of the various levels and the response variable k were used; we remind that for pH, its definition of the “–
log[H+]” was used.
Two evaluation criteria have been used, i.e. the standard error (S) and the coefficient of determination
(R2, %). ANOVA was also performed (the detailed ANOVA tables can be found in the Supplementary
material) and put in evidence the order of importance among the factors.
Iohexol > H2O2 or pH > Fe2+.
This order is only qualitative since often the Fenton reagents and the pH failed to pass the P-test of 95%
confidence interval (e.g. Tables S1.1.1 or S1.1.5. in Supplementary Material). Also, the order among H2O2
and pH depends on the matrix, with WW regarding the H2O2 addition as most important and UR matrices
(especially the undiluted) depending more on the pH. This effect can be attributed to the efficient
photolysis or the homolysis of H2O2 in the more transparent matrices, compared to UR, whereas
acidification favors the photo-Fenton participation.
As it is clearly shown in the two previous Tables (6.5 and 6.6), the process cannot be described fairly by a
linear model. The interactions and/or the square terms need to be added. In all cases, Iohexol amount is
the most important factor in determining the order of magnitude of the k constant. The use of the
multiplicative model provides a far simpler expression, without conceding much in terms of accuracy in
most of the cases. As the scale is different, the importance of the parameters is also changed, with pH
becoming more important for wastewater and Fe2+ for urine.
165
Table 6.5 – Wastewater models with S and R2 values.
WASTEWATER Linear Linear w/squares Quadratic WASTEWATER Multiplicative
Linear
Linear
Constant 1.46E-01 3.56E-01 3.36E-01
Constant 9.33E-01
[I] -1.43E-04 -2.86E-03 2.85E-03
log[I] -9.75E-01
[H2O2] 2.30E-05 2.93E-04 3.33E-04
log[H2O2] 2.79E-02
[Fe2+] -8.00E-05 2.89E-03 5.08E-03
log[Fe2+] 1.07E-01
pH -1.69E-03 -3.14E-03 -3.00E-04
log[H+] 2.32E-02
Squares
[I] x [I]
3.00E-06 3.00E-06
[H2O2] x [H2O2]
-1.00E-06 1.00E-06
[Fe2+] x [Fe2+]
-6.10E-05 -1.20E-04
pH x pH
-7.30E-05 -1.97E-04
Interactions
[I] x [H2O2]
-1.00E-06
[I] x [Fe2+]
-2.00E-06
[I] x pH
-5.00E-06
[H2O2] x [Fe2+]
3.00E-06
[H2O2] x pH
1.20E-05
[Fe2+] x pH
-1.01E-04
S 0.07 0.02 0.02
S 0.10
R2 38.44 92.38 93.90
R2 96.62
DILUTED WASTEWATER Linear Linear
w/squares Quadratic DILUTED WASTEWATER Multiplicative
Linear
Linear
Constant 2.48E-01 6.68E-01 6.29E-01
Constant 1.37E+00
[I] -2.39E-04 -3.33E-03 -3.79E-03
log[I] -9.18E-01
[H2O2] 9.80E-05 8.70E-05 2.69E-04
log[H2O2] 5.60E-03
[Fe2+] -1.74E-03 1.50E-03 1.11E-02
log[Fe2+] 6.56E-02
pH 3.00E-04 -8.45E-02 -7.70E-02
log[H+] 8.60E-02
Squares
[I] x [I]
3.00E-06 3.00E-06
166
[H2O2] x [H2O2]
-1.00E-06 2.00E-06
[Fe2+] x [Fe2+]
4.10E-05 -1.08E-04
pH x pH
7.69E-03 7.00E-03
Interactions
[I] x [H2O2]
-1.00E-06
[I] x [Fe2+]
-2.00E-06
[I] x pH
1.70E-05
[H2O2] x [Fe2+]
-3.00E-05
[H2O2] x pH
2.00E-05
[Fe2+] x pH
-6.30E-04
S 0.08 0.04 0.04
S 0.17
R2 61.38 92.50 95.76
R2 92.24
167
Table 6.6 – Urine models with S and R2 values
URINE Linear Linear w/squares Quadratic URINE Multiplicative
Linear
Linear
Constant 9.28E-02 1.86E-01 1.02E-01
Constant -3.39E-01
[I] -2.50E-05 8.90E-05 -2.30E-04
log[I] -3.37E-01
[H2O2] -9.00E-05 -1.22E-04 -2.47E-04
log[H2O2] 7.90E-03
[Fe2+] 2.38E-04 2.47E-03 9.33E-03
log[Fe2+] 2.20E-01
pH -1.02E-02 -6.29E-02 -2.06E-02
log[H+] 1.33E-01
Squares
[I] x [I]
-1.00E-06 1.00E-06
[H2O2] x [H2O2]
1.00E-06 -1.00E-06
[Fe2+] x [Fe2+]
-5.00E-05 -1.41E-04
pH x pH
5.56E-03 1.12E-03
Interactions
[I] x [H2O2]
-1.00E-06
[I] x [Fe2+]
2.00E-06
[I] x pH
2.90E-05
[H2O2] x [Fe2+]
5.00E-06
[H2O2] x pH
4.20E-05
[Fe2+] x pH
-1.25E-03
S 0.02 0.01 0.01
S 0.17
R2 59.52 79.59 95.81
R2 83.42
DILUTED URINE Linear Linear w/squares Quadratic
DILUTED URINE
Multiplicative
Linear
Linear
Constant 1.19E-01 2.41E-01 2.30E-01
Constant 2.08E-01
[I] -1.60E-04 -1.31E-03 -1.05E-03
log[I] -6.35E-01
[H2O2] 6.14E-04 9.10E-05 -1.63E-04
log[H2O2] 5.05E-02
[Fe2+] -1.33E-03 -8.40E-04 -5.40E-04
log[Fe2+] 1.43E-01
pH 2.33E-03 -1.10E-03 -5.50E-03
log[H+] 3.39E-02
Squares
[I] x [I]
1.00E-06 1.00E-06
168
[H2O2] x [H2O2]
3.00E-06 2.00E-05
[Fe2+] x [Fe2+]
4.70E-05 6.20E-05
pH x pH
-7.70E-04 4.00E-04
Interactions
[I] x [H2O2]
-1.00E-06
[I] x [Fe2+]
-
[I] x pH
-
[H2O2] x [Fe2+]
-4.00E-06
[H2O2] x pH
1.10E-04
[Fe2+] x pH
-1.54E-04
S 0.03 0.01 0.01
S 0.08
R2 76.14 95.08 95.39
R2 95.39
The prediction of degradation time holds high importance for the technical applications, therefore
optimization of the models has been assayed. The problem is broken down to maximizing an objective
function k = f (Iohexol, H2O2, Fe2+, pH). The optimization took place through the desirability function
(Derringer and Suich 1980, Papoutsakis et al. 2015b). This method allows the simultaneous optimization
of several equations. The desirability function for each equation is given by the following expression (6.3):
(6.3)
Since normalization of the parameters has taken place, the R different desirability functions d can be
combined to the (overall) desirability function, for the k constant, as follows (6.4):
(6.4)
R is the number of functions,
d the desirability of each function and
D the desirability of the system.
169
The optimization results are presented in Table 6.7, showing the desirability function values and the
operating regions. As it appears, the optimal region for maximizing the k constant is when Iohexol is
minimal, as the addition of higher amounts of Iohexol changes dramatically the k values. As expected, for
the linear models we found the optimum at the border of the experimental domain.
Table 6.7 – Optimal regions for treatment Iohexol through optimization by the desirability function.
Wastewater Iohexol H2O2 Fe2+ pH D Urine Iohexol H2O2 Fe2+ pH D
Linear 10 1000 50 lowest 0.3947 Linear 10 1000 50 lowest 0.7815
Quadratic 10 1000 32.3 7 1 Quadratic 10 1000 22.7 lowest 1
Diluted WW Iohexol H2O2 Fe2+ pH D Diluted UR Iohexol H2O2 Fe2+ pH D
Linear 10 1000 50 lowest 0.7401 Linear 10 1000 50 7 0.7829
Quadratic 10 1000 1 7 1 Quadratic 10 1000 1 7 0.9986
For the quadratic model in the undiluted matrices, the gains from the increase of the Fe2+ amounts starts
to get mitigated and values around 20-30 ppm are suggested. This is probably caused by the physical
blocking of UV light by the iron particles. Between WW and UR, the difference is found in the Fe2+ amount
added, as more iron is suggested in the case of WW. Since in UR acidification of the matrix was
recommended, less iron was suggested for the optimal performance in this case. Also, Fe2+ is an efficient
HO● scavenger, hence higher amounts will not necessary mean more advantageous performance. As far
as the desirability of the proposed operating regions is concerned, the linear models did not produce
solutions very close to D=1. On the other hand, the quadratic models often found the optimal regions and
the desirability of the system is ~1.
In conclusion, our statistical approach resulted in models with satisfactory performance (based on S and
R2 values). However, the optimization with a single response variable is relatively blindsided by other
factors, such as the cost of the process. In that case, the optimal region would be a compromise among
the efficiency and the cost. It is recommended that the quadratic model has to be preferred but in further
work, more response variables should be taken into consideration, such as involving the cost of reagents,
iron reclamation, residual H2O2 elimination, pH neutralization and others as in other works (e.g.
(Papoutsakis et al. 2015b).
170
6.3.3. Analytical approach – Global measurements (COD, TOC, and UV-vis absorbance)
combined with specific HPLC and MS analysis
The combination of the findings of the previous two parts do not fully support the idea of using H2O2 to
enhance the degradation efficiency of Iohexol in aqueous matrices. Therefore in this part, an effort has
been made to decode the reasons behind this effect and propose the proper operational conditions under
a new prism.
In Figure 6.4 (a-d) we present the profiles of the transformation products (TPs) by Peaks (area) vs. time
graphs. The operational conditions were set to Iohexol at 1000 ppm and H2O2 logarithmically increasing
from 0 (UV photolysis) to 1000 ppm (highly oxidative conditions). In all figures, the treatment was stopped
after 11 hours and the colored lines of the graphs represent the TPs by their elution time, corresponding
to Iohexol and the generated by-products under the different studied conditions. We have excluded the
peaks below 3.5 min elution time as they represent highly-polar aliphatic acids, with low absorbance and
non-linear correspondence to the UV detector set at 254 nm. Also, a representative chromatogram can
be found at the supplementary material (Figure S2).
As it can be observed, the degradation of the parent compound is proceeding in all cases as time
progresses (peak at 10.12 min) towards complete elimination, but achieved only when 100 and 1000 ppm
H2O2 were used. During the degradation of Iohexol, intermediate peaks appear in distinctive times,
representing the more polar by-products resulting from the elimination of Iodine atoms, the -OH addition
and the side chains breakage from the central aromatic ring. Also, it can be observed that increasing the
H2O2 concentration also leads to faster peak maxima in mid-range intermediates. This effect is profound
at 1000 ppm addition, where the fastest oxidation of the lower range intermediates is observed. In terms
of peak areas, Figure 6.4d shows the lowest areas, thus demonstrating the effect of H2O2. The HPLC
method used for the analysis of Iohexol was set at 254 nm, which is in-between the maximum absorbance
of the central aromatic ring (Weast 1985), and therefore, the detected intermediates have their central
ring intact. Since H2O2 addition has caused lower detection in overall, it means that it actively contributes
to the mineralization of the parent compound and the generated by-products, due to the non-selectivity
of the HO● radicals.
171
Figure 6.4 – HPLC peak areas evolution during Iohexol degradation by the UV photolytic and
photocatalytic process. A) UV only, B) 10 ppm H2O2, C) 100 ppm H2O2, D) 1000 ppm H2O2. 100 ppm of
Iohexol was chosen as initial spiking.
In order to assess the extent of mineralization, further investigation was initiated, focusing in the
degradation of the compound and the reduction of organic load in the bulk. The three tests assayed and
presented in Figure 6.5 are UV, UV/H2O2 and UV/H2O2/Fe2+ process. Enhancing the UV degradation process
with H2O2 and then with Fe2+ and H2O2 inflicted a t90% reduction of 40 and 50% respectively for the two
aforementioned additions. Nevertheless, the addition of iron enhanced only the early stages of the
treatment, as the time necessary for complete elimination was similar with the UV/H2O2 process alone.
Furthermore, the COD evolution shows a very similar behavior for UV photolysis and UV/H2O2 oxidation.
Up to 30 min of treatment, the two processes are quasi-identical which means that there is transformation
to more readily oxidized forms of carbon rather than actual degradation of the total carbon content. On
172
the other hand, the presence of iron in the solution that enhances the hydroxyl radical generation
demonstrates an immediate and constant rhythm of reduction. Most probably, the degradation pathway
of the combined UV/H2O2/Fe2+ process has different steps than the oxidation process, such as enhanced
side chains breakage instead of simple substitutions.
Figure 6.5 – Iohexol elimination by the UV-based AOPs. Iohexol degradation was followed by HPLC
(blue trace), COD (red trace) and TOC decrease (green trace) during the following treatment methods:
UV photolysis (trace: ), UV/H2O2 process (50 ppm H2O2, trace: ), and UV/H2O2/Fe2+ process (5 ppm
Fe2+, 50 ppm H2O2, trace: ). H2O2 reduction: brown traces. A system employing 35-W UV-C lamps
(instead of the 11-W ones of the previous parts, but otherwise identical) was used here. 100 ppm
Iohexol was chosen as initial spiking.
Finally, as far as the TOC removal is concerned, the compound confirms its highly recalcitrant behavior,
with the three processes demonstrating similar and limited reduction for the first 15-20 mins. After the
total (parent) Iohexol removal, the TOC is further reduced, up to 30 and 55% for UV/H2O2 and
UV/H2O2/Fe2+, respectively. This TOC removal justifies experimentally for the first time so far in this
investigation that extended treatment in presence of H2O2 and Fe2+ will eliminate the majority of the
organic carbon present in the solution.
If we consider the Average Oxidation State as a normalized measure to assess the overall oxidation state
of the solution (Bandara et al. 1997), we get:
173
(2.6)
where COD and TOC values are expressed in mol O2/L and mol C/L, respectively, and ranges from -4 (fully
oxidizable, e.g. CH4) to +4 for CO2 (completely oxidized)
For each case, for time 0 to time 120 min:
A) UV AOS: from 0.1 to 0.25
B) UV/H2O2 AOS: from 0.1 to 1.03
C) UV/ H2O2/Fe2+ AOS: from 0.1 to 3.24.
As it appears, for the same conditions, only with a moderate iron addition, the overall system did not
leave residual H2O2, which strengthens the economic design of the system and secondly, the overall state
of the system demonstrates an almost complete carbon elimination. Also, as H2O2 in high amounts is toxic
to microorganisms, complete elimination during treatment will reduce the post-treatment removal costs.
Therefore, apart from the Iohexol removal, which is moderately enhanced, the intermediates can be
effectively removed, which is often a common question when treating (recalcitrant) pharmaceuticals
(Malato et al. 2009, Sarria et al. 2003).
What was made evident, is that the degradation process differs among the three processes. For this
reason, the degradation products from the different treatment methods (after 5 min) were identified by
HPLC-HR-MS analysis according to the corresponding spectral characteristics: mass spectra, accurate mass
and characteristic fragmentation. Supplementary Tables S2.1 and S2.2 show the molecular formulas,
double bond equivalent (DBE), theoretical and experimental masses along with mass accuracy (∆m)
expressed in ppm.
In order to depict the differences, a synthetic representation of the intermediate products is shown in
Figure 6.6. For all the studied treatment methods, the degradation of Iohexol starts by scission of iodine
from the aromatic ring and subsequent addition of -OH at iodo-sites, which results in single or double de-
iodination, forming the phenolic products P1 and P6. Additionally, two more products were produced via
direct attack of HO on the side chain of Iohexol molecule (C1 and P3), with ketone formation and side-
chain breakage, respectively. Identified products are in the agreement with some products identified by
other authors (Jeong et al. 2010).
After P1, the degradation continues with HO attack on side chains via oxidation, -OH addition and
decarboxylation reactions, as seen in relevant works (Jeong et al. 2010, Tian et al. 2014, Zhao et al. 2014),
with minor differences between the treatments (different color arrows). Indeed, the influence of the UV
irradiation is the main actor in the degradation process. However, degradation at P1, which also includes
174
HO attacks by treatment B and C (UV/H2O2 and UV/H2O2/Fe2+) continues with the loss of a second iodine
atom, resulting to product P6. At this point, the degradation with UV (treatment A) is finished. The biggest
differences in the products appeared after P6 degradation, with four products identified for treatment B
and three for treatment C. The degradation of the P6 product is a pathway that is based on UV exposure,
as all processes, but proceeds further only in presence of H2O2 and/or Fe2+. The structure of these by-
products suggests that the degradation continues via the removal of the third iodine atom, plus further
oxidation and decarboxylation of side chains. However, the appearance of unique and different products
for treatments B and C imply that formation rate of HO plays crucial role in all stages of the degradation
process. Also, it is also noteworthy that in several pathways the formation of a non-ring hydroxylated
derivative of Iohexol is derived from ring-hydroxylated TP of Iohexol, which is rare, but has occurred again
in relevant literature (Csay et al. 2012, Jović et al. 2013).
Figure 6.6 – Overall mechanistic degradation pathway of Iohexol treated by UV-based AOPs. Products
common for all three treatments were marked with P, UV marked with A, for UV/H2O2 with B and for
UV/H2O2/Fe2+ with C. Products common for A and C treatment were marked as AC, and accordingly,
products common for B and C treatment were marked as BC.
Additionally, the use of Fe2+ and its affinity to the side chain structures, results to their higher substitution
or breaking. From the products’ structure, it could be concluded that the addition of iron is increasing the
efficiency of the treatment, giving products with shorter side chains (products C4 and C5), and even
nitrogen removal (product C4). The presence of hydroxyl radicals is responsible for their further
degradation, as well as for the oxidation of the side chains removed. The MS analysis at 5 min corroborates
175
with the HPLC results, which detection took place at 254 nm, indicating that the aromatic ring remains
intact. Nevertheless, at 15 min, there is identified presence of products without iodine atoms, with the
aromatic ring, but with degraded side chains. Finally, the absorbance spectra (see supplementary Figure
S3) shifts significantly after 15 min of treatment, there are no exclusive UV pathways and mineralization
initiates after this point, therefore we can conclude that the processes B and C involving HO attacks and
especially C, are the most efficient. The addition of iron is strongly recommended for efficient parent
compound and by-product degradation.
6.4. Conclusions
Iodinated contrast media, such as the investigated Iohexol, can burden the environment with their
presence for a relatively long time, due to their refractory nature. Since AOPs gained more attention over
the last decades, the abilities of the synthetic UV/H2O2/Fe2+ process were assayed. To achieve efficient
degradation and deep insight on the inactivation pathway, in the present work we assessed three
approaches in degrading this drug, namely the operational parameter testing, the statistical optimization
and the analytical chemical investigation.
As it appears, the dominant driving force in Iohexol degradation is the UV-C irradiation. The undertaken
assays however, showed that the t90%, as a measure of comparison among the various experiments, can
be moderately reduced if H2O2 and/or Fe2+ are added in the bulk. Also, depending on the matrix used,
dilution was proven very effective in reducing organic matter and solids concentration, thus enhancing
the removal of Iohexol.
The process was very well described by a quadratic model, which provided the best prediction of the
kinetics constant for both wastewater and urine, and diluted or undiluted matrix. Also, a multiplicative
model was produced, which sustained adequate accuracy while offering a simple formula. Additionally,
the target of indicating the optimal operation regions for Iohexol degradation was achieved.
Finally, evidence for the main degradation actor and the evolution of the process, as well as the
intermediates formed during the degradation of the parent compound were obtained. H2O2 and Fe, while
macroscopically had a modest effect, their contribution in the mineralization is noteworthy. This is of high
importance, as the ICM are notorious for their recalcitrance and their subsequent presence in the
environment. Hence, although initially H2O2 and Fe2+ presence seem as an economic side-effect, our
investigation suggests the optimization of their quantities and their addition to the UV process, which can
effectively reduce the organic pollution in the subsequent matrices.
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7. Chapter 7 - Solar photo-Fenton and UV/H2O2 processes
against the antidepressant Venlafaxine in urban
wastewaters and human urine. Intermediates formation
and biodegradability assessment.
Published work:
Stefanos Giannakis, Idriss Hendaoui, Milica Jovic, Dominique Grandjean, Luiz Felippe De Alencastro,
Hubert Girault, and Cesar Pulgarin (2017). Solar photo-Fenton and UV/H2O2 processes against the
antidepressant Venlafaxine in urban wastewaters and human urine. Intermediates formation and
biodegradability assessment. Chemical Engineering Journal 308, 492-504.
Web link:
http://www.sciencedirect.com/science/article/pii/S1385894716313286
Supplementary material:
Appendix F
Doctoral Candidate’s contribution:
Main investigator and author.
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7.1. Introduction
During the last years, there is a lot of word on the new challenges and problems that have emerged in
Environmental Engineering and more specifically, wastewater (WW) treatment. Water scarcity and reuse
(Jimenez and Asano 2008), emerging pollutants (Richardson and Ternes 2005) and the rise of antibiotic
resistance (Rossolini et al. 2014) are only a few that are closely related to the absence of potent measures
to limit or mitigate their effect. With that being said, wastewater treatment plants (WWTPs) hold their
fair share of blame for inefficiently stopping some of the new threats.
One of the most crucial problems the WWTPs face, and is connected with the improvement of life
standards globally, is the perception of illness and the ways drugs are administered nowadays. Apart from
the physical illnesses, injuries etc. which require antibiotics, sanitizers and similar products, the taboos of
psychological conditions have crumbled and as their recognition as illnesses is established, treatment is
now considered as nothing out of the ordinary. The intense ways of living have been proven to increase
the stress levels of people, leading to anxiety and chronic symptoms, as serious as sleep deprivation or
depression (Melchior et al. 2007). The administration of proper medication has led to the second problem
WWTPs have to face: emerging contaminants.
Venlafaxine (VFA, brand name: Effexor XR, Lanvexin or Trevilor), is an anti-depressant, which belongs in
the general family of selective serotonin and norepinephrine reuptake inhibitors (SSNRIs) (Andrews et al.
1996, Harvey et al. 2000). Practically, it treats depression, anxiety and panic disorders by increasing the
concentrations these natural substances in the body and brain of the patient (USNLM 2016a, Weller et al.
2000). Chemically, it belongs to the class of benzene and substituted derivatives and is a tertiary amino
compound that is N,N-dimethylethanamine substituted at position 1 by a 1-hydroxycyclohexyl and 4-
methoxyphenyl group (Table 1). Its excretion from the body follows the renal route, ends up in WWTPs
and therefore is found in natural waters, as VFA and its metabolites are escaping in almost 50% rate the
wastewater treatment process (Lajeunesse et al. 2012, Metcalfe et al. 2010, Rúa-Gómez and Püttmann
2012, Stadler et al. 2015). Measured concentrations range from 18 to 122 ng L−1 for VFA (Rúa-Gómez and
Püttmann 2013), or 102 and 690 ng L−1 (Rúa-Gómez and Püttmann 2012, Schultz et al. 2010) which could
affect the natural biota.
Since this compound lacks functional groups that hydrolyze under environmental conditions (pH 5 to 9),
hydrolysis is not expected to be an important environmental process, and therefore the risk of
bioaccumulation is possible. With an estimated bio-concentration factor (BCF) of 60, the potential for bio-
concentration in aquatic organisms is classified as moderate (USNLM 2016b). Furthermore, the exposure
experiments of Bisesi et al. (Bisesi et al. 2014) have indicated that Venlafaxine exposures of bass increased
time to capture their prey (minnows), and the analysis of brain tissues revealed that VFA caused decrease
179
in brain serotonin concentrations, thus explaining the behavior changes. Fong and Molnar (Fong and
Molnar 2013) investigated the biological effects of antidepressants comprising VFA on the mollusks and
crustaceans, i.e. foot detachment, a potentially sub-lethal effect that could result in transport to
unfavorable habitats for the target organisms; VFA exposure caused this effect even by exposure to
concentrations significantly lower than the ones found in WWTP effluents (Fong and Ford 2014). The
question is due to the food chain and cycle of water, how this is going to demonstrate on human beings.
As there risks similar to VFA in WW are increasing, WWTPs need to adapt to modern era threats more
effectively. Under this spirit, the new Swiss regulations for wastewater treatment include a list of 12
priority contaminants for elimination from WWTPs, and VFA has become one of the recent additions to
that list (Giannakis et al. 2015c). The said regulation involves the upgrade of WWTPs to employ activated
carbon, ozone or another advanced oxidation process (AOP) and ensure 80% removal of the chosen
micropollutants. As it appears, AOPs can play an important role acting as a barrier for contaminants of
emerging concern before reaching natural waters (Comninellis et al. 2008).
Recently, works have been initiated on the degradation of VFA by UV/H2O2 and TiO2 photocatalysis
(García-Galán et al. 2016, Lambropoulou et al. 2016) dealing with the elucidation of the degradation
pathway by these methods and also focusing on the toxicological safety of the degradation by-products.
To contribute to this end, in our work we employ 5 Advanced Oxidation Processes (UV, UV/H2O2, solar
light, Fenton, solar photo-Fenton) to degrade VFA in the matrices mostly expected to be encountered.
After a systematic investigation of the opportunities and pitfalls of treatment in water, urban wastewater
effluents and human urine containing VFA are employed and the degradation efficiency is assessed.
Finally, we investigate the degradation pathway of VFA inflicted by the various AOPs and explore the use
of AOPs as a pre-treatment step to increase the biodegradability of this contaminant with the Zahn-
Wellens tests.
7.2. Materials and methods
7.2.1. Chemicals and reagents
The chemicals for the experiments were used as received. Venlafaxine HCl (see Table 7.1) was acquired
from TCI (Germany), the HPLC solvents (acetonitrile, acetic acid and ammonium acetate) and the Fenton
reagents (hydrogen peroxide 30% and iron sulfate heptahydrate) were acquired from Sigma-Aldrich
(Switzerland).
Table 7.1 – Venlafaxine characteristics and physicochemical properties (USNLM 2016b).
180
Compound Chemical structure
Molecular
Weight
(g/mol)
Water solubilit
y
(mg/L)
log kow pKa
Henry’s coefficient
(H)
(atm.m3/mol)
HO• reaction rate constant
(M-1.s-1)a,b,c,d,e
Venlafaxine
C17H27NO2
277.402
267 3.20
10.01 2.0 x 10-11
(8.15±0.4)x109
(8.46±0.5)x109
(8.8±1.5)x109
1010
a: (Wols et al. 2013), b: (Santoke et al. 2012), c: (García-Galán et al. 2016), d: (Abdelmelek et al. 2011), e:
(Lee et al. 2014)
7.2.2. Water, wastewater and urine matrices
The preparation of the synthetic matrices involved dissolution of 100 mg/L VFA in either Mili-Q (MQ)
water (18.2 MΩ cm-1), synthetic wastewater (SWW) or synthetic urine (SUR). The composition of the
synthetic matrices is presented in Table 7.2. Real wastewater samples were collected from the local
wastewater treatment plant of Vidy, Lausanne (Switzerland), after an activated sludge process, a moving
bed bio-reactor or a coagulation-flocculation unit. The corresponding (initial) concentrations before
treatment were determined by HPLC/MS and were around 300 ng/L. For the real urine experiments, 10
μg/L VFA was added prior to experimentation.
Table 7.2 – Composition of the synthetic matrices used in this study.
Synthetic Wastewater
Name Chemical formula SWW composition [mg/l]
Peptone - 160
Meat Extract - 110
Urea CH4N2O 30
Dipotassium Phosphate HK2PO4 28
Sodium Chloride NaCl 7
Calcium Chloride dihydrate CaCl2·2H2O 4
Magnesium Sulfate Heptahydrate MgSO4·7H2O 2
Synthetic Urine
Name Chemical formula SUR composition [g/L]
Urea CH4N2O 25
181
Sodium Chloride NaCl 2.925
Sodium Sulfate Na2SO4 2.25
Potassium chloride KCl 1.6
Potassium phosphate monobasic KH2PO4 1.4
Calcium Chloride dihydrate CaCl2·2H2O 1.103
Creatinine C4H7N3O 1.1
Ammonium chloride NH4Cl 1
7.2.3. Light sources and corresponding reactors-experimental apparatus
For the UV and UV/H2O2 experiments, two double-wall, water-jacketed glass batch reactors were used in
parallel. The sample was placed within and the lamps, covered by a quartz sleeve were then submerged
in it. The monochromatic, Hg discharge UV-C lamps were 11-W Philips TUV mini (11W/G11 T5 UV) with
I11W = 26 μW/cm2. For the real WW and UR tests, a 35-W lamp was used instead. For protection of the UV
equipment and standardized conditions, water at 22 °C was recirculated with a Neslab RTE-111
thermostat.
For solar and photo-Fenton experiments, a Hanau Suntest CPS solar simulator was used, employing a
1500-W Xenon lamp, equipped with UVC and IR cut-off filters. The intensity was set at 900 W/m2 and
temperature was kept below 38 °C at all times by air-cooling. The Pyrex-glass reactors were kept in
constant agitation (350 rpm) by magnetic bars. The (dark) Fenton tests were performed in identical
reactors and conditions without providing light to the system.
7.2.4. Analytical methods
7.2.4.1. Venlafaxine determination routine by HPLC
The determination of Venlafaxine concentration was performed through HPLC. An HP 1100 Agilent series
HPLC was used. Briefly, the mobile phase consisted of 0.14 M ammonium acetate buffer, (1.079 g/L
acidified with glacial acetic acid (pH = 4). This was then mixed with 10% methanol/acetonitrile solution
and sonicated for 15 min. Finally, filtration from 0.45 μL membrane was done. The HPLC conditions
consisted of 40 °C temperature, 20 μL injection volume, RP-C18 column (4.6mm x 250 mm) and detection
of the peaks at 254.4 nm.
7.2.4.2. Venlafaxine quantification by UPLC/MS in real WW and RU
An online SPE-UPLC®/MS-MS (Acquity Xevo-TQ, Waters) was used. Samples were acidified to pH = 2.0
(32% hydrichloric acid), spiked with a standard mixture of surrogate, containing the MPs in deutered form
and filtered with glass fiber filter (Simplepure PP+GF, 0.22 μm, 25 mm, BGB). Standard solutions have
182
followed the same preparation. Five ml of each sample were loaded on an SPE column (Oasis HLB 25 μm,
2.1 x 20 mm, Waters) with ultrapure water, acidified at 1% of formic acid, as eluent. The online transfer
of VFA to the analytical column (Acquity HSS T3, 1.8 μm, 2,1 x 100 mm, Waters) was made with a gradient
of ultrapure water and acetonitrile acidified at 0.1% of formic acid. Multiple reaction monitoring mode
with two transitions was used to detect MPs and quantification was performed with internal standard
calibration.
7.2.4.3. Intermediates identification by TOF-MS analysis
HR-MS analyses were conducted on a Xevo G2-S QTOF mass spectrometer coupled to the Acquity UPLC
Class Binary Solvent Manager and BTN Sample Manager (Waters, Corporation, Milford, MA). Mass
spectrometer detection was operated in positive ionization using the ZSpray™ dual-orthogonal multimode
ESI/APCI/ESCi® source. Samples were diluted in H2O and directly infused into the mass spectrometer at a
flow rate of 100 μL/min. The TOF mass spectra were acquired in the sensitive mode over the range of m/z
50-1200 at an acquisition rate of 1 sec/spectra. A mass accuracy better than 5 ppm was achieved using a
leucine-encephalin solution as lock-mass (200 pg/ L in ACN/H2O (50:50)) infused continuously using the
LockSpray source (5 sec reference Scan frequency). Source settings were as follows: cone, 25V; capillary,
3 kV, source temperature, 120° C; desolvation temperature, 500° C, cone gas, 100 L/h, desolvation gas,
500 L/h. Data were processed using MassLynx™ 4.1 software.
7.2.4.4. Global chemical analyses (TOC, COD, H2O2 and UV/Vis Absorbance)
The COD of the solution was monitored with HR/LR dichromate vials (HACH Lange, Switzerland) and TOC
was followed by a Shimadzu TOC-VCSN analyzer, with an ASI-V automatic sampling module. H2O2 was
determined spectrophotometrically, after the addition of 10 μL of titanium oxysulfate in 1 mL of sample
and measurement at 410 nm (DIN 38402H15 method). Finally, the absorbance spectra was recorded at
each sampling point (Shimadzu 1800 UV spectrophotometer) and the pH was followed by a Mettler-
Toledo Seven Easy pH meter.
7.3. Results and Discussion
7.3.1. UV-based AOPs degradation of Venlafaxine
7.3.1.1. Monochromatic UV-C photolysis
Figure 7.1 presents the photolysis of Venlafaxine (VFA), under the exposure to monochromatic UV-C (peak
at 253.7 nm) irradiation. The photolysis rates, quantum yields and the proven, but limited efficiency to
degrade VFA by UV light in a collimated beam apparatus have been recently documented (García-Galán
et al. 2016, Wols et al. 2013). The kphot has been in the order of 1.5x10-4 cm2/J in the corresponding work.
183
0 10 20 30 40 50 60 70 80
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
TOC COD VFA
ln(C
/C0) VF
A
Dose (mJ/cm2)
0 10 20 30 40 50 60 70 80
0.0
0.1
2.2
2.3
2.4
COD/TOC ratio Asymptotic fit
CO
D/T
OC
ratio
Dose (mJ/cm2)
Figure 7.1 – Summary of the UV-C photolysis experiments. a) UV-induced degradation of Venlafaxine
followed by HPLC, COD removal and TOC reduction during UV photolysis. b) Evolution of the COD/TOC
ratio.
In our work, a merry-go-round reactor with submerged lamp was employed and the corresponding
kinetics are depicted in Figure 7.1. In principle, the degradation follows a linear trend in (natural)
logarithmic scale which allows the determination of first-order reaction rate constant, being 0.0104
cm2/mJ, calculated as follows:
(7.1)
or as:
(7.2)
By re-arranging the equation 1, we get:
(7.3)
Due to the reactor design and configuration, the actual irradiance received by the system and determined
by iodide/iodate actinometry (Rahn 1997) is 0.005 mW/cm2, which is much higher than the collimated
beam apparatus. Since the degradation follows first-order kinetics, the time necessary to degrade 90% of
the initial concentration (t90%) has been determined and will be used for comparison among the various
processes. From (7.3), by substitution we get:
(7.4)
or:
184
(7.5)
The required time for 90% was 163 min and until the t90% was reached, the UV-C system removed 7% and
4% of COD and TOC. Even by extending the treatment for 4 h, UV-C alone is not sufficient to degrade more
than 20% of COD or remove more than 15% of TOC. As it appears, the complex VFA structure is affected
by UV in the double bonds present but light alone cannot efficiently mineralize the carbon content of the
solution attributed to the degradation by-products and intermediates. Figure 7.1b corroborates with the
findings, and the depicted COD/TOC ratio presents asymptotic, plateau-like tendencies. This reveals the
formation and accumulation of stable by-products, which after an initial fast oxidation, do not further
undergo significant modification or mineralization. Furthermore, Figure S1 of the supplementary material
also confirms this tendency, where the absorbance spectra indicate that although VFA is removed (1st
peak) a plateau is reached after 2 h of exposure, where a formation of intermediates is stable and fails to
proceed further. From the wavelength of the peak (260-280 nm) we postulate that the cyclohexanol cycle
is not affected by UV and the intermediate formation stops there.
7.3.1.2. UV/H2O2 Advanced Oxidation Process
Following the UV photolysis, the same set-up was used to induce UV/H2O2 advanced oxidation of VFA. As
such, in a H2O2 dosing optimization process 5 different H2O2 addition levels were tested, and the results
are summarized in Figure 7.2 (7.2a and 7.2b).
The homolytic disruption of the HO-OH bond results in the release of hydroxyl radicals (HO●) (Guo et al.
2013). The addition of H2O2 and the production of HO● has a direct effect on the degradation of
Venlafaxine. Hydroxyl radicals can act on molecules via oxidation, -OH substitution, as well as water
abstraction and decarboxylation, as seen in related works (García-Galán et al. 2016, Lambropoulou et al.
2016). These attacks drastically modify the properties of VFA and proceed to more efficient degradation
than UV alone.
0 5 10 15 20 25 30
0.0
0.2
0.4
0.6
0.8
1.0
5 ppm 10 ppm 20 ppm 50 ppm
ln(C
/C0) VF
A
Dose (mJ/cm2)0 10 20 30 40 50 60 70 80 90 100 110
0.0
0.2
0.4
0.6
0.8
1.0
2.0
2.2
2.4
COD/TOC
TOC COD H2O2
Ct/C
0
Dose (mJ/cm2)
185
0 5 10 15 20 25 30 35 40 45 50
0
2
4
6
8
10
12 t90%
H2O2 consumed
Initial H2O2
H2O
2 con
sum
ptio
n
0
25
50
75
100
125
150
175
t 90%
Figure 7.2 – UV/H2O2 Advanced Oxidation of Venlafaxine: degradation and process optimization. a)
Degradation of VFA by UV/H2O2 with addition of 5-50 mg/L H2O2. b) Evolution of COD/TOC ratio (for
50 mg/L initial H2O2 addition). c) Consumption of H2O2 (black axis and traces) and changes in the t90%
(blue axis and traces) as a function of initial H2O2 amounts.
The addition of even 5 mg/L H2O2 improved the VFA degradation 20% respectively, compared to the sole
UV experiments. VFA has –OCH3 and –OH groups that react fast when faced to hydroxyl radicals (order of
kHO ≈ 109 M-1.s-1 and 108 M-1.s-1, respectively), but also a –CN group that has a much slower rate constant
(kHO ≈ 107 M-1.s-1) (USNLM 2016b), hence the overall degradation rate will be determined by these groups
and the direct photolysis rate (kphot) when treated by the UV/H2O2 process.
The stepwise increase in H2O2 concentration reveals the changes in degradation kinetics and the
limitations of the employed experimental system (Figure 7.2a & 7.2b). After 50 mg/L the improvement in
reaction kinetics is marginal (data for 100 mg/L not shown). In addition, in (García-Galán et al. 2016) and
(Wols et al. 2013), the photolysis rate was considerably lower than the corresponding rate for oxidation
due to the hydroxyl radicals, and was considered negligible. Here, the oxidation kinetics are estimated as
follows:
(7.6)
Where, i: the H2O2 addition (mg/L).
Table 7.3 – Measured pseudo-first order degradation kinetics of Venlafaxine per AOP and matrix.
Pseudo first order reaction kinetics k (min-1)
186
UV alone MQ
0.0141
UV/H2O2 MQ
0.0392 1.78
0.0757 4.37
0.1412 9.01
0.2948 19.91
0.3726 25.43
Solar light MQ Synergy12.5|58.3 =
0.0002 89.46
Fenton (pH = 3) MQ
0.0026
photo-Fenton (pH = 3) MQ
0.0161
0.1443
0.1814
0.2505
0.2363
As an example, the kHO /kphot ratio was calculated 5.5 for 10 mg/L (more details are given in Table 7.3).
Hence, although these measurements reveal the high contribution of the photolysis in the process, they
can be partially attributed to the specific reactor geometry that has relatively short optical path, and light
attenuation is small. Therefore, this design influences the economical parameters of the degradation
process.
Nevertheless, the consumption of H2O2 increases with increasing addition. We further notice that the
overall oxidation of the system proceeds towards mineralization of the existing carbon content for each
case. A 4-h exposure to UV/H2O2 system with 50 mg/L H2O2 (i.e. for as long as there was H2O2 present) the
COD and TOC removal is improved compared to the plain UV system, and an additional 20% was removed
187
for both parameters. However, according to the absorbance spectra recorded, after the removal of VFA,
the remaining intermediates and by-products are not removed equally fast, and a lower second order kHO
must be in effect (detailed graphs can be found in the supplementary Figure S2).
7.3.2. Fenton-related AOPs degradation of Venlafaxine
In order to fully attribute the effects of the synthetic photo-Fenton process against the degradation of
VFA, a stepwise construction of the process took place. Hence, solar exposure, Fenton treatment in the
dark and the combined process took place and the results are presented in the respective groups. To our
knowledge, this is the first instance where VFA is systematically treated by the photo-Fenton process and
therefore, the different parts will be analyzed separately.
7.3.2.1. Solar photolysis of Venlafaxine
The experiments of simulated solar exposure of VFA were performed in order to establish solar photolysis
rates and check the potential photo-transformation of the drug. Santoke et al. (Santoke et al. 2012)
proved that Venlafaxine is undergoing limited photolysis. Here, after 24 h of irradiation at relatively high
solar irradiance (900 W/cm2) a mere 12% of the initial VFA amount has been removed. As such, a ksol =
0.0002 min-1 was measured (Table 7.3). As far as the COD and TOC of the solution are concerned, limited
removal was observed. COD was removed at 13% and 4% TOC was eliminated during the course of 24h
(for more details, see Supplementary Figure S2). However, the direct action of solar light includes 1) the
excitation of the organic compound at singlet-excited state (Ryan et al. 2011), 2) its intersystem crossing
to triplet state and 3) its reaction with oxygen to form singlet oxygen (Vione et al. 2014). Afterwards, the
micropollutant returns to ground state, but the singlet oxygen created by the reaction with water
participates in i) the superoxide radical anion formation from oxygen and consequently ii) to the formation
of H2O2 from water (Vione et al. 2014) or iii) the direct attack to double bonds present in the molecule.
Although of lesser importance, these results will play the role of reference when the photo-Fenton process
will be described from its parts.
7.3.2.2. Fenton-driven degradation of Venlafaxine in the dark
The degradation of VFA in the dark due to the Fenton reaction were assessed in a range of parameters,
such as the initial pH and the starting Fenton reagents concentration. Literature suggests that the
reactivity of Venlafaxine with hydroxyl radicals is ranging among 8x109 to 1010 M-1 s-1 (see Table 7.1). Figure
3 presents 4 of the Fe|H2O2 ratios tested (indicatively chosen), in the 3 different pH levels of operation,
i.e. 3, 5 and 7. The results of the optimization are summarized in Figure 7.3a (analytical data in
supplementary Figure S3a-S3c), for 24 h of treatment for each batch process.
188
5|10 5|50 12.5|30 20|501
10
100
1000
t 90% (h
)
Fe|H2O2 ratio
pH= 3 pH= 5 pH= 7
0 4 8 12 16 20 24
0.0
0.1
1.8
1.9
2.0
2.1
2.2
2.3
2.4
2.5
CO
D/T
OC
ratio
Time (h)
5|10 5|50 12.5|30 20|50-3 20|50-5 20|50-7
Figure 7.3 – Treatment of Venlafaxine by the Fenton process in the dark. a) Evolution of the t90% with
increasing Fe|H2O2 ratio and pH. b) COD/TOC ratio modification by the Fenton process at various
Fe|H2O2 ratios (pH=3) and increasing pH for a 20|50 (mg/L|mg/L) ratio.
As expected, Figure 7.3 shows that at pH=3 the results were optimal (see also Table 7.3), as the Fenton
process greatly benefits of the soluble iron at that pH (Pignatello et al. 2006). Although limited by the
regeneration of Fe3+ back to Fe2+, 3 out of the 4 processes were able to degrade more than 50% of the
initial content. These processes contained H2O2 in the highest amount, which played the role of the
reductant of ferric iron, as indicated in the following reactions:
● (1.8)
● (7.7)
● ● (7.8)
● ● (7.9)
● (7.10)
● (7.11)
● (7.12)
● ● (7.13)
189
The generation of the Reactive Oxygen Species (ROS) by the Fenton process is dependent on the catalyst
regeneration, i.e. the Fe3+ back to Fe2+. However, the reaction kinetics of equation 1.8 compared with the
others is orders of magnitude higher, and for this reason, the regeneration of the catalyst, especially by
Eq. 7.8, is considered a limiting step. In water, Fe3+ forms different aqua-complexes, according to its pH,
with precipitation tendencies as the pH increases. The iron speciation in water changes according to the
Pourbaix diagram and Salgado et al. (Salgado et al. 2013) have updated the original contribution, with the
most recent knowledge. At acidic pH, the most abundant form of iron is [Fe2+] which is the strongest
reductive form. The optimal value to perform the Fenton reaction is near 3; the rate increases with the
pH (Millero and Sotolongo 1989). After pH 4, the majority of the iron species are insoluble (Fe2O3, or other
colloidal forms) and therefore, the reactivity drops.
However, moving up to pH=5 the degradation potential are diminished and only the 20|50 addition
Fe|H2O2 ratio was sufficient to inflict a 70% degradation after 24 h. At pH = 7 even this ratio was limited
to a 35% degradation of VFA. Nevertheless, as 24 and 22 mg/L H2O2 were still measured after 24 h, the
process could continue, albeit in lower rates. At pH 5, solid Fe(OH)2 species dominate, since they are
more readily oxidized (compared to Fe2+ and FeOH+) (Morgan and Lahav 2007). Nevertheless, until pH 5.8
the contribution of the homogeneous photo-Fenton is still considerable (Barona et al. 2015). Finally
among pH 5 and 7 (up to 8), solid iron species dominate and no further increase in its concentration
appear (Morgan and Lahav 2007). However, at this pH HO2●─ is formed in higher quantities and indirectly
helps the Fe2+ formation through the Equation 7.12 (Papoutsakis et al. 2015b). The soluble iron species
have very different rate constants reported, which practically means that their participation in redox
reactions depends on the distribution of these species (Fe2+, FeOH+, and solid Fe(OH)2) (Morgan and Lahav
2007).
As pseudo-first order kinetics were established for the degradation process, the t90% was established for
each ratio and pH level. It can be observed that the theoretical t90% can reach 1000 hours in the near-
neutral pH and low Fe|H2O2 ratios, although increasing the amounts can reduce it to merely a day, which
is great improvement. The acidic pH on the other hand ensures proper removal and never exceeds 100 h
of treatment, while 11 h are necessary with high reactants concentration.
Finally, during the 24-h treatment by the Fenton process the mineralization rate of the organic matter
remains low for high pH and low concentrations of Fe and H2O2. The biggest removal noted was at pH=3
and 20|50 ratio. Nevertheless, the COD/TOC ratio indicates a fast initial degradation step and a
decelerated process afterwards. As no process was H2O2-limited for any pH or ratio, this indicates that the
VFA structure contains some easily removed groups, which readily react with the HO● radicals (see
supplementary Figure S4 and Table S1, for analytical COD & TOC measurements, and H2O2, respectively).
The corresponding absorbance spectra in Figure 7.4 indicate the formation of different intermediates and
190
complexes with iron, depending on the pH and the Fe|H2O2 ratio. Nevertheless, the VFA removal is
confirmed to be low for most cases, and the participation of the iron is demonstrated by the absorbance
in higher wavelength UV and visible light; Fe can bind to acidic groups or side-chains and create stable
organo-complexes. In Figure 7.4, axis x shows the wavelength (nm), y the absorbance (a.u.) and z either
the Fe|H2O2 ratio (left group) or the pH level (right group). Also, the stability of the solution after 6 h,
indicates the low levels of reaction with the organics present. However, these absorbance spectra
suggests that these complexes are photo-active, as they absorb UV and visible light in higher rates than
the original solution with iron (t=0) and therefore we anticipate their possible involvement in the photo-
Fenton process.
Figure 7.4 – Absorbance spectra during the 24-h Fenton treatment of Venlafaxine, for various Fe|H2O2
ratios (panels a-d) and pH levels (panels i-iii). Fe|H2O2 ratios: a) 5|10, pH=3. b) 5|50, pH=3. c) 12.5|30,
pH=3. d) 20|50, pH=3. pH levels: i) 20|50, pH=3. ii) 20|50, pH=5. iii) 20|50, pH=7.
7.3.2.3. The photo-Fenton driven degradation of Venlafaxine
The final step in this section considers the combined photo-Fenton process. In Figure 7.5, we summarize
the experiments performed, in a similar manner to the Fenton process. As pseudo-first order kinetics were
established, Figure 7.5a shows the evolution of t90% as the Fenton reactants and the pH levels increase
(detailed data on the photo-Fenton action can be found in the Supplementary Figure S5 and the H2O2
consumption at Table S1). A very similar trend with the Fenton process is observed, but the t90%, even the
theoretical one is now measured in minutes rather than hours. The synergy of the Fenton with light is very
high, yielding t90% as low as 10 min for 20|50 at pH=3.
191
5|10 5|50 12.5|30 20|501
10
100
1000t 90
% (m
in)
Fe|H2O2 ratio
pH= 3 pH= 5 pH= 7
0 30 60 90 120 150 180
0.0
0.1
1.8
1.9
2.0
2.1
2.2
2.3
2.4
2.5
CO
D/T
OC
ratio
Time (min)
5|10 5|50 12.5|30 20|50-3 20|50-5 20|50-7
Figure 7.5 – Treatment of Venlafaxine by the photo-Fenton process (irradiance: 900 W/m2). a)
Evolution of the t90% with increasing Fe|H2O2 ratio and pH. b) COD/TOC ratio evolution by the solar
photo-Fenton process at various Fe|H2O2 ratios (pH=3) and increasing pH for a 20|50 ratio.
As the mode of action of the Fenton process has been previously explained, here we will assess only the
changes and improvements inflicted by light. The most notable difference among these results and the
Fenton process in the dark, is the change in the time scale, from hour to minute range. Here, all
experiments were handled within 3 hours. Although some processes (5|10 ratio) did not conclude, the
great number of completed experiments within the experimental time demonstrates the efficiency of the
photo-Fenton process. In presence of light, the iron recycling is facilitated by the absorption of light by
the photosensitive aqua-hydroxy- and organo-complexes. At pH=3, the prevalent form is [Fe(H2O)5(OH)]2+;
in general, the photo-reduction can be summarized with the following two reactions (15-16), also leading
to an extra hydroxyl radical production:
(7.14)
● (7.16)
At higher pH, the contribution in radicals’ formation is reduced, along with the photo-active compounds
concentration. The production of the hydroxyl radical, as described before, induces hydroxylation of two
possible sites simultaneously or independently, or even reaction with the nitrogen group (Santoke et al.
2012), resulting to efficient degradation (Klamerth et al. 2012, Mackuľak et al. 2015).
As the mineralization rate indicates (figure 7.5b), he overall removal of organic matter in the solution stays
limited, within the duration of the experiment. According to the H2O2 consumption rates, and the residual
H2O2 at the end of 3h, which is lower than the respective after 24 in the Fenton process, the process is, or
will be H2O2 limited for some combinations. Hence, the COD and TOC removal is halting and re-dosing
192
would be necessary to continue the degradation (detailed COD and TOC measurements can be found in
the supplementary material).
Figure 7.6 – Absorbance spectra during the 3-h photo-Fenton treatment of Venlafaxine, for various
Fe|H2O2 ratios (panels a-d) and pH levels (panels i-iii). Fe|H2O2 ratios: a) 5|10, pH=3. b) 5|50, pH=3. c)
12.5|30, pH=3. d) 20|50, pH=3. pH levels: i) 20|50, pH=3. ii) 20|50, pH=5. iii) 20|50, pH=7.
Finally, the combined photo-Fenton process effects are also demonstrated in the changes in absorbance
spectra, in Figure 7.6. The photoactivity of the complexes remains high, which means an active ligand-to-
metal charge transfer could be facilitated:
● (7.17)
The sacrificial ligand is offered from either VFA or some intermediate and the regenerated Fe2+ will re-
participate in the Fenton reaction. The changes found can be grouped under either i) the higher complex
formation (higher absorbance) compared to the Fenton system, ii) the significantly faster plateau
achievement or iii) the bigger differences in the neutral and near-neutral process (differences between
pH=3 and 7).
7.3.3. Venlafaxine degradation experiments in wastewater and urine
7.3.3.1. Experiments in real secondary wastewater effluents and human urine
The occurrence of VFA and its metabolites in surface waters (Rúa-Gómez and Püttmann 2012) indicates
the improper elimination in WWTPs and their extreme adverse effects underlines the need for their
193
degradation prior to their discharge. Table 7.4 summarizes literature values and own measurements of
VFA in WWTPs, at various stages, from influents to effluents.
Table 7.4 – Occurrence and fate of Venlafaxine in urban WW effluents.
Venlafaxine occurrence in
WWTPs
Treatment stage
Quantity (ng/L) Source
Pre-
trea
tmen
t Influent
500-1100 (Metcalfe
et al. 2010)
800
(Rúa-Gómez
and Püttmann
2012)
623±18 Own
measurements
235±21 (Margot
et al. 2013)
Primary treatment 374±111
Own measure
ments
Seco
ndar
y Tr
eatm
ent
Biological treatment (high/low
HRT)
900-1000 (Metcalfe
et al. 2010)
Degradation of Venlafaxine (this work)
140-150 (Petrie et al. 2015) Measured pseudo-first order kinetics k (min-1)
95-188 (Margot
et al. 2013)
UV-C UV/H2O2 Solar Fenton photo-Fenton
AS 281±83 Own
measurements
0.073 nc 0.0001 0.006 0.033
MBBR 224+67 Own
measurements
0.08 nc 0.0001 0.007 0.035
CF 299+9 Own
measurements
0.042 nc 0.0001 0.001 0.032
194
Effluents 95-188 (Margot
et al. 2013)
In our work, we assessed the degradation of VFA with the same AOPs analyzed in the previous parts, in
the amounts found in three different secondary effluents, namely activated sludge (AS), moving bed bio-
reactors (MBBR), and coagulation-flocculation effluent. For more information on the nature and the
composition of the effluents, as well as COD and TOC removal, interested readers should refer to
(Giannakis et al. 2015c), (Cunningham 2004) and (Edberg et al. 2000) and the supplementary material
(Table S2). Figure 7.7 depicts the degradation measurements in the two families of AOPs per process and
per effluent. As expected, the UV-based AOPs presented the fastest degradation kinetics, as summarized
also in Table 7.4.
Figure 7.7 – Treatment of Venlafaxine by AOPs in urban WW effluents. The experimental conditions
are marked in the corresponding graphs. a) VFA degradation by UV-based AOPs in AS, MBBR and CF
effluents. b) VFA degradation by the Fenton-related processes in AS, MBBR and CF effluents.
Recent works have demonstrated their efficiency in VFA degradation by the Fenton and Fenton-like
processes (Mackuľak et al. 2016, Mackuľak et al. 2015), confirming the feasibility of its application in real
WW samples. Venlafaxine degradation is a function of contradicting factors in real effluents. On the
antagonists of the process, we can mention the i) suspended solids, blocking UV and solar light
transmission, ii) the Effluent Organic Matter (EfOM), consisting in still particulate organic matter (POM),
biodegradable organic matter, refractory organic matter and other MPs, which all compete for the
oxidants generated by AOPs (Giannakis et al. 2015c) and screen the light (Ryan et al. 2011), iii) the ROS
scavengers, such as (bi)carbonates, nitrate and nitrite (Vione et al. 2014), and iv) the microorganisms. On
195
the other hand, the very presence of some substances has been proven to enhance the self-purification
capabilities of the effluents, such as a) the presence of photo-sensitizable organic matter (PhOM), which
further produces ROS, and b) the nitrates and the carbonates, which contribute in producing nitrate
radicals, carbonate radicals and ROS, all with mild oxidative potential (Giannakis et al. 2015c). In the end,
what we perceive as “degradation” is the net force of all these factors, which leans on the negative side
overall, compared to simulated WW or water.
As far as the initial content is concerned, the similar values in AS and MBBR have been recently verified
(Margot et al. 2013) and the close values in CF effluents are a result of the low solubility and the
hydrophobicity, as expressed by the logkow; VFA tends to adsorb to the generated flocs and is “removed”
by settling. More specifically, the degradation kinetics follow a similar trend to the content of suspended
matter and organic content in the effluents, as well as the alkalinity of the matrix, an indicator of
(bi)carbonates content and therefore a precursor of HO scavenging. As shown in (Margot et al. 2013) and
Chapter 6, the physicochemical characteristics of the effluents measured, verify a trend, as MBBR has the
best characteristics, followed by AS and then CF.
Concerning the experiments in human urine, based on manufacturer, medical and pharmaco-kinetical
data, we have found that the normal dose of Venlafaxine (as Effexor) for patients is 75 mg/day and can
reach up to 150 mg/day in severe cases. Out of the administered amount, 92% is recovered in urine, as
the renal excretion pathway is prevailing. However, VFA in urine appears in only 5% (1-10%, (Metcalfe et
al. 2010), unconjugated O-desmethyl Venlafaxine (29%), conjugated O-desmethyl Venlafaxine (26%), 1%
N-desmethyl Venlafaxine, and the rest as the other intermediates. Hence, a normal person excretes ~2 L
urine per day, it is normal to expect μg/L concentrations in patients. As such, 10 μg/L spiking was
performed in urine collected by healthy individuals. The COD of the solution varied significantly from 2.5
to 8.5 g/L. Therefore, collection and homogenization over the course of 6h was performed to mitigate the
differences in chemical and optical properties. The average urine characteristics can be found in the
supplementary material (Table S2). Besides, 10% diluted urine experiments took place, to assess the
possibility of yielding higher UV transmittance in exchange of higher treatment volumes. The results of
the study are summarized in Figure 7.8.
196
Figure 7.8 – Treatment of Venlafaxine by UV-based methods in human urine. a) VFA degradation by
UV-based AOPs (0, 50 or 100 mg/L H2O2 and 0/100% or 10%-90% urine/water ratio. b) COD reduction
and DOC (0.45μm filtration) removal in the same conditions.
During the experiments in undiluted urine, the efficacy of UV alone in degrading VFA was low. As urine
contains light absorbing compounds (organic matter, nitro-, phosphoro- and other groups), light
attenuation was a limiting step in the degradation process (Iohexol, Chapter 6). The step-wise addition of
H2O2 (50 and 100 mg/L) was beneficial, reaching up to ~30% degradation of VFA. Other researchers have
also demonstrated the increase in PhACs’ degradation by the addition of H2O2 in the bulk (Zhang et al.
2015). The positive aspects of H2O2 addition are found also in the COD removal, where up to 15% of COD
and 13% of DOC were removed. In real urine, this amount corresponds to 750 mg/L, from a 5000-average
COD. Diluting the urine x10 times has modified the matrix significantly, allowing up to 80% degradation
of VFA (spiking was done after dilution) and the H2O2 addition further improved degradation, up to 100%.
An interesting correlation can be derived from the COD removal and the VFA degradation, where a 20%
removal of COD (or 15% DOC) was found to indicate the end of the VFA treatment period. Hence, this
process could be monitored by following global parameters instead of sophisticated LC/MS methods.
Furthermore, the dilution of urine has been studied in another contaminant (Iohexol, Chapter 6), and the
optimization experiments revealed that a near-optimal performance could be obtained by 10% dilution
of the matrix. The effect of dilution improves the transmittance of urine, thus improving light absorption
by the organic matter in solution, but also improve the homolytic disruption of H2O2, the subsequent
197
increase in HO● production and the decrease in scavenging by the organic matter. On the other hand, the
x10 times increase of the treated volume holds technical and engineering implications, as well as
questions on the water used for dilution. Here, as a proof of concept we have shown that the effects are
multiple and since the human urine production is small, even this dilution is not a limiting agent to a
potential application.
Finally, no photo-Fenton experiments were performed as the k in synthetic urine were too slow and the
treatment of urine in open vessels seems impractical. Nevertheless, medium (MP) UV lamps could be
suggested as a potential substitute for monochromatic UV or solar light, as they emit an array of peaks
and photo-Fenton reaction could be sustained.
7.3.4. Elucidation of the AOP-driven degradation pathway and inherent biodegradability
properties of Venlafaxine
7.3.4.1. Degradation pathway of Venlafaxine by AOPs through TOF-MS
The identification of degradation products is essential for providing the risk assessment information of
drug residues in the environment, as well as for the improvement of water treatment technologies. In our
study, Venlafaxine degradation products were identified after each degradation procedure (UV, UV/H2O2,
solar treatment, Fenton and solar photo-Fenton). All identified products were shown in supplementary
Table S3, including their molecular formula, theoretical and experimental m/z value, double bond
equivalent (DBE) and mass accuracy in ppm (accepted structures with error less than 5 ppm). Ten
degradation products were identified in overall: one for solar treatment, six for UV treatment, five for
UV/H2O2 treatment, seven for Fenton degradation and seven for photo-Fenton treatment. Based on the
identified structures, a simple mechanistic scheme was proposed (Figure 7.9).
Transformation of Venlafaxine can occur via four dominant reactions: 1) sequential hydroxylation of the
aromatic ring, 2) transformation of the methoxy- group, 3) hydroxylation and shortening of the
cyclohexanol ring and 4) attack on the nitrogen group.
Firstly, the degradation pathway of VFA was sequential hydroxylation: once hydroxylated VFA yielding
m/z 294.2072 (P8) was identified in all treatments except solar treatment; followed by di-hydroxylated
product with m/z 310.202 (P9) identified in UV, UV/H2O2 and photo-Fenton treatment; and tri-
hydroxylated product with m/z 326.1956 (P10) identified only in the UV treatment (Treatment B). The
sequence of the identified hydroxylated degradation products implies that UV light was the main driving
force in the multiple hydroxylation of the aromatic ring. Here, the identified products were also reported
in the literature (García-Galán et al. 2016, Lambropoulou et al. 2016, Lester et al. 2014, Santoke et al.
2012). Santoke et al. identified two products formed by the attack of HO● radical on the aromatic ring and
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the N-chain, but they were not identified in this study (marked with red dashed arrow in the degradation
pathway) (Santoke et al. 2012).
Figure 7.9 – Combined Venlafaxine degradation pathway through the application of the treatment
methods analyzed.
A second degradation pathway started with dehydrated Venlafaxine’s product m/z 260.2012 (P6),
identified in all degradation procedures. Combinations of dehydration and hydroxylation reactions
present a transformation pathway also dominant for VFA UV/TiO2 treatments (Lambropoulou et al. 2016).
HO● attack on the tertiary C-atom and cyclohexanol structure led to the formation of products with m/z
215.1431, m/z 229.1429 and m/z 292.1914; P4, P5 and P7, respectively.
Demethylation presents a well-known VFA transformation route in biological and chemical reactions (Boix
et al. 2016, Li et al. 2015, Santoke et al. 2012). Transformation of the methoxy group was identified within
the products m/z 121.0654 (P1), m/z 178.1231 (P2) and m/z 194.1182 (P3), which were at the same time
the final degradation products. Aliphatic nitrogen products identified by Garcia-Galan et al. (García-Galán
et al. 2016), were not identified in this study, however they were also included in the degradation scheme
(marked with blue dashed arrow in the degradation pathway) to complement the overall VFA degradation
routes. It should be noted that the structures of identified products for different UV/H2O2 treatments
depend not only on the reaction time, but also on the H2O2 concentration used in the experiments. Finally,
the appearance of apparent biodegradable compounds calls for assessment of the biodegradability
assessment of VFA and the AOP-treated effluents containing it.
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7.3.4.2. Zahn-Wellens (ZW) biodegradability test of AOP-treated Venlafaxine solutions
As literature suggests low removal of VFA in WWTPs, we assessed the biodegradability of VFA, by
subjecting it first through an AOP. This strategy has been successfully used in various effluents (Malato et
al. 2009, Sarria et al. 2003). Therefore, treatment of VFA solutions until 50% and 100% initial
concentration degradation, along with a reference compound (diethylene glycol) and untreated VFA were
subjected to a 28-day Zahn-Wellens inherent biodegradability tests (Lin and Ganesh 2013, Nataro and
Kaper 1998). In parallel, DOC was followed at the corresponding blanks (test suspension and inoculum
blank). In order to avoid self-inhibition problems, the initial VFA amount was reduced to 10 mg/L. The
results of the study are summarized in Figure 7.10.
Figure 7.10 – Zahn-Wellens inherent biodegradability test of Venlafaxine and treated solutions in MQ.
a) ZW test after treatment of 50% of the initial VFA solution. b) ZW test after treatment of 100% of the
initial VFA solution. Note that results are normalized towards the initial DOC to enable comparison.
First of all, the test is considered valid as 70% of the initial DOC of the reference compound has been
degraded (>72%) within 14 days. This indicates the suitability of the activated sludge inoculum. Secondly,
VFA alone was removed at 35%, which corresponds to similar degradation rates of VFA in biological
treatment facilities (see Table 7.4). As far as the applied AOPs are concerned, 50% pre-treatment of VFA
resulted in 20-25% biodegradability improvement. The most efficient process was the photo-Fenton
reaction, only by marginal difference. According to TOF- MS analysis for VFA in this work, and Orbitrap-
MS for Iohexol (Chapter 6), using AOPs where iron is involved always leads to enhanced modifications on
the target contaminant. If VFA was eliminated 100% a further 10-15% was achieved, depending on the
process. This indicates that over the course of 28 days, almost 70% of the initial DOC was eliminated,
reaching the threshold for considering the solution biodegradable. Of course, further treatment of the
parent solutions would achieve the threshold with greater ease, and correlation with the initial DOC
200
removal should be made instead. Hence, by extrapolation, it could be possible to propose a pre-treatment
step in industries or hospitals, where mass flows of similar contaminants are released, if the said facilities
do not employ their own WWTPs, as it would seriously ease the burden off the municipal WWTPs.
7.4. Conclusions
The ubiquitous presence of drugs in surface waters demands strict control frameworks and efficient
removal methods at the level of WWTPs. Under this scope, the degradation of the antidepressant
Venlafaxine was systematically investigated, through the application of 5 AOPs. UV-based technologies
(UV-C light alone and UV/H2O2) and Fenton-related techniques (solar photolysis, Fenton and photo-
Fenton oxidation) were assessed as control measures and their efficiency was estimated.
The investigation on the degradation kinetics has shown that Venlafaxine demonstrates moderate
photolysis under UV, and the addition of H2O2 with the simultaneous HO● generation enhances the
degradation potential of the chosen treatment. On the other hand, solar photolysis was found limited,
but in combination with the action of the Fenton process (in the dark), the photo-Fenton process was
efficient in degrading the contaminant, with decreasing, but not diminishing performance tendencies as
we approached the neutral pH.
The tests in wastewater and urine revealed a drop in efficiency, due to the presence of antagonists in the
matrix. Urban wastewater and human urine tests indicated that the actual conditions expected in the field
demand intensive treatment; in wastewater the degradation of Venlafaxine is subjected to similar
problems as most ng/L contaminants present, but the efficient removal is possible, and the human urine
experiments indicate an innovative treatment proposal, by the use of UV to collect and treat on-site the
emerging contaminants, and addition of H2O2, if high simultaneous DOC removal is desired, before
dispersion in the wastewater matrices.
The mechanistic interpretation (degradation pathway) based on our own TOF-MS experiments and recent
advances in the field revealed the opportunity of converting Venlafaxine to its bio-degradable
intermediates. The Zahn-Wellens tests performed showed that pre-treatment of Venlafaxine solutions
increases biodegradability, and under certain conditions, conversion of the mixture of intermediates into
biodegradable is possible.
In the light of the above findings, we conclude that the non-selective and highly oxidative character of the
Advanced Oxidation Processes is capable in controlling substances before their discharge in natural
aquifers and their upcoming environmental consequences. Environmental protection has a well-
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established ally in traditional contaminant categories (priority pollutants, organic matter) and the
application of AOPs can play a role of outmost importance towards this direction in the near future.
8. Chapter 8 - General conclusions, perspectives and future
work
In this thesis, the use of AOPs was selected towards pollutant decontamination and disinfection of
effluents. UV, UV/H2O2, solar light (shown to work as an AOP), Fenton and solar photo-Fenton are
established as powerful allies in the ongoing task of wastewater purification. From the various works
analyzed, the key conclusions are the following:
1) UV-based AOPs are efficient for MP removal and MO inactivation. Although changing dynamically,
the Swiss reality on hospital wastewater treatment dictates their discharge in the municipal
collection network, and therefore imply their co-treatment with municipal wastes. The UV-based
AOPs (UV and UV/H2O2) were found to be effective micropollutant removal strategies in ng/L level
and bacterial inactivating processes, after biological secondary pre-treatment, as found in
municipal wastewaters. When used in simulated hospital wastewaters and urine treatment, as
alternative micropollutant elimination strategies, their efficiency was measured and established
against a list of contaminants, with parallel elimination of the contained organic matter. The
degradation was fast although the engineering parameters and costs were not part of this study,
the reactants addition and necessary light doses were moderate.
2) The solar photo-Fenton process and its constituents can be very effective in the proper context.
Despite the lower apparent efficiency of this process when compared with its UV-based
counterparts, photo-Fenton was found to effectively and non-selectively remove micropollutants
and effluent organic matter. Furthermore, their application resulted in high bacterial removal,
regrowth suppression, yeasts and viruses inactivation from water and wastewater effluents. Most
importantly, through systematic studies the mechanism and the key points of the process against
the aforementioned targets were characterized. Special emphasis was given to the organic matter
present in WW, as it is found to hinder the inactivation process but other benefits, such as iron
complexation, also occur.
3) The selected model hospital/industrial contaminants (Iohexol, Venlafaxine) helped elucidate the
pitfalls and opportunities in HWW treatment by AOPs. The AOPs were found to work particularly
well against the concentrated, (simulated) industrial wastewater, hospital flows and urine.
Therefore, their application in hospitals and related industrial activities is promising. Also, the
structural deformation of the selected pollutants provided helpful insights on the operational and
chemical constraints on applying the various AOPs; for instance the use of iron (when H2O2 is
202
present) is strongly recommended for faster and more intense degradation of the contaminants
in HWW. Finally, apart from the degradation point of view, the AOPs studied increased the
biodegradability of the selected compounds treated solutions, which could allow their use as pre-
treatment methods in HWWTPs.
In conclusion, more work is necessary to establish these methods as suitable for application in hospital
environments. However, the initial results strongly support their further development, and future work
stemming from the present research is encouraged to be sought.
To begin with, the combination of three secondary pre-treatment methods with an AOP as a post-
treatment showed great potential in micropollutant elimination and enhanced bacterial disinfection, with
regrowth repression. Although certain combinations (e.g. MBBR+UV/H2O2) were very efficient, the overall
findings indicate great potential for the UV-based methods in developed countries. Some topics that need
to be addresses involve:
- The treatment combinations in pilot- or full-scale.
- Assessment of AOPs in lab- or pilot scale in conjunction with the recent developments in
secondary treatment (SBR, Annamox etc.).
- The optimization of the full-scale treatment for micropollutant removal and microorganism
elimination; Optimization of operational parameters, such as H2O2, UV light lamp types etc.
- Engineering proper reactors for WW treatment by AOPs.
- Techno-economical assessment of the proposed treatment processes.
Nevertheless, in developing countries the thought of WW treatment is at infant stage at most. Therefore,
the focus should be turned towards the improvement of the existing strategies. Almost intuitively, the
populations have developed the lagoons as a means of WW retention and (accidental) treatment, the
photo-Fenton process could offer a barrier towards surface water decontamination. The sunlight and the
inherent iron content of waters provide a good starting point for further exploration of these techniques.
Also, developing simple operating and performance monitoring aspects could be explored.
The study of the photo-Fenton process as a microorganism disinfection technique revealed that under the
eye of hydroxyl radicals, all microbes are the same. From the simple MS2 coliphage, to the “fortified”
yeast model tested, microbial disinfection was eventually achieved. However, the proposed mechanistic
model for both viruses and yeasts, contains many variables that escaped the focus of this work and
demand further investigation. Some propositions are:
- The quantification of ROS production in WW and their contribution towards inactivation.
- The characterization of the kinetic constants throughout the complex mechanisms proposed.
- The contribution of endogenous inactivation, for the different microbial species.
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- Extension towards human pathogens, in real WW (urban and hospital), and achievement of
proper inactivation, through the establishment of an order of removal among the pathogenic
species.
As far as the hospital WW treatment is concerned, setting up a local HWWTP with biological treatment
and AOPs as polishing steps would be ideal. Nevertheless, the primary evidence collected indicated great
potential for the in-situ urine treatment in health facilities. As it appears, dispersion of the chemical
contaminants in HWW and then in UWW collection systems will require higher residence times of
advanced treatment solution for their elimination. On the other hand, focusing on small, concentrated
volumes at hospital level could remove a burden from the downstream treatment. The use of medium-
pressure UV lamps and the photo-Fenton treatment is a potentially powerful process, as shown by the
corresponding low-pressure UV/H2O2/Fe2+ process. A wider list of MPs, and exploration of a portable
reactor for urine treatment could facilitate this treatment process. Also, although urine leaves the kidneys
microorganism-free, microbiological assessment should be conducted, in order to ensure lack of cross-
contaminations, safe recovery and explore potential reuse (e.g. for phosphorus recovery).
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Appendix A: Supplementary material of Chapter 2
1. MP degradation details
Observing the degradation rates of each MP, in combination with the specific pollutant information
of Supplementary Table 2, a detailed explanation is given below.
Diclofenac
This compound has a relative high k value when treated with UV-C, which could not be estimated
because it was eliminated before the sampling interval. It also presented a high degradation constant
when exposed to solar irradiation, indicating its photo-sensitive behavior. It also reacted quickly with
OH• radicals, which is normal because diclofenac has reported the highest apparent second-order rate
constant among the eight selected MPs (1.0 x 1011 M-1.s-1). It showed high degradation rate for Fenton,
and photo-Fenton, except for the WW produced by CF which was very slow, and the delay was related
with the physicochemical characteristics of the WW instead of the pollutant (Klamerth et al. 2010).
The UV/H2O2 process degraded Diclofenac very fast in all three types of WW.
Mecoprop
Together with diclofenac, this compound showed the highest degradation rate when treated with UV-
C irradiation. This is attributed to its chromophores that absorb UV at wavelengths between 280 and
290 nm. During solar irradiation, the degradation rate was high in the AS WW type, while very low for
the MBBR and CF WW types. The higher suspended solid concentrations of these two WW types may
be a reason of solar irradiation low degradation rates. Mecoprop again (De la Cruz et al. 2013) showed
moderate degradation rates which comply with previous apparent second-order rate constants
observed (kOH = 1.0 x 1010 M-1.s-1). The presence of –OH and –OCH3 radicals in its chemical structure
facilitates its degradation (kOH = 97 x 107 M-1.s-1 and 100 x 107 M-1.s-1, respectively).
Metoprolol
This compound showed (after diclofenac) a remarkable degradation rate when treated with UV-C
radiation. Indeed, Metoprolol UV-absorption peak is at 223 nm, very close to 254 nm emission of the
UV-C lamps. It was also well degraded when exposed to solar irradiation, pointing out a general photo-
sensible nature. Again in this case, the degradation rate constant was higher in MBBR than CF WW
type; which might be partly explained by the inexistent potential desorption effect of Metoprolol in
CF (high solubility = 16900 mg/L and low kow = 1.88). On the contrary, this compound degraded
223
moderately fast when exposed to hydroxyl radicals in Fenton and photo-Fenton treatment (Prieto-
Rodríguez et al. 2013) which agrees with the HO rate constant (kOH = 9.6 x 1010 M-1.s-1). UV/H2O2
treatment entailed high (measured) degradation rates of this compound.
Benzotriazole
This compound demonstrated the highest degradation rate constants, compared to the rest of MPs,
when treated with UV-C irradiation. However, it is suggested that this behavior is attributed to the
fact that the initial Benzotriazole concentration was ~50 times higher than the other MPs for all types
of effluents. Degradation rate constants were also high when it was exposed to solar irradiation, which
is expected, given that the UV-absorption peak of this compound is at 465 nm. Only Benzotriazole
contained in CF WW type showed resistance to solar irradiation (k = 0 min-1), probably because of the
high concentration of suspended solids that may have blocked sunlight transmittance. Benzotriazole
showed relatively low degradation rates when exposed to hydroxyl radicals during Fenton and photo-
Fenton treatment, which is consistent with previous HO apparent second-order rate constant
observed (6.0 x 1010 M-1.s-1). The small rate reaction of Benzotriazole with hydroxyl radicals (De la Cruz
et al. 2013) is explained by the presence of –CN compound in its chemical structure (kOH = 2.2 x 107 M-
1.s-1).
Carbamazepine
This compound withholds moderate degradation constants for UV-C and solar irradiation because it
contains chromophores that absorb at wavelengths greater than 290 nm and therefore may be
susceptible to direct photolysis by UV-C and even by sunlight. Only the WW coming from CF showed
insignificant removal after solar irradiation (ksolar = 0 min-1). Moreover, Carbamazepine treated with
Fenton, photo-Fenton and UV/H2O2 also showed moderate degradation rate constants (Klamerth et
al. 2010), which is coherent with the apparent second-rate constant reported in literature (k = 4.9 x
1010 M-1.s-1). Carbamazepine also has a -NH2 compound, which reacts fast with hydroxyl radicals (kOH
= 420 x 107 M-1.s-1). However, further degradation is expected to decelerate due to the formation of a
carboxylic radical (kOH= 1.6 x 107 M-1.s-1). Only carbamazepine contained in the CF WW type showed
very low degradation constants (e.g. kFenton = 0 min-1) when subjected to these treatment methods.
Clarithromycin
This compound showed the lowest degradation rates for UV-C, UV/H2O2, photo-Fenton, solar
irradiation and Fenton reaction. Furthermore, it was the only compound not degraded after 5 minutes
of UV/H2O2 treatment for the AS WW type. This persistent behavior might be attributed to its higher
224
molecular weight (748 g/mol), compared to the other MPs and mainly to its complex chemical
structure which includes several deactivating groups. The degradation pathway of this pollutant
involves a significant number of intermediates prior to mineralization. Previous works reported low k
for Clarithromycin as well (Kim et al. 2009b).
2. Supplementary Figures
Figure S1 – H2O2 consumption during UV/ H2O2 treatment
225
Figure S2 – Dissolved iron content and H2O2 consumption during Fenton treatment
226
Figure S3 – Dissolved iron content and H2O2 consumption during photo-Fenton treatment
227
Figure S4 – Summary of the degradation results, per secondary (pre)treatment method and
advanced (post)treatment process.
0102030405060708090
100
UV - 10' UV - 30' UV/H2O2 - 5' UV/H2O2 - 10' Solar - 30' Solar - 60' Fenton - 60' Fenton - 120' Photo-Fenton -30'
Photo-Fenton -60'
% D
egra
datio
nActivated Sludge
Carbamazepine
Diclofenac
Metoprolol
Clarithromycin
Benzotriazole
Mecoprop
0102030405060708090
100
UV - 10' UV - 30' UV/H2O2 - 5' UV/H2O2 - 10' Solar - 30' Solar - 60' Fenton - 60' Fenton - 120' Photo-Fenton -30'
Photo-Fenton -60'
% D
egra
datio
n
Moving Bed Bioreactor
Carbamazepine
Diclofenac
Metoprolol
Clarithromycin
Benzotriazole
Mecoprop
0102030405060708090
100
UV - 10' UV - 30' UV/H2O2 - 5' UV/H2O2 - 10' Solar - 30' Solar - 60' Fenton - 60' Fenton - 120' Photo-Fenton -30'
Photo-Fenton -60'
% D
egra
datio
n
Coagulation-Flocculation
Carbamazepine
Diclofenac
Metoprolol
Clarithromycin
Benzotriazole
Mecoprop
228
3. Supplementary Tables
Table S1: Micropollutant degradation order, per process and matrix involved.
UV-based all matrices Carbamazepine Clarithromycin Metoprolol Benzotriazole Mecoprop Diclofenac Fenton-related all matrices Clarithromycin Benzotriazole Metoprolol Carbamazepine Mecoprop Diclofenac
UV-based
AS Benzotriazole Carbamazepine Metoprolol Clarithromycin Mecoprop Diclofenac
MBBR Carbamazepine Clarithromycin Metoprolol Benzotriazole Mecoprop Diclofenac
CF Carbamazepine Clarithromycin Metoprolol Benzotriazole Mecoprop Diclofenac
Fenton-related
AS Clarithromycin Benzotriazole Metoprolol Mecoprop Carbamazepine Diclofenac
MBBR Clarithromycin Benzotriazole Metoprolol Carbamazepine Mecoprop Diclofenac
CF Clarithromycin Benzotriazole Metoprolol Carbamazepine Mecoprop Diclofenac
Table S2: Main physical and chemical properties of the eight selected micropollutants (USNLM 2014).
Compound Chemical structure
Molecular
weight
(g/mol)
Water
solubility
(mg/L)
log
kow pka
Henry’s
coefficient
(H)
(atm.m3/mol)
OH•
reaction
rate
constant
(M-1.s-1)
Carbamazepine
C15H12N2O
236.269 18 2.45 13.9 1.1 x 10-10
4.9 x
1010
Diclofenac
C14H11Cl2NO2
296.149 2.4 4.51 4.15 4.7 x 10-12
1.0 x
1011
229
Clarithromycin
C38H69NO13
747.953 1.7 3.16 8.99 - 5 x 109
Metoprolol
C15H25NO3
267.364 16900 1.88 9.68 2.1 x 10-11
9.6 x
1010
Benzotriazole
C6H5N3
119.124 19800 1.44 8.37 3.17 x 10-7 6.0 x 108
Mecoprop
C10H11ClO3
214.646 880 3.13 3.78 3.8 x 10-9
1.0 x
1010
230
Appendix B: Supplementary material of Chapter 3
Supplementary Figure S1 – UV reactor configuration.
231
Supplementary Figure S2 – Absorbance and transmittance spectra of the four effluents. For the
transmittance, samples were analyzed as received, and for the absorbance spectra, filtering through
0.45 μm filter took place beforehand.
232
Table S1 – AOPs used, sampling times and reagents addition for all effluents.
Microorganisms Initial H2O2 Initial Fe2+
[mg/L] [mg/L] UV-C irradiation - -
UV/H2O2 20 -
Solar irradiation - - Fenton 10, 20 2
photo-Fenton 10, 20 2
Micropollutants Initial H2O2 Initial Fe2+
[mg/L] [mg/L] UV-C irradiation - -
UV/H2O2 25 -
Solar irradiation - - Fenton 25 5
photo-Fenton 25 5
233
Table S2 – Synergy (S) among the photo-Fenton constituents for micropollutant degradation in the
treated effluents.
Degradation % per minute Pretreatment Process Activated Sludge Moving Bed BioReactor Coagulation-Flocculation
Fenton process 0.2417 0.3884 0.1550 Solar light 0.2092 0.3076 0.1279
Photo-Fenton 0.6894 0.8516 0.4289
Solar + Fenton 0.4509 0.6960 0.2829
1.5289 1.2236 1.5161
234
Table S3 – Synergy (S) among the solar photo-Fenton constituents in microorganism elimination: first
order reaction kinetics constant.
Kinetics constant (k) Pretreatment
process Primary
Treatment Activated
Sludge Moving Bed BioReactors
Coagulation-Flocculation
Fenton process 0.32 0.45 0.51 0.45
Solar light 0.61 0.76 0.81 0.62 Photo-Fenton 0.95 2.14 2.21 1.09
Solar + Fenton 0.93 1.21 1.32 1.07
1.02 1.77 1.68 1.02
235
Appendix C: Supplementary material of Chapter 4
Figure S1 – Suntest solar simulator light wavelength emission spectrum (Manufacturer: Suntest Xenon
Test-Instruments Brochure)
Figure S2 – (dark) Fenton and solar disinfection experiments. a) Individual effect of the Fenton
reagents (Fe(II), Fe(III) and H2O2). b) Solar wastewater exposure under 300, 600 and 900 W/m2 global
irradiance.
236
Figure S3 - Absorbance spectra of Fe(III) in Mili-Q water or wastewater and iron solubility experiments, 1, 2 or 5 mg/L iron addition in MQ or wastewater (reference: pure MQ).
237
Appendix D: Supplementary material of Chapter 5
Figure S1 – H2O2 evolution during the assays. The different tests are: H2O2 only, light/ H2O2 (hv/H2O2)
and photo-Fenton (pF) with FeSO4 as starting iron salt (FeSO4 pF), with iron citrate (Fe-cit) and
Goethite (Goethite pF). The numbers following indicate the starting pH of the corresponding test.
238
Statistical connection among the cultivability and viability assays
Table S1 summarizes the findings of the Pearson correlation test and the P-Values of the statistical
significance test. As it appears, the three parameters are connected with each other. The CFDA
diminishing is well correlated with the cultivability (0.71 Pearson value) and P<0.05 for the 95% confidence
interval, while PI increase is not well correlated (<0.6) with the cultivability.
Table S1 – Correlation among CFDA or PI staining techniques results and cultivability
CFDA IP
IP -0.855 - Pearson
value
0 - P-value
Cultivability 0.71 -0.512 Pearson
value
0.001 0.03 P-value
This difference is attributed to the intermediate cell states existing, which count as non-cultivable, but do
not repel the propidium ion (yet). Our values are lower than the ones obtained by other authors with TiO2
[27], probably because of the difference in the mode of action, among TiO2 and photo-Fenton. The
contour plot in FigureS2 depicts this correlation among the three assays.
Figure S2 – Contour plot of the correlation among the staining techniques results and the cultivability.
Cultivability (%) vs CFDA (%) and PI (%)Cultivability (%)
PI
CFDA
239
In order to decrease 1-log the cultivability, the readings of CFDA are among 40 and 70%, for all possible PI
values. Consequently, 2-log reduction for CFDA < 40%, 3-log for CFDA < 10% and 50-70% IP and total
inactivation (>4-log) at simultaneous 95% PI and 95% decrease of CFDA.
Figure S3 – Overview of the results of the different staining techniques. a) CFDA staining, indicating
the live cells. b) PI staining, indicating the dead cells.
In Figure S3, there is a consistent trend, where the decrease of esterase activity is slower in simulated
solar light, followed by the hv/H2O2 system. The photo-Fenton systems executed at pH = 7.5 are more
efficient, and finally the pH 6.0 and 5.5 tests are the fastest to disrupt the esterase activity. Conversely, PI
staining appears in the opposite order. The yeast inactivation efficiency is as follows: photo-Fenton (pH<7)
> photo-Fenton (pH=7.5) > hv/H2O2 > hv.
240
Appendix E: Supplementary material of Chapter 6
Supplementary figures
Figure S1 – Experimental installation. UV reactors and related apparatus.
Figure S2 – Indicative chromatogram and peaks of Iohexol TPs during UV/H2O2 treatment.
241
Figure S3 – Absorbance spectra for UV, UV/H2O2 and UV/H2O2/Fe2+ treatment. The UV process is
marked with A, UV/H2O2 with B and for UV/H2O2/Fe2+ with C, in MQ water.
Supplementary Table
Table S1: Detailed information on the CCD for each of the following matrices: WW, diluted WW, UR,
diluted UR.
Factors 3 Run H2O2 Fe2+ pH Levels 2 1 -1 -1 -1
2 1 -1 -1 a 1.68179 3 -1 1 -1
Base runs 20 4 1 1 -1 Replicates 2 5 -1 -1 1 Total Runs 40 6 1 -1 1
7 -1 1 1 Cube points 8 8 1 1 1
Center points 6 9 -1.68179 0 0 Axial points 6 10 1.681793 0 0
11 0 -1.68179 0 Levels -1 1 12 0 1.681793 0 H2O2 20 50 ppm 13 0 0 -1.68179 Fe2+ 10 20 ppm 14 0 0 1.681793 pH 3 5 15 0 0 0
16 0 0 0 Response k min-1 17 0 0 0
18 0 0 0 19 0 0 0 20 0 0 0
242
Statistical analyses nomenclature and abbreviations
DF: Degrees of Freedom
Seq SS: Sequential Sum of Squares
Adj SS: Adjusted Sum of Squares
Adj MS: Adjusted Mean of Squares
F-Value: Ratio of Mean Squares
P-Value: Hypothesis test value
S: Standard Error
R2: Coefficient of Determination
R2 (adj): Adjusted Coefficient of Determination
PRESS: Prediction Sum of Squares
R2 (pred): Predicted Coefficient of Determination
243
1. Statistical Analysis: Models and ANOVA tables for each model
1.1. ANOVA and Model Summary for (Undiluted) WW models
Linear:
Table S1.1.1. Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 0.087581 38.44% 0.087581 0.021895 5.15 0.002
Linear 4 0.087581 38.44% 0.087581 0.021895 5.15 0.002
[I] 1 0.086400 37.92% 0.057602 0.057602 13.55 0.001
[H2O2] 1 0.000773 0.34% 0.000602 0.000602 0.14 0.709
[Fe] 1 0.000034 0.01% 0.000022 0.000022 0.01 0.943
pH 1 0.000374 0.16% 0.000374 0.000374 0.09 0.769
Error 33 0.140245 61.56% 0.140245 0.004250
Total 37 0.227826 100.00%
Table S1.1.2. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0651909 38.44% 30.98% 0.163796 28.10%
Linear with Squares:
Table S1.1.3. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 8 0.210459 92.38% 0.210459 0.026307 43.93 <0.001
Linear 4 0.087581 38.44% 0.200111 0.050028 83.54 <0.001
[I] 1 0.086400 37.92% 0.166283 0.166283 277.66 <0.001
[H2O2] 1 0.000773 0.34% 0.000468 0.000468 0.78 0.384
[Fe] 1 0.000034 0.01% 0.000043 0.000043 0.07 0.790
pH 1 0.000374 0.16% 0.001882 0.001882 3.14 0.087
244
Square 4 0.122878 53.94% 0.122878 0.030720 51.30 <0.001
[I] x [I] 1 0.115482 50.69% 0.109366 0.109366 182.62 <0.001
[H2O2] x [H2O2] 1 0.004193 1.84% 0.003042 0.003042 5.08 0.032
[Fe] x [Fe] 1 0.003198 1.40% 0.003157 0.003157 5.27 0.029
pH x pH 1 0.000006 0.00% 0.000006 0.000006 0.01 0.922
Error 29 0.017367 7.62% 0.017367 0.000599
Total 37 0.227826 100.00%
Table S1.1.4. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0244717 92.38% 90.27% 0.0494703 78.29%
Quadratic Model:
Table S1.1.5. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 14 0.213923 93.90% 0.213923 0.015280 25.28 <0.001
Linear 4 0.087581 38.44% 0.092411 0.023103 38.22 <0.001
[I] 1 0.086400 37.92% 0.008808 0.008808 14.57 0.001
[H2O2] 1 0.000773 0.34% 0.002171 0.002171 3.59 0.071
[Fe] 1 0.000034 0.01% 0.000093 0.000093 0.15 0.699
pH 1 0.000374 0.16% 0.000111 0.000111 0.18 0.673
Square 4 0.122878 53.94% 0.123821 0.030955 51.21 <0.001
[I] x [I] 1 0.115482 50.69% 0.104702 0.104702 173.21 <0.001
[H2O2] x [H2O2] 1 0.004193 1.84% 0.000068 0.000068 0.11 0.741
[Fe] x [Fe] 1 0.003198 1.40% 0.000738 0.000738 1.22 0.281
pH x pH 1 0.000006 0.00% 0.000025 0.000025 0.04 0.842
2-Way Interaction
6 0.003464 1.52% 0.003464 0.000577 0.95 0.477
[I] x [H2O2] 1 0.002745 1.20% 0.001254 0.001254 2.07 0.163
[I] x [Fe] 1 0.000231 0.10% 0.000248 0.000248 0.41 0.529
245
[I] x pH 1 0.000034 0.01% 0.000004 0.000004 0.01 0.933
[H2O2] x [Fe] 1 0.000398 0.17% 0.000412 0.000412 0.68 0.417
[H2O2] x pH 1 0.000038 0.02% 0.000034 0.000034 0.06 0.814
[Fe] x pH 1 0.000018 0.01% 0.000018 0.000018 0.03 0.865
Error 23 0.013903 6.10% 0.013903 0.000604
Total 37 0.227826 100.00%
Table S1.1.6. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0245865 93.90% 90.18% * *
Multiplicative model:
Table S1.1.7. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 9.03575 96.62% 9.03575 2.25894 242.94 <0.001
Linear 4 9.03575 96.62% 9.03575 2.25894 242.94 <0.001
log[I] 1 8.55057 91.43% 8.43966 8.43966 907.65 <0.001
log[H2O2] 1 0.07906 0.85% 0.02190 0.02190 2.35 0.134
log[Fe] 1 0.34392 3.68% 0.10067 0.10067 10.83 0.002
log[H+] 1 0.06220 0.67% 0.06220 0.06220 6.69 0.014
Error 34 0.31614 3.38% 0.31614 0.00930
Total 38 9.35189 100.00%
Table S1.1.8. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0964280 96.62% 96.22% 0.454375 95.14%
246
1.2. ANOVA and Model Summary for Diluted WW models
Linear:
Table S1.2.1. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 0.192009 61.38% 0.192009 0.048002 7.15 0.001
Linear 4 0.192009 61.38% 0.192009 0.048002 7.15 0.001
[I] 1 0.186773 59.71% 0.136364 0.136364 20.32 <0.001
[H2O2] 1 0.000720 0.23% 0.003609 0.003609 0.54 0.473
[Fe] 1 0.004511 1.44% 0.002598 0.002598 0.39 0.542
pH 1 0.000004 0.00% 0.000004 0.000004 0.00 0.980
Error 18 0.120790 38.62% 0.120790 0.006711
Total 22 0.312798 100.00%
Table S1.2.2. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0819179 61.38% 52.80% 0.181728 41.90%
Linear with Squares:
Table S1.2.3. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 8 0.289349 92.50% 0.289349 0.036169 21.59 <0.001
Linear 4 0.192009 61.38% 0.262954 0.065738 39.25 <0.001
[I] 1 0.186773 59.71% 0.223651 0.223651 133.53 <0.001
[H2O2] 1 0.000720 0.23% 0.000342 0.000342 0.20 0.658
[Fe] 1 0.004511 1.44% 0.000503 0.000503 0.30 0.592
pH 1 0.000004 0.00% 0.004705 0.004705 2.81 0.116
Square 4 0.097341 31.12% 0.097341 0.024335 14.53 <0.001
[I] x [I] 1 0.093373 29.85% 0.068851 0.068851 41.11 <0.001
247
[H2O2] x [H2O2] 1 0.000512 0.16% 0.000418 0.000418 0.25 0.625
[Fe] x [Fe] 1 0.000584 0.19% 0.000049 0.000049 0.03 0.867
pH x pH 1 0.002872 0.92% 0.002872 0.002872 1.71 0.211
Error 14 0.023449 7.50% 0.023449 0.001675
Total
Table S1.2.4. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0409260 92.50% 88.22% 0.0775774 75.20%
Quadratic Model:
Table S1.2.5. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 14 0.299548 95.76% 0.299548 0.021396 12.92 0.001
Linear 4 0.192009 61.38% 0.089026 0.022256 13.44 0.001
[I] 1 0.186773 59.71% 0.009570 0.009570 5.78 0.043
[H2O2] 1 0.000720 0.23% 0.000914 0.000914 0.55 0.479
[Fe] 1 0.004511 1.44% 0.000406 0.000406 0.24 0.634
pH 1 0.000004 0.00% 0.000408 0.000408 0.25 0.633
Square 4 0.097341 31.12% 0.078487 0.019622 11.85 0.002
[I] x [I] 1 0.093373 29.85% 0.076154 0.076154 45.98 <0.001
[H2O2] x [H2O2] 1 0.000512 0.16% 0.000561 0.000561 0.34 0.577
[Fe] x [Fe] 1 0.000584 0.19% 0.000115 0.000115 0.07 0.799
pH x pH 1 0.002872 0.92% 0.000758 0.000758 0.46 0.518
2-Way Interaction
6 0.010199 3.26% 0.010199 0.001700 1.03 0.472
[I] x [H2O2] 1 0.003070 0.98% 0.001021 0.001021 0.62 0.455
[I] x [Fe] 1 0.005907 1.89% 0.000070 0.000070 0.04 0.842
[I] x pH 1 0.000438 0.14% 0.000395 0.000395 0.24 0.639
[H2O2] x [Fe] 1 0.000697 0.22% 0.000436 0.000436 0.26 0.622
248
[H2O2] x pH 1 0.000002 0.00% 0.000076 0.000076 0.05 0.836
[Fe] x pH 1 0.000086 0.03% 0.000086 0.000086 0.05 0.826
Error 8 0.013250 4.24% 0.013250 0.001656
Total 22 0.312798 100.00%
Table S1.2.6. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0406972 95.76% 88.35% 107.505 0.00%
Multiplicative model:
Table S1.2.7. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 6.56526 92.24% 6.56526 1.64132 56.47 <0.001
Linear 4 6.56526 92.24% 6.56526 1.64132 56.47 <0.001
log[I] 1 5.89394 82.81% 4.87605 4.87605 167.77 <0.001
log[H2O2] 1 0.06083 0.85% 0.00026 0.00026 0.01 0.926
log[Fe] 1 0.34575 4.86% 0.01315 0.01315 0.45 0.509
log[H+] 1 0.26473 3.72% 0.26473 0.26473 9.11 0.007
Error 19 0.55222 7.76% 0.55222 0.02906
Total 23 7.11748 100.00%
Table S1.2.8. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.170482 92.24% 90.61% 0.985649 86.15%
249
1.3. Correlation among diluted and undiluted WW
Linear:
logK_dil = 0.1730 + 0.9879 logK_undil
S = 0.0823160 R2 = 97.7% R2 (adj) = 97.6%
Table S1.3.1. - Analysis of Variance
Source DF SS MS F P
Regression 1 5.57677 5.57677 823.03 0.000
Error 19 0.12874 0.00678
Total 20 5.70551
250
1.4. ANOVA and Model Summary for (undiluted) UR models
Linear:
Table S1.4.1. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 0.021003 63.78% 0.021003 0.005251 14.97 <0.001
Linear 4 0.021003 63.78% 0.021003 0.005251 14.97 <0.001
[I] 1 0.006919 21.01% 0.002533 0.002533 7.22 0.011
[H2O2] 1 0.000356 1.08% 0.000280 0.000280 0.80 0.378
[Fe] 1 0.006179 18.76% 0.000229 0.000229 0.65 0.425
pH 1 0.007550 22.93% 0.007550 0.007550 21.52 0.000
Error 34 0.011928 36.22% 0.011928 0.000351
Total 38 0.032931 100.00%
Table S1.4.2. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0187304 63.78% 59.52% 0.0164007 50.20%
Linear with Squares:
Table S1.4.3. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 8 0.026208 79.59% 0.026208 0.003276 14.62 <0.001
Linear 4 0.021003 63.78% 0.008111 0.002028 9.05 <0.001
[I] 1 0.006919 21.01% 0.001088 0.001088 4.85 0.035
[H2O2] 1 0.000356 1.08% 0.000005 0.000005 0.02 0.878
[Fe] 1 0.006179 18.76% 0.000003 0.000003 0.01 0.906
pH 1 0.007550 22.93% 0.006649 0.006649 29.67 <0.001
Square 4 0.005206 15.81% 0.005206 0.001301 5.81 0.001
[I] x [I] 1 0.000045 0.14% 0.000232 0.000232 1.03 0.317
251
[H2O2] x [H2O2] 1 0.000166 0.51% 0.000551 0.000551 2.46 0.127
[Fe] x [Fe] 1 0.002209 6.71% 0.003093 0.003093 13.80 0.001
pH x pH 1 0.002785 8.46% 0.002785 0.002785 12.43 0.001
Error 30 0.006723 20.41% 0.006723 0.000224
Total 38 0.032931 100.00%
Table S1.4.4. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0149695 79.59% 74.14% 0.0113284 65.60%
Quadratic model:
Table S1.4.5. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 14 0.031552 95.81% 0.031552 0.002254 39.25 <0.001
Linear 4 0.021003 63.78% 0.001325 0.000331 5.77 0.002
[I] 1 0.006919 21.01% 0.000328 0.000328 5.71 0.025
[H2O2] 1 0.000356 1.08% 0.000031 0.000031 0.54 0.472
[Fe] 1 0.006179 18.76% 0.000011 0.000011 0.18 0.672
pH 1 0.007550 22.93% 0.000937 0.000937 16.31 <0.001
Square 4 0.005206 15.81% 0.000972 0.000243 4.23 0.010
[I] x [I] 1 0.000045 0.14% 0.000004 0.000004 0.07 0.790
[H2O2] x [H2O2] 1 0.000166 0.51% 0.000043 0.000043 0.75 0.394
[Fe] x [Fe] 1 0.002209 6.71% 0.000914 0.000914 15.92 0.001
pH x pH 1 0.002785 8.46% 0.000052 0.000052 0.90 0.353
2-Way Interaction
6 0.005344 16.23% 0.005344 0.000891 15.51 <0.001
[I] x [H2O2] 1 0.000098 0.30% 0.000013 0.000013 0.22 0.640
[I] x [Fe] 1 0.001262 3.83% 0.000262 0.000262 4.57 0.043
[I] x pH 1 0.001757 5.34% 0.002120 0.002120 36.91 <0.001
[H2O2] x [Fe] 1 0.000458 1.39% 0.000801 0.000801 13.95 0.001
252
[H2O2] x pH 1 0.000014 0.04% 0.001577 0.001577 27.46 <0.001
[Fe] x pH 1 0.001754 5.33% 0.001754 0.001754 30.55 <0.001
Error 24 0.001378 4.19% 0.001378 0.000057
Total 38 0.032931 100.00%
Table S1.4.6. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0075780 95.81% 93.37% 0.0047446 85.59%
Multiplicative model:
Table S1.4.7. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 5.04941 83.42% 5.04941 1.26235 41.50 <0.001
Linear 4 5.04941 83.42% 5.04941 1.26235 41.50 <0.001
log[I] 1 1.16137 19.19% 1.40367 1.40367 46.15 <0.001
log[H2O2] 1 0.07470 1.23% 0.00149 0.00149 0.05 0.826
log[Fe] 1 2.57934 42.61% 0.42109 0.42109 13.84 0.001
log[H+] 1 1.23400 20.39% 1.23400 1.23400 40.57 <0.001
Error 33 1.00373 16.58% 1.00373 0.03042
Total 37 6.05314 100.00%
Table S1.4.8. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.174402 83.42% 81.41% 1.39151 77.01%
253
1.5. ANOVA and Model Summary for diluted UR models
Linear:
Table S1.5.1. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 0.033269 76.14% 0.033269 0.008317 11.97 <0.001
Linear 4 0.033269 76.14% 0.033269 0.008317 11.97 <0.001
[I] 1 0.024963 57.13% 0.029512 0.029512 42.46 <0.001
[H2O2] 1 0.005612 12.84% 0.005586 0.005586 8.04 0.013
[Fe] 1 0.002572 5.89% 0.000996 0.000996 1.43 0.250
pH 1 0.000122 0.28% 0.000122 0.000122 0.18 0.681
Error 15 0.010425 23.86% 0.010425 0.000695
Total 19 0.043694 100.00%
Table S1.5.2. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0263631 76.14% 69.78% 0.0422853 3.22%
Linear with Squares:
Table S1.5.3. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 8 0.041546 95.08% 0.041546 0.005193 26.60 <0.001
Linear 4 0.033269 76.14% 0.040179 0.010045 51.44 <0.001
[I] 1 0.024963 57.13% 0.037442 0.037442 191.75 <0.001
[H2O2] 1 0.005612 12.84% 0.001893 0.001893 9.69 0.010
[Fe] 1 0.002572 5.89% 0.000015 0.000015 0.08 0.786
pH 1 0.000122 0.28% 0.000585 0.000585 2.99 0.111
Square 4 0.008277 18.94% 0.008277 0.002069 10.60 0.001
[I] x [I] 1 0.008184 18.73% 0.004800 0.004800 24.58 <0.001
254
[H2O2] x [H2O2] 1 0.000059 0.13% 0.000035 0.000035 0.18 0.679
[Fe] x [Fe] 1 0.000021 0.05% 0.000034 0.000034 0.17 0.686
pH x pH 1 0.000014 0.03% 0.000014 0.000014 0.07 0.794
Error 11 0.002148 4.92% 0.002148 0.000195
Total 19 0.043694 100.00%
Table S1.5.4. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0139739 95.08% 91.51% 0.0263597 39.67%
Quadratic Model:
Table S1.5.5. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 12 0.043335 99.18% 0.043335 0.003611 70.46 <0.001
Linear 4 0.033269 76.14% 0.037618 0.009405 183.49 <0.001
[I] 1 0.024963 57.13% 0.037442 0.037442 730.54 <0.001
[H2O2] 1 0.005612 12.84% 0.000019 0.000019 0.36 0.566
[Fe] 1 0.002572 5.89% 0.000000 0.000000 0.00 0.978
pH 1 0.000122 0.28% 0.000131 0.000131 2.55 0.154
Square 4 0.008277 18.94% 0.003233 0.000808 15.77 0.001
[I] x [I] 1 0.008184 18.73% 0.002854 0.002854 55.68 <0.001
[H2O2] x [H2O2] 1 0.000059 0.13% 0.000006 0.000006 0.12 0.743
[Fe] x [Fe] 1 0.000021 0.05% 0.000040 0.000040 0.78 0.406
pH x pH 1 0.000014 0.03% 0.000003 0.000003 0.05 0.829
2-Way Interaction
4 0.001789 4.09% 0.001789 0.000447 8.73 0.007
[I] x [H2O2] 1 0.001651 3.78% 0.001764 0.001764 34.43 0.001
[H2O2] x [Fe] 1 0.000097 0.22% 0.000002 0.000002 0.03 0.867
[H2O2] x pH 1 0.000036 0.08% 0.000039 0.000039 0.76 0.412
[Fe] x pH 1 0.000005 0.01% 0.000005 0.000005 0.11 0.754
255
Error 7 0.000359 0.82% 0.000359 0.000051
Total 19 0.043694 100.00%
Table S1.5.6. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0071591 99.18% 97.77% 0.592478 0.00%
Multiplicative model:
Table S1.5.7. - Analysis of Variance
Source DF Seq SS Contribution Adj SS Adj MS F-Value P-Value
Model 4 2.01639 95.39% 2.01639 0.50410 82.74 <0.001
Linear 4 2.01639 95.39% 2.01639 0.50410 82.74 <0.001
log[I] 1 1.61151 76.23% 1.61151 1.61151 264.50 <0.001
log[H2O2] 1 0.11925 5.64% 0.01715 0.01715 2.82 0.113
log[Fe] 1 0.26743 12.65% 0.03630 0.03630 5.96 0.027
log[H+] 1 0.01820 0.86% 0.01820 0.01820 2.99 0.103
Error 16 0.09748 4.61% 0.09748 0.00609
Total 20 2.11388 100.00%
Table S1.5.8. - Model Summary
S R2 R2 (adj) PRESS R2 (pred)
0.0780558 95.39% 94.24% 0.305412 85.55%
256
1.6. Correlation among diluted and undiluted UR
Linear:
logK_dil = - 0.2781 + 0.5143 logK_undil
S = 0.249791 R2 = 43.9% R2 (adj) = 41.0%
Table S1.6.1. - Analysis of Variance
Source DF SS MS F P
Regression 1 0.92836 0.928357 14.88 0.001
Error 19 1.18552 0.062396
Total 20 2.11388
Quadratic:
logK_dil = - 3.092 - 3.217 logK_undil - 1.149 (logK_undil)2
S = 0.148008 R2 = 81.3% R2 (adj)= 79.3%
Table S1.6.2. - Analysis of Variance
Source DF SS MS F P
Regression 2 1.71956 0.859781 39.25 0.000
Error 18 0.39431 0.021906
Total 20 2.11388
Cubic:
logK_dil = 4.436 + 11.52 logK_undil + 8.025 (logK_undil)2 + 1.821 (logK_undil)3
S = 0.108540 R2 = 90.5% R2 (adj) = 88.9%
Table S1.6.3. - Analysis of Variance
Source DF SS MS F P
257
Regression 3 1.91360 0.637867 54.14 0.000
Error 17 0.20028 0.011781
Total 20 2.11388
258
2. MS supplementary material: List of identified products
Table S2.1. Mass spectrum characteristics of Iohexol products identified in degradation studies after 5 min
No Product Treatment Formula m/z experimental m/z theoretical ppma DBEb
1 P1 UV C19H27I2N3O10 711.9888 711.9859 4.07 6.5
2 P2 UV C19H25I2N3O11 709.9695 709.9702 0.99 7.5
3 P3 UV C14H18I3N3O6 705.8411 705.8402 1.28 5.5
4 P4 UV C18H21I2N3O9 677.9464 677.9440 3.54 8.5
5 P5 UV C18H21I2N3O10 675.9652 675.9647 0.74 8.5
6 AC1 UV C16H21I2N3O7 621.9553 621.9542 1.77 6.5
7 P6 UV C19H28IN3O11 602.0859 602.0841 2.99 6.5
8 P7 UV C14H19I2N3O6 579.9445 579.9436 1.55 5.5
1 P1 UV/H2O2 C19H27I2N3O10 711.9888 711.9859 4.07 6.5
2 P2 UV/H2O2 C19H25I2N3O11 709.9695 709.9702 0.99 7.5
3 P3 UV/H2O2 C14H18I3N3O6 705.8411 705.8402 1.28 5.5
4 BC1 UV/H2O2 C19H25I2N3O9 693.9762 693.9753 0.90 7.5
5 BC2 UV/H2O2 C18H23I2N3O9 679.9585 679.9596 0.90 7.5
6 P4 UV/H2O2 C18H21I2N3O9 677.9464 677.9440 3.54 8.5
7 P5 UV/H2O2 C18H21I2N3O10 675.9652 675.9647 0.74 8.5
8 P6 UV/H2O2 C19H28IN3O11 602.0859 602.0841 2.99 6.5
9 B1 UV/H2O2 C19H26IN3O11 600.0715 600.0684 5.17 13
10 P7 UV/H2O2 C14H19I2N3O6 579.9445 579.9436 1.55 5.5
11 B2 UV/H2O2 C18H24IN3O9 554.0636 554.063 1.08 7.5
12 B3 UV/H2O2 C19H27N3O11 474.1726 474.1718 1.69 7.5
13 B4 UV/H2O2 C18H25N3O10 444.1617 444.1613 0.90 7.5
1 C1 UV/Fenton C16H20I3N3O7 747.8510 747.8508 0.27 6.5
2 C2 UV/Fenton C19H26I2N3O11 725.9645 725.9651 0.83 7.5
3 P1 UV/Fenton C19H27I2N3O10 711.9888 711.9859 4.07 6.5
4 P2 UV/Fenton C19H25I2N3O11 709.9695 709.9702 0.99 7.5
5 P3 UV/Fenton C14H18I3N3O6 705.8411 705.8402 1.28 5.5
6 BC1 UV/Fenton C19H25I2N3O9 693.9762 693.9753 0.90 7.5
7 BC2 UV/Fenton C18H23I2N3O9 679.9585 679.9596 0.90 7.5
8 P4 UV/Fenton C18H21I2N3O9 677.9464 677.9440 3.54 8.5
9 P5 UV/Fenton C18H21I2N3O10 675.9652 675.9647 0.74 8.5
10 C3 UV/Fenton C16H21I2N3O8 637.9501 637.9491 1.57 6.5
11 AC1 UV/Fenton C16H21I2N3O7 621.9553 621.9542 1.77 6.5
12 P6 UV/Fenton C19H28IN3O11 602.0859 602.0841 2.99 6.5
259
13 P7 UV/Fenton C14H19I2N3O6 579.9445 579.9436 1.55 5.5
14 C4 UV/Fenton C14H21IN2O7 456.0416 456.0388 6.14 5
15 C5 UV/Fenton C11H14IN3O8 442.9820 442.982 0.90 6
16 C6 UV/Fenton C17H23N3O9 414.1519 414.1507 0.90 7.5
Table S2.2. Mass spectrum characteristics of Iohexol products identified in degradation studies after 15 min
No Product Treatment Formula m/z experimental m/z theoretical ppma DBEb
1 1 UV C19H27I2N3O10 711.9888 711.9859 4.07 6.5
2 2 UV C19H25I2N3O11 709.9695 709.9702 0.99 7.5
3 3 UV C19H23I2N3O12 707.9576 707.9546 4.24 8.5
4 4 UV C14H18I3N3O6 705.8411 705.8402 1.28 5.5
5 5 UV C19H25I2N3O9 693.9762 693.9753 1.30 7.5
6 6 UV C18H21I2N3O9 677.9464 677.9440 3.54 8.5
7 7 UV C17H25I2N3O9 669.9750 669.9753 0.45 5.5
8 8 UV C17H23I2N3O8 651.9648 651.9647 0.15 6.5
9 9 UV C16H21I2N3O7 621.9553 621.9542 1.77 6.5
10 10 UV C19H28IN3O11 602.0859 602.0841 2.99 6.5
11 11 UV C14H19I2N3O6 579.9445 579.9436 1.55 5.5
12 12 UV C18H24IN3O9 554.0636 554.063 1.08 7.5
13 13 UV C19H27N3O11 474.1726 474.1718 1.69 7.5
14 14 UV C19H25N3O10 456.1614 456.1613 0.22 8.5
15 15 UV C14H20IN3O6 454.0473 454.047 0.66 5.5
16 16 UV C18H25N3O10 444.1617 444.1613 0.90 7.5
1 17 UV/H2O2 C19H16IN3O15 652.9575 652.9621 7.04 13
2 18 UV/H2O2 C18H16IN3O16 640.9571 640.9621 7.80 12
3 20 UV/H2O2 C13H14IN3O11 514.9654 514.9667 2.52 8
1 21 UV/Fenton C17H24I3N3O8 779.8792 779.8770 0.90 5.5
2 22 UV/Fenton C14H18I3N3O7 721.8367 721.8352 0.90 5.5
3 4 UV/Fenton C14H18I3N3O6 705.8411 705.8402 0.90 5.5
4 23 UV/Fenton C19H25I2N3O9 693.9762 693.9753 0.90 7.5
5 9 UV/Fenton C16H21I2N3O7 621.9553 621.9542 0.90 6.5
6 10 UV/Fenton C19H28IN3O11 602.0859 602.0841 0.90 6.5
7 24 UV/Fenton C14H19I2N3O7 595.9375 595.9385 0.90 5.5
8 11 UV/Fenton C14H19I2N3O6 579.9445 579.9436 0.90 5.5
9 25 UV/Fenton C11H14IN3O8 442.9820 442.982 0.90 6
260
10 26 UV/Fenton C17H23N3O9 414.1519 414.1507 0.90 7.5
11 27 UV/Fenton C13H16N2O11 377.0846 377.0827 0.90 6.5
appm - Mass Accuracy in ppm bDBE - Double Bond Equivalent A – Exclusive products from UV treatment B – Exclusive products from UV/H2O2 treatment C – Exclusive products from UV/Fenton treatment P - Products common for all three treatment methods AC - Products common for UV (A) and UV/Fenton (C) treatment BC - Products common for UV/H2O2 (B) and UV/Fenton (C) treatment
261
Appendix F: Supplementary material of Chapter 7
Figure S1 – Summary of the UV-C photolysis experiments for the two different energy output systems.
Absorbance spectra changes during the UV exposure.
225 250 275 300 325 350 375 4000.0
0.5
1.0
1.5
2.0
2.5
3.0
Abs
orba
nce
(a.u
.)
Wavelength (nm)
0' 15' 30' 60' 120' 180' 240'
Absorbance spectra during UV treatment
262
Figure S2 – UV/H2O2 Advanced Oxidation of Venlafaxine: global analyses. a) COD removal, TOC
reduction (red traces and axis) and H2O2 consumption (blue trace and axis) with addition of 50 mg/L
H2O2. b) Absorbance changes during UV/H2O2 treatment (50 mg/L H2O2).
0 30 60 90 120 150 180 210 240
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
COD TOC H2O2
Time (min)
CO
D/C
OD
0 & T
OC
/TO
C0
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
(H2O
2)/(H
2O2) 0
11 W
225 250 275 300 325 350 375 4000.0
0.5
1.0
1.5
2.0
2.5
3.0
50 ppm H2O2
Abs
orba
nce
(a.u
.)
Wavelength (nm)
0' 11' 30' 60' 90' 120' 150' 180'
Absorbance spectraduring UV/H2O2 treatment
11 W
263
264
Figure S3 – Treatment of Venlafaxine by the Fenton process in the dark. a) VFA degradation at pH=3 and varied Fe|H2O2 ratio. b) VFA degradation at pH=5 and varied Fe|H2O2 ratio. c) VFA degradation
at pH=7 and varied Fe|H2O2 ratio
265
Figure S4 – Treatment of Venlafaxine by the Fenton process in the dark. a) COD reduction by the Fenton process in by the various Fe|H2O2 ratios at pH=3 and increasing pH for 20|50 ratio. b) TOC
removal by the Fenton process in by the various Fe|H2O2 ratios at pH=3 and increasing pH for 20|50 ratio.
266
267
Figure S5 - Treatment of Venlafaxine by the photo-Fenton process (irradiance: 900 W/m2). a) VFA
degradation at pH=3 and varied Fe|H2O2 ratio. b) VFA degradation at pH=5 and varied Fe|H2O2 ratio.
c) VFA degradation at pH=7 and varied Fe|H2O2 ratio.
268
Figure S6 - Treatment of Venlafaxine by the photo-Fenton process (irradiance: 900 W/m2). a) COD
reduction by the photo-Fenton process by the various Fe|H2O2 ratios at pH=3 and increasing pH for
20|50 ratio. b) TOC removal by the photo-Fenton process by the various Fe|H2O2 ratios at pH=3 and
increasing pH for 20|50 ratio.
269
Supplementary Tables
Table S1 – H2O2 evolution during the Fenton and photo-Fenton experiments in MQ water
Fenton photo-Fenton pH= 3 pH= 3
Sample ID
initial [H2O2]
H2O2 consumption in 24 hours [ppm]
Sample ID
initial [H2O2]
H2O2 consumption during the experiment [ppm]
5|10 10 4.83 5|10 10 5.32 5|50 50 40.74 5|50 50 48.15
20|50 50 28.34 20|50 50 37.27 12.5|5
8.3 58.3 48.3 12.5|58.3 58.3 54.13
12.5|30 30 23.62 12.5|3
0 30 23.24
pH= 5 pH= 5
Sample ID [H2O2]
H2O2 consumption in 24 hours [ppm]
Sample ID [H2O2]
H2O2 consumption during the experiment [ppm]
5|10 10 1.28 5|10 10 6.5 5|50 50 15.11 5|50 50 45.25
20|50 50 21.27 20|50 50 39.97 12.5|5
8.3 58.3 26.24 12.5|58.3 58.3 49.26
12.5|30 30 6.44 12.5|3
0 30 20.79
pH= 7 pH= 7
Sample ID [H2O2]
H2O2 consumption in 24 hours [ppm]
Sample ID [H2O2]
H2O2 consumption during the experiment [ppm]
5|10 10 0.39408867 5|10 10 6.3 5|50 50 11.5 5|50 50 33.9
20|50 50 14.02 20|50 50 26.3 12.5|5
8.3 58.3 17.94 12.5|58.3 58.3 35.55
12.5|30 30 4.14 12.5|3
0 30 20.9
270
Table S2 – Basic physicochemical characteristics of the used effluents in the study.
Parameter Unit Wastewater previously treated with Activated Moving Bed Coagulation
Sludge Bioreactor Flocculation pH - 7.3-7.8 6.6-7.4 7.3-7.9
TOC mg/L 28.08±12.62 14.615±7.9 68.47±15.94 COD mg/L 51±10 20±11 85±5
Alkalinity mg CaCO3/L 230±35 95±10 240±10 TSS mg/L 12.1±2.8 14.2±1.4 28.5±5.7
Total iron mg Fe/L 0.95±0.05 1.75±0.15 5.5±1
271
Table S3 – Basic average physicochemical characteristics of the used urine in the study.
Parameter Value unit
TDS 60 g/L
pH 6.5
COD 8.3 g/L
TOC 5 g/L
272
Table S4 - Mass spectrum characteristics of Venlafaxine's products identified in degradation studies
No Product Treatment Formula m/z experimental m/z theoretical ppma DBEb
1 P6 Solar C17H25NO 260.2016 260.2009 2.69 5.5
1 P3 UV C11H15NO2 194.1179 194.1175 2.06 4.5
2 P5 UV C12H20O4 229.1429 229.1434 2.18 2.5
3 P6 UV C17H25NO 260.2012 260.2009 1.15 5.5
4 P8 UV C17H27NO3 294.2057 294.2064 2.38 4.5
5 P9 UV C17H27NO4 310.2021 310.2013 2.58 4.5
6 P10 UV C17H27NO5 326.1956 326.1962 1.84 4.5
1 P1 UV/H2O2 C8H8O 121.0652 121.0648 3.30 4.5
2 P4 UV/H2O2 C15H18O 215.1431 215.1430 0.46 6.5
3 P6 UV/H2O2 C17H25NO 260.2017 260.2009 3.07 5.5
4 P8 UV/H2O2 C17H27NO3 294.2072 294.2064 2.72 4.5
5 P9 UV/H2O2 C17H27NO4 310.202 310.2013 2.26 4.5
1 P1 Fenton C8H8O 121.0653 121.0648 4.13 4.5
2 P2 Fenton C11H15NO 178.1231 178.1226 2.81 4.5
3 P3 Fenton C11H15NO2 194.1181 194.1175 3.09 4.5
4 P4 Fenton C15H18O 215.1433 215.1430 1.39 6.5
5 P6 Fenton C17H25NO 260.2017 260.2009 3.07 5.5
6 P7 Fenton C17H25NO3 292.1914 292.1907 2.40 5.5
7 P8 Fenton C17H27NO3 294.2070 294.2064 2.04 4.5
1 P1 Photo-Fenton C8H8O 121.0654 121.0648 4.96 4.5
2 P2 Photo-Fenton C11H15NO 178.1231 178.1226 2.81 4.5
3 P3 Photo-Fenton C11H15NO2 194.1182 194.1175 3.61 4.5
4 P4 Photo-Fenton C15H18O 215.1434 215.1430 1.86 6.5
5 P6 Photo-Fenton C17H25NO 260.2018 260.2009 3.46 5.5
6 P8 Photo-Fenton C17H27NO3 294.2071 294.2064 2.38 4.5
7 P9 Photo-Fenton C17H27NO4 310.2017 310.2013 1.29 4.5
appm - mass accuracy in ppm bDBE - Double Bond Equivalent
273
Curriculum Vitae of the Candidate
Stefanos GIANNAKIS
Address: Av. Ed. Dapples 12 CH-1006, Lausanne Switzerland Tel: +41787690465 Email: [email protected] Web: https://www.researchgate.net/profile/Stefanos_Giannakis
EDUCATION
2009-2010 M.Sc. Environmental Protection and Sustainable development Aristotle University of Thessaloniki, Greece School of Engineering, Department of Civil Engineering Grade: 9.15, Excellent (top 3% for academic year 2010-2011) Thesis Grade 9.95/10
2003-2009 Diploma (M.Sc. Equivalent) Aristotle University of Thessaloniki, Greece School of Engineering, Department of Civil Engineering Double major: Civil Engineering, Hydraulics and Environmental Engineering Grade: 7.26, Very good Thesis Grade 10/10
AWARDS AND SCHOLARSHIPS
2012-2013 “Swiss Government Excellence Scholarships” Type: Research Fellowship Place: École Polytechnique Fédérale de Lausanne (EPFL), Switzerland Department: Institute of Chemical Sciences and Engineering Research Domain: Environmental Engineering
2011-2012 “Mediterranean Office for Youth – Mobility Grant” Type: Research Fellowship Place: Universitat Politècnica de Catalunya (UPC), Catalonia, Spain Department: Institut d'Investigació Tèxtil i Cooperació Industrial de Terrassa (INTEXTER) Research Domain: Environmental Engineering
RESEARCH AND TEACHING EXPERIENCE
Teaching
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2015-2016 Chemical Technology and Biology of the Environment, EPFL Teaching Assistant Professors: Cesar Pulgarin
2014-2015 Chemical Technology and Biology of the Environment, EPFL Teaching Assistant Professors: Christos Comninellis, Cesar Pulgarin
2014-2015 Chemical engineering lab & project, EPFL Laboratory Assistant Professors: Liubov Kiwi, Kevin Sivula, Jeremy Luterbacher
2013-2014 Chemical engineering lab & project, EPFL Laboratory Assistant Professors: Liubov Kiwi
2010-2011 Environmental Chemistry, AUTh Laboratory assistant Professors: Darakas Efthymios, Aikaterini Tasoula
2010-2011 Environmental Engineering, AUTh Laboratory assistant Professors: Darakas Efthymios, Aikaterini Tasoula
Student Projects and Theses
Student Year Level Origin/University
Ana Isabel Merino Gamo 2013 MSc Erasmus (University of Barcelona, Spain)
Simon Schindelholz 2014 MSc EPFL, Lausanne, Switzerland
Miquel Pastor Gelabert 2014 MSc Erasmus (University of Barcelona, Spain)
Angelica Varon Lopez 2014 PhD/Trainee University of Cali, Colombia
David Muzard 2014 MSc GPAO, EPFL, Lausanne, Swizerland
Lula Dind 2014 Trainee GPAO, EPFL, Lausanne, Swizerland
Idriss Hendaoui 2014 Trainee GPAO, EPFL, Lausanne, Swizerland
Idriss Hendaoui 2014 MSc GPAO, EPFL, Lausanne, Swizerland
Franco Alejandro Gamarra Vives 2014 MSc EPFL, Lausanne, Switzerland
Barbara Androulaki 2014 Trainee University of Patras, Greece
Margaux Voumard 2014 Project EPFL, Lausanne, Switzerland
Siting Liu 2015 MSc GPAO, EPFL, Lausanne, Swizerland
Siting Liu 2015 Trainee GPAO, EPFL, Lausanne, Swizerland
Samuel Watts 2015 MSc EPFL, Lausanne, Switzerland
Samuel Watts 2015 Trainee GPAO, EPFL, Lausanne, Swizerland
Cristian Pinilla 2015 Trainee GPAO, EPFL, Lausanne, Swizerland
275
Paola Villegas Guzman 2015 PhD/Trainee University of Antioquia, Colombia
Margaux Voumard 2015 MSc EPFL, Lausanne, Switzerland
Margaux Voumard 2016 Trainee GPAO, EPFL, Lausanne, Swizerland
Pilar Valero 2016 PhD/Trainee University of Zaragoza, Spain
Casto Ramos 2016 Trainee EPFL, Lausanne, Switzerland
Cristian Pinilla 2016 MSc Co-supervision (University of Geneva, Switzerland)
Projects
2014-2016 Contributor Member Swiss National Foundation Project (No. 146919) “Treatment of the hospital wastewaters in Côte d'Ivoire and in Colombia by advanced oxidation processes”
2014-2015 Contributor Member Swiss-Hungarian Cooperation Program, No. SH7/2/14 “Towards a sustainable fine chemical and pharmaceutical industry: screening and re-utilisation of carbon-rich liquid wastes”
2013-2014 Contributor Member FP7 LIMPID project (Project No.: 310177) “Nanocomposite materials for photocatalytic degradation of pollutants”
TRAINING COURSES – LIFELONG EDUCATION
2016 COSEC Responsible for Laboratory Safety and Security, GPAO, EPFL
2016 Participant CM1305 ECOSTBio Summer School, Groningen, Netherlands, 8-16 July, 2016
2015 Participant 1st AOPs PhD Summer School, Salerno (Fisciano), Italy, June 15-19, 2015
2015 Participant Swiss Program for Research on Global Issues and Development, Filzbach, Switzerland, 18-20 March, 2015
2015 Participant Teaching Toolkit Workshop, EPFL, 19 May 2015, Lausanne, Switzerland
2014-2015 Participant Introduction to University Teaching, EPFL, completed: 29 June 2015, Lausanne, Switzerland
2013 Participant Mediterranean Office for Youth-Campus France, “Mediterranean Programs Forum”, 20 June 2013, Marseille, France,
2012 Participant 18th European Students Symposium on the Environment “Conservation is not isolation”, 19-26 May 2012, Bratislava, Slovakia
2011 Participant
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17th European Students Symposium on the Environment “Biodiversity and Urbanism”, 20-28 May 2011, Zagreb, Croatia
2011 Participant 4th Summer School "Climate change in cities and city regions – Time to adapt?", 26–30 September 2011, Hamburg, Germany
2011 Participant Full scholarship for participation in the 4th Summer School "Environmental Decision Support Systems (EDSS): A Tool for Wastewater Management in the XXI Century", 3-9 July, Girona, Spain
2011 Participant 2nd Training Course “Water Supply in a Changing Environment”, Aristotle University of Thessaloniki, 11-15/4/2011, Thessaloniki, Greece
PUBLICATIONS
Peer-reviewed Journals
1. Mangayayam, M., Kiwi, J., Giannakis, S., Pulgarin, C., Zivkovic, I., Magrez, A. and Rtimi, S. (2017) FeOx magnetization enhancing E. coli inactivation by orders of magnitude on Ag-TiO2 nanotubes under sunlight. Applied Catalysis B: Environmental 202, 438-445.
2. Giannakis, S., Hendaoui, I., Jovic, M., Grandjean, D., De Alencastro, L.F., Girault, H. and Pulgarin, C. (2017) Solar photo-Fenton and UV/H2O2 processes against the antidepressant Venlafaxine in urban wastewaters and human urine. Intermediates formation and biodegradability assessment. Chemical Engineering Journal 308, 492-504.
3. Giannakis, S., Jovic, M., Gasilova, N., Pastor Gelabert, M., Schindelholz, S., Furbringer, J.M., Girault, H., Pulgarin, C., Iohexol degradation in wastewater and urine by UV-based Advanced Oxidation Processes (AOPs): Process modeling and by-products identification." Journal of Environmental Management (2016), In press, Accepted Manuscript
4. Giannakis, S., Polo López, M.I., Spuhler, D., Sánchez Pérez, J.A., Fernández Ibáñez, P., Pulgarin, C. Solar disinfection is an augmentable, in situ-generated photo-Fenton reaction—Part 1: A review of the mechanisms and the fundamental aspects of the process (2016) Applied Catalysis B: Environmental, 199, pp. 199-223.
5. Giannakis, S., López, M.I.P., Spuhler, D., Pérez, J.A.S., Ibáñez, P.F., Pulgarin, C. Solar disinfection is an augmentable, in situ-generated photo-Fenton reaction-Part 2: A review of the applications for drinking water and wastewater disinfection (2016) Applied Catalysis B: Environmental, 198, pp. 431-446.
6. Giannakis, S., Voumard, M., Grandjean, D., Magnet, A., De Alencastro, L.F., Pulgarin, C. Micropollutant degradation, bacterial inactivation and regrowth risk in wastewater effluents: Influence of the secondary (pre)treatment on the efficiency of Advanced Oxidation Processes (2016) Water Research, 102, pp. 505-515.
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7. Rtimi, S., Giannakis, S., Bensimon, M., Pulgarin, C., Sanjines, R., Kiwi, J. Supported TiO2 films deposited at different energies: Implications of the surface compactness on the catalytic kinetics (2016) Applied Catalysis B: Environmental, 191, pp. 42-52.
8. Giannakis, S., Ruales-Lonfat, C., Rtimi, S., Thabet, S., Cotton, P., Pulgarin, C. Castles fall from inside: Evidence for dominant internal photo-catalytic mechanisms during treatment of Saccharomyces cerevisiae by photo-Fenton at near-neutral pH (2016) Applied Catalysis B: Environmental, 185, pp. 150-162.
9. Rtimi, S., Giannakis, S., Sanjines, R., Pulgarin, C., Bensimon, M., Kiwi, J. Insight on the photocatalytic bacterial inactivation by co-sputtered TiO2-Cu in aerobic and anaerobic conditions (2016) Applied Catalysis B: Environmental, 182, pp. 277-285.
10. Giannakis, S., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Solar disinfection modeling and post-irradiation response of Escherichia coli in wastewater (2015) Chemical Engineering Journal, 281, pp. 588-598.
11. Giannakis, S., Gamarra Vives, F.A., Grandjean, D., Magnet, A., De Alencastro, L.F., Pulgarin, C. Effect of advanced oxidation processes on the micropollutants and the effluent organic matter contained in municipal wastewater previously treated by three different secondary methods (2015) Water Research, 84, pp. 295-306.
12. Giannakis, S., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Temperature-dependent change of light dose effects on E. coli inactivation during simulated solar treatment of secondary effluent (2015) Chemical Engineering Science, 126, pp. 483-487.
13. Giannakis, S., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Environmental considerations on solar disinfection of wastewater and the subsequent bacterial (re)growth (2015) Photochemical and Photobiological Sciences, 14 (3), pp. 618-625.
14. Giannakis, S., Rtimi, S., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Light wavelength-dependent E. coli survival changes after simulated solar disinfection of secondary effluent (2015) Photochemical and Photobiological Sciences, 14 (12), pp. 2238-2250.
15. Giannakis, S., Papoutsakis, S., Darakas, E., Escalas-Cañellas, A., Pétrier, C., Pulgarin, C. Ultrasound enhancement of near-neutral photo-Fenton for effective E. coli inactivation in wastewater (2015) Ultrasonics Sonochemistry, 22, pp. 515-526.
16. Giannakis, S., Merino Gamo, A.I., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Monitoring the post-irradiation E. coli survival patterns in environmental water matrices: Implications in handling solar disinfected wastewater (2014) Chemical Engineering Journal, 253, pp. 366-376.
17. Giannakis, S., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Elucidating bacterial regrowth: Effect of disinfection conditions in dark storage of solar treated secondary effluent (2014) Journal of Photochemistry and Photobiology A: Chemistry, 290 (1), pp. 43-53.
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18. Giannakis, S., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. The antagonistic and synergistic effects of temperature during solar disinfection of synthetic secondary effluent (2014) Journal of Photochemistry and Photobiology A: Chemistry, 280, pp. 14-26.
19. Giannakis, S., Merino Gamo, A.I., Darakas, E., Escalas-Cañellas, A., Pulgarin, C. Impact of different light intermittence regimes on bacteria during simulated solar treatment of secondary effluent: Implications of the inserted dark periods (2013) Solar Energy, 98 (PC), pp. 572-581.
Conferences
1. Near-Neutral Photo-Fenton And The Differentiated Response Of Microbiological And Chemical Contaminants In Wastewater, César Pulgarin, Stefanos Giannakis, SPEA9, 13-17/6, Strasbourg, France (Oral Presentation)
2. Operational And Economical Optimization Of Venlafaxine Treatment By The Photo-Fenton Reaction Through Response Surface Methodology And Desirability Functions, Stefanos Giannakis, Idriss Hendaoui, Jean-Marie Furbringer, César Pulgarin, SPEA9, 13-17/6, Strasbourg, France (Poster Presentation)
3. New insight on the bacterial inactivation by Co-sputtered TiO2-Cu in aerobic and anaerobic media under low intensity actinic light, S. Rtimi, S. Giannakis, C. Pulgarin, J. Kiwi, COST MP1106 Symposium “Smart and Green Interfaces: Fundamentals and Diagnostics (SGI-FunD 2015)”, Sofia, Bulgaria, 29 – 31 October 2015
4. Comparative Evolution Between Oxidation Processes Used For Bacterial Inactivation After Three Different Secondary Treatment Methods, C. Pulgarin, M. Voumard, S. Giannakis – EAAOP4, Athens, October 2015 (Oral presentation)
5. Optimization And Modeling Of Iohexol Treatment By Advanced Oxidation Processes In Environmentally Relevant Matrices, S. Giannakis, M. Pastor Gelabert, S. Schindelholz, J.M. Furbringer, C. Pulgarin – EAAOP4, Athens, October 2015 (Poster Presentation)
6. New Pathways In Heterogeneous And Homogeneous Near-Neutral Photo-Fenton Bacterial Inactivation By Iron Oxides And Iron Citrate Complexes, S. Giannakis, C. Ruales-Lonfat, C. Pulgarin – EAAOP4, Athens, October 2015 (Poster Presentation)
7. Degradación por UV254/H2O2 de contaminantes emergentes en efluentes de PTAR domesticas: desde el laboratorio hasta el piloto final. C. Pulgarin, S. Giannakis, Primer congreso Colombiano de Procesos avanzados de Oxidación, Manizales, Colombia, 21-24 September 2015
8. Emergent chemical and microbiological pollutants related with hospital wastewater in Colombia, Ivory Coast and Switzerland, S. Giannakis, C. Pulgarin. Invited talk. Simposio ACIS 2015: ¿Hasta cuándo tendremos agua en Colombia? September 11th–12th, 2015, Geneva, Switzerland (Oral Presentation)
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9. Internal photo-Fenton leads the solar inactivation of Saccharomyces cerevisiae in hv/H2O2/Fe systems at neutral pH, S. Giannakis, C. Ruales-Lonfat, C. Pulgarin, Swiss Chemical Society Photochemistry Section Annual Meeting 2015, September 8, 2015 - ETH Zurich, Switzerland (Oral Presentation)
10. Environmental Considerations On Solar Disinfection Of Wastewater And The Subsequent Bacterial (Re)growth, S. Giannakis, E. Darakas, A. Escalas-Cañellas, C. Pulgarin, SPEA8, Thessaloniki, Greece, 25-28 June 2014 (Poster presentation)
11. Usage of solar radiation and artificially induced UV irradiation for water and wastewater disinfection, S. Giannakis and E. Darakas, 2012., International Conference on Protection and Restoration of the Environment, PRE XI, Thessaloniki, Greece, July 3-6.
12. Investigation of the environmental impact of Thessaloniki’s main streams on the coastal pollution of Thermaikos Gulf, S. Giannakis and E. Darakas, 2011, 4th Environmental Conference of Macedonia, Thessaloniki, Greece, March 18-20.
13. Statistical analysis of fecal indicator bacteria kinetics based on the initial concentration of the population and the dilution rate, S. Giannakis, E. Darakas and M. Vafeiadis, 2010, 2nd COST 929 Symposium: Future Challenges in food and environmental virology, Istanbul, Turkey, October 7-9.
14. Effects of extreme weather conditions in natural wastewater systems, S. Giannakis and E. Darakas, 2010, 3rd Conference: Small and Decentralized Water and Wastewater Treatment Plants, Skiathos, Greece, May 14-16.
LANGUAGE SKILLS
Language Level (Common European Framework)
Reading Writing Speaking Greek C2 C2 C2
English C2 C2 C2 French Β2 Β2 Β2 Spanish Β2 Β1 Β1 Catalan Α2 Α2 Α2 German Α2 Α1 Α1
SCIENTIFIC COMMITTEE & PROFESSIONAL/ACADEMIC MEMBERSHIPS
AOPs PhD School: Student Representative
Journal Referee: Applied Catalysis B: Environmental, Chemical Engineering Journal, Water Research, Environmental Science and Pollution Research, Water Air and Soil Pollution, Journal of Environmental Management, Process Safety and Environmental Protection, Photochemical and Photobiological Sciences, Journal of Photochemistry and Photobiology A: Chemistry, Desalination and water treatment, Water Science & Technology, RSC Advances