analytical applications of 1, io-anthraquinones: a review
TRANSCRIPT
Talanra, Vol 38, No 6, pp 571-588, 1991 Prmted m Great Brltam All nghts reserved
0039-9 140/9 I $3 00 + 0 00 Pergamon Press plc
ANALYTICAL APPLICATIONS OF 1, IO-ANTHRAQUINONES: A REVIEW
AURORANAVAS DIAZ
Department of Analytlcal Chemistry, Faculty of Saences, Umverslty of MBlaga, 29071-Mblaga, Spam
(Recewed 7 March 1988 Rewed 19 November 1990 Accepted 24 January 1991)
Summary-AnalytIcal aspects of the chemistry m solution of I,lO-anthraqumone (AQ) derlvatlves IS revlewed The mformatlon about photometric and fluonmetnc determmatlon of morgamc species has been condensed and presented m tabular form
Although technological advances m mstrumen- tation have shifted the emphasis of analytical research towards Improvement of methods by means of new and more powerful Instruments or by modification of the Instrumental configur- ation, the prmcrple of chemical analysis still remains chemical reaction between the sub- stance to be determined and an auxiliary sub- stance to be added, the reagent. The extensive but widely dispersed amount of mformation on reaction chemrstry makes a comprehensive and sufficiently critical review of great value for choosmg a reagent for a particular application.
This review deals with anthraqumone (AQ) dertvatlves, a group of reagents widely used m analytical chemistry, but not hitherto surveyed.
The chemistry of anthraqumones has received much attention1-5 because of its relevance to some important technological processes. Anthraqumone derivattves have also been widely used m analytical chemistry, mainly as strong chelatmg agents and chromophores. The major focus of this paper is on their optical properties, which are extensively used in analyti- cal practice, mainly photometry and fluor- tmetry, and m the study of acid-base, redox, complexatton and photochemical reactions. These compounds also display Interesting electrochemical behavtour but its analytical use 1s more limited
The basic chemical structure of anthra- qumones is shown m Fig 1, with the posttion and nomenclature of the substituents. The trade names used by the dyestuff manufacturers can be obtained from the Colour Index6 and the chemical structures and properties can be found m the book by Venkataraman ’
In dyes obtained by chemical synthesis, only substances which have formed during manufac-
ture, together with small amounts of electrolytes obtained during neutralization, will appear In the commercial dyes different types of impurittes may be present 7 Separation of anthraqumone dyes has been dtscussed’ and various chromato- graphic procedures are available for analytt- ca17-12 and preparative scale’3s’4 separations
The properties of anthraqumone and Its de- nvatlves that are of mam interest m analytical chemistry are related to their spectral features Theoretical and experimental studies of the ab- sorption 1s-25 and emtssion25-30 electromc spectra have been reported. The spectral characteristics of AQ compounds are related to the molecular structure and to the nature and relative pos- itions of the electronic states AQ is character- ized by the electronic states S,, T, ,+, T,,. , S,,,, , s . The weak long-wavelength dti to the &,
absorption is transition Phosphorescence
occurs from the T,,=. transition Both transitions are mainly due to the carbonyl group, which ensures minimum energy difference between the lowest excited and ground (SO) electronic levels.3’ S n,n. transitions are responsible for the intense short-wavelength absorptions.** 3’
The optical properties of AQ derlvattves are modified by various factors. the nature and posttions of the substituents, the formation of hydrogen bonds, and other mtermolecular and mtramolecular Interactions. The spectral, photochemtcal and photophystcal properties of the AQs have recently been reviewed 32
ACID-BASE PROPERTIES
Studies have been made of the effect of pH on the spectra of AQ derivatives, m terms of the acid-base equtllbrta,33-36 which depend on the nature, number and posttion of the substituents
571
572 AURORA NAVAS DIAZ
Fi, 0 4 Fig 1 Basic chemical structure of l,lO-anthraqumone
Although the agreement between the various reports of pK, values is generally quite good, there are some discrepancies, which may be attributed to differences m the solvent system and the method of calculation.
In strong acid media, the nitrogen atom of I- and 2-ammoanthraqumone is protonated3’ and m suffictently acidic media so are the sulphomc groups m 1,5- and 1 ,S-dihydroxyanthraqumone- dtsulphomc acid (pKAr(sO,njH+ = -6.03 and - 3.90 respecttvely).38 At pH < 4-6 the immo- nitrogen atom m arylammoanthraquinones 1s protonated 33
The acidity of a derivative depends on the electron-donor or acceptor nature of the sub- stituent and on the conlugation effects mvolved
Generally, the pK value for the ammo group is higher for the non-sulphonated compounds than the corresponding sulphonated deriva- tives 33*34,39-4’ This is usually attributed to the mductive effect of the sulphonate group leading to easier ionization of the ammo group.
1,4-Diammoanthraqumone and 1 ,Cdihy- droxyanthraqumone have higher pK, values than those for the imine groups of Qumizarm Green and its non-sulphonated derivative. For the diammoanthraqumone this is attributed to the greater electron-donor power of the aryl- ammo substituents m the latter compounds, and for the dihydroxyanthraquinones to the effect of intramolecular hydrogen bonding 33 The effect of different substituents can be observed m the pK value of the ammo group for some 1-ammoanthraqumone derivatives. for I-ammoanthraqumone-2-sulphonic acid pK, = 3 79, for 1-ammoanthraqumone-2-carboxyhc acid pK, = 5 74, for 1-ammo-4-hydroxyanthra- qumone pK, = 9.10, and for I-amino-2-bromo- 4-hydroxyanthraqumone pK, = 9.93 23
Changes m the posttion of substitution can affect the pK values. For example, the values for I-hydroxyanthraqumone are about two units greater than those for the 2-hydroxy com- pound,35 but the dissociation constants of 1,2- dihydroxyanthraqumone are similar to those of the 2,3-dihydroxy derivative 42
Intramolecular hydrogen bonding also affects the acidity of AQ derivatives The markedly higher pK values of the 2- than the 1 -derivatives have been attributed to mtramolecular hydro- gen bonding. ” Taking as examples ahzarm (1,2-dihydroxyanthraqumone) and qumahzarm (1,2,5,8-tetrahydroxyanthraqumone), the hy- drogen bond of the 8-hydroxyl group with the carbonyl group should affect the stability of the hydrogen bond of the 1-hydroxyl group with the same carbonyl group, this reduces the bastctty of the 1-hydroxyl group.43
In methanol, the ammo- and N-substituted 2-ammoanthraqumones are markedly more basic than the correspondmg l-ammo deriva- tives. Hydroxyanthraqumones show a similar effect.” The basic strength of l-dimethylammo- anthraqumone is higher than that of either ammo- or methylammoanthraqumone, because m the former the ammo group is out of the plane of the aromatic nucleus, so the comu- gation is reduced and the group tends to exert its normal basictty.”
The pK values measured m pure aqueous solutions are mostly higher than those obtained m mixed solvents (~40% v/v water/organic solvent), the latter leading to increased iomz- atton,33*34*37*44 but pK values have been reported for 1,4-dihydroxyanthraqumone,42 1,8-dihy- droxyanthraquinone45 and 1,2,7-trihydroxy- anthraqumone‘@ m water which are greater than those obtained m mixed solvents (>30% v/v water/ethanol).
The ionization of AQ derivatives is Influenced by the nature and concentration of the solvent system. The changes m pK, with organic solvent concentration, though mamly governed by the dielectric constant, are also affected by the solvent basictties 33*34
The pK of AQ derivatives increases as the dielectric constant of the medium decreases, e g., in the presence of high proportions of alcohols,33*34’46 acetone33,34 or dioxan33 47 but de- creases with increase m amount of ethylene glycol or glycerol. This is explained on the basis that the latter solvents act as proton- acceptors rather than donors, leadmg to easier dissociatton.33*”
The acidity constants of hydroxy- and ammo- anthraquinones m 1.2 v/v dioxan-water are always higher for the excited smglet3748 and triplet49 states than for the ground state, but the triplet state constant lies much closer to the ground state value than does that for the singlet state
Analytlcal apphcatlons of l,lO-anthraqumones A rewew 573
Some AQ derivatives, mainly the hydroxy- anthraqumones, change colour with pH and have been used as acid-base indicators. For analytical purposes the most suitable transition of HAQs is that between yellow and red. Qumizarm (1,4-dihydroxyanthraquinone) and Alizarm S (1,2-dihydroxyanthraqumone sul- phonate) are very good mdicators with a colour change quality similar to that of Bromocresol Green; ahzarm is also a good indicator but with shghly lower colour change quality, and the colour change of qumahzarm (1,2,5,8-tetra- hydroxyanthraqumone) IS still poorer.sO
Diaminoanthraquinones, which do not show such marked colour changes with pH as do various ammohydroxyanthraqumones m aqueous medium, have been used as indicators m the titration of weak bases such as urea and sodium acetate, benzoate or sahcylate with perchloric acid m glacial acetic acid alones’” and mixed with other solvents,56~s7 but are not applicable m the titration of weaker bases with perchloric acid.‘*
COMPLEXATION REACTIONS
Anthraqumones have long been used as ana- lytical reagents and particularly as chromogenic and fluorogemc hgands for various metal ions.
The co-ordmation reactions of AQ deriva- tives characteristically display moderate selec- tivity and large absorbance changes.‘* The absorption and emission properties of these compounds and their complexes give great fluonmetric potential, but the relatively high blank signal and the comparatively small spectral shifts due to complexation impair the analytical performance 58
The optical characteristics of the anthra- qumone co-ordmation compounds are due to mtrahgand transitions, so the complexation re- sults m modification of only the position of the absorption and emission maxima, and non- fluorescent derivatives do not generate fluor- escent complexes. It has been shown that, depending on the acidity, the solvent and the metal ion, the same reagent may give erther excellent or poor analytical response s9
When a more highly acidic reagent, such as Quimzarm Green m comparison with 1,4- dihydroxyanthraqumone,a is used, the stability of the complexes of the more acidic reagent will be lower than that of the complexes of the less acidic compound, and also the formation of its
complexes should be affected less by the pH of the solution.60
When the colour contrast IS due to differences in the positions of the absorption band maxima of the various acid-base forms, to make full use6’ of the contrast it is essential to adjust the acidity or choose a solvent so that the free reagent will be in its molecular form, but the anionic form will be present m the metal complex.
As regards the influence of the solvent m the complexanon, it has been shown46 that it IS necessary to consider the influence of the di- electnc constant of the medium An mcrease m the dielectric constant causes6* a decrease m the relative fluorescence intensity m both re- agent and complex The absorption maxima of both the reagent and the complex are shifted to longer wavelengths with mcreasmg solvent polarity The pH for maximum difference in absorbance between 1,2,7-trihydroxyanthra- qumone and its Cu(I1) complex as a function of the dielectric constant of the medium, shifts m parallel to the correspondmg pK value for the reagent.&
The nature of the metal, its position m the Periodic Table, the iomc charge, radius and potential, cation-field energies etc., all affect the properties of the complexes.
It has been shown43 that the molar absorptiv- ity and luminescence intensity of alizarm and its complexes with group IIIa and IIIb elements are inversely related to the cation-field energy The higher the field energy of the cation introduced into the complex, the higher the degree of localtzation of the n-electrons of the hetero- atom, and the greater the electron-density deficiency m the ring. This affects the optical properties of the molecules Hence reagents such as ahzarin have been recommended43 for deter- mmation of elements with cations which have a lower cation-field energy or iomc potential, z.e , cations with large radius and small charge
Mixed-hgand complexes of elements of subgroup IIIb with hydroxyanthraqumones and auxiliary ligands have been widely studied The auxiliary hgands mclude 8-hydroxyqumo- line,63*6( ethylenediamme,64*65 phenazone,66*67 benzoic acid,6s N-phenylbenzohydroxamic acid@ and sulphosahcyhc acid.” It has been shown that auxiliary hgands contammg mtrogen donor atoms form the most stable ternary complexes.70 The order of stability of the ternary Th(IV) complexes of 3-ammo- 1,2-dihydroxyanthra- qumone is as follows, for the auxihary hgands
514 AURORA NAVAS DIAZ
named: l,lO-phenanthrolme > 2,2’-bipyridyl > sahcyhc acid > 5-sulphosahcyhc acid = 5-mtro- sahcyhc acid. This order 1s explamed” as due to mteraction between the n-systems of the two hgands bound to Th(IV) These ternary com- plexes are more stable than the binary complex.
For the mixed-hgand complexes of the rare- earth metals with 1,2,5,8,-tetrahydroxyanthra- qumone and 8-hydroxyqumohne the molar absorptivtty depends directly on the ionic poten- tial (cation-field energy) 43 Addition of boric acid to the system increases the linear range 63
The reported complexation reactions of AQ derivatives generally show moderate sensitivity and selectivity, but m some cases the variables were not optimized for modern mstrumen- tation Also, recent approaches62,7’-73 have improved the general performance of the ana- lytical methods, especially sensitivity and selec- tivity For example, a sigmficant improvement m sensitivity and selectivity m the determmation of Be(I1) 1s achieved by use of its mcluston complex m cyclodextrms 58 Again, develop- ments m the treatment of spectral signals allow analysis of mixtures of lanthamdes at trace levels, which is otherwise difficult because of interelement interferences ” ”
The most important mformation on the use of anthraqumones m determmation of elements by complexation reactions is given m Table 1 at the end of the paper The most widely used reagents and their types of co-ordmation are summarized below
Hydroxy-, polyhydroxy- and carboxyanthra- qumones have two oxygen donor-atoms, some typical configurations are shown m Fig 2. Thus chelation by the qumonoid oxygen atom and the hydroxy group occurs m the Ahzarm S com- plexes with Th(IV), Hf(IV) and Cr(III), and chelation by the two hydroxyl groups of the same reagent occurs with Pb(II), V(V), W(VI), UOz(II)74 and with Zr(IV) ”
It has been reported that with l-hydroxy- anthraqumone an ML, chelate is formed with Mg(I1) whereas with 1 ,Cdihydroxyanthra-
Fig 2 Configuratlons of (a) hydroxy-. (b) polyhydroxy- and (c) carboxyanthraqumones
quinone a 1.1 complex is formed.76 The latter was reported to be polymeric.
Some complexes are polymers. For example, the fluorescent product formed between 1,2,4- trihydroxyanthraqumone-3-carboxyhc acid and Cu(I1) 1s said to have a polymeric complex structure.” Polymeric characteristtcs have also been assigned78 to the lakes that are often formed by AQ derivatives and metal tons
(Fig 3). The ahzarm-Co(II)-Co(III) complex shows
a similar structure, with partictpatton of the 2-hydroxy group m the polymerization.” It has been reported that chain co-ordination poly- mers of 1,4-dthydroxyanthraqumone and biva- lent metal ions with co-ordmation number 4 can be formed from the metal acetylacetonates.76 Alcohol solutions of o-hydroxyanthraqumones form internal complex salts when treated with magnesium acetate. *’ Because of its polarity, N,N-dimethylformamide is very often used as the medium for obtammg polymers “q8’
The formation of msoluble hydroxyanthra- qumone complexes of ion metals has long been used m quahtattve analysts. Thus, Al(II1) is identified by means of the red lake formed with ahzarm m baste medium Qumahzarm IS used for the identification of magnesium and various bt-, ter- and quadnvalent cations by means of lake formation.
Amino-, polyammo- and ammohydroxy- anthraqumones are compounds with N,N or 0,N donor-atom configurations, as shown m Fig 4
Fig 3 SchematIc formula of the lakes m which M:’ IS a tervalent metal and M, IS hydrogen, or a umvalent, blvalent
or quadrlvalent metal
AnalytIcal apphcations of I,lO-anthraqumones A review 515
Fig 4 ConfiguratIons of (a) ammo-, (b) polyammo- and (c) ammohydroxyanthraqumones
The co-ordmatton sites of the complexes of these AQ derivatives may be the carbonyl and ammo groups, but the structure of the chelates may be due not only to the donor character of the carbonyl group and the displacement of a proton from the ammo group by a metal but also to the donor character of the ammo mtro- gen atom. Furthermore, several of the reactions with metal ions may be attributed to redox processes.
Ammoanthraqumones, m contrast to the “broad spectrum” reacttvity of the hydroxy- anthraqumones, exhibit selectivity m their reac- tions, particularly m ethanohc medium.82 This selectivity is decreased m sulphurtc acid medium, however.8384 Thus m ethanohc media ammoanthraqumones react with the transition metal tons Pd(II), Cu(I1) and Co(II), which tend to prefer mtrogen donor atoms The Cu(I1) complex wtth 1,2-diammoanthraqumone has been used as a metallochromic mdicator m the complexometnc titration of calcmm and strontium 85
In contrast, m concentrated sulphuric acid medium, ammoanthraqumones co-ordinate with Se(IV), boric acid, calcium, strontium and barium Selenmm(IV) reacts with aromatic compounds contammg ammo and carbonyl groups. Of the monoammo anthraquinones only the l-isomer reacts to form the dimer (Se),( 1 -AAQ), 86 Similarly, 4,5-dtamino- 1,8- dihydroxyanthraqumone has an ammo group adlacent to the qumone oxygen and reacts with Se(IV) to give both an SeL and an SeL, complex *’
Ammohydroxyanthraqumones form metal co-ordmation compounds which have the characteristics of both the ammo- and hydroxy- anthraqumone complexes With metals such as Be, Th and the lanthamdes they react in a similar manner to the hydroxyanthraqumones, and with Pd and Cu similarly to ammoanthra- qumones The stability constant of the 1.1 complexes of some rare-earth metals with 1 -ammo-4-hydroxyanthraqumone are very stmilar, mcreasmg as the size of the cation decreases ‘*
The anthraquinone-complexan reagents are derivatives which possess an iminodiacetic group, and have been applied for the photo- metric determination of several tons and as complexometnc mdicators 89.90 Ahzarm Com- plexan (Ahzarm Fluorme Blue) forms red com- plexes with Ce(III), La(II1) and Pr(II1) When fluoride is present tt replaces a molecule of water in the co-ordination sphere of the metal ion and a blue ternary complex 1s formed (Ftg. 5).*9-92
Other anthraqumone derivattves used m complexation reactions are mtroanthraqumones and arylaminoanthraqumones. It has been re- porteds9 that the reaction between Tt(IV) and mtroahzarin gives a colour contrast comparable with that of the reaction of Al(II1) and alrzarm l,CDiamino-5nitroanthraqumone is not itself fluorescent, but gives an orange fluorescence with tons such as Au(II1) and V(V).93 The complexanon eqmhbna of La(III)94 and Y(III)@’ wtth 1,4-bts(4’-methylamlmo)anthraqumone (Qumrzarm Green) have been studied spectro- photometrtcally.
Among the coloured chelates of anthra- quinone derivatives and transition metal ions, the most widely studied and used is that of Zr with Ahzarm Red S m strong acrd medium This reaction has been applied m the photometric determmation of Zr rn various materials, such as plutomum-uranium fisston alloys95.96 and other alloys97*98 and mmerals.9~‘@’
The most widely studied of the reacttons of AQs with subgroup IIIa elements are those of aluminium with Ahzarm Red S, which is smt- able for determination of alummmm m various matertals,‘0’-‘03 and those of boron with carmmlc acid’“-‘lo and qumalizarm.‘“~“‘-“4
The reaction between fluoride and Alizarm Complexans9-92 is one of the few colour reac- tions of the fluoride ion. It has been widely studied and applied.“4-‘20
/\ 0
*
H2: lF I ’ ocdCe~c02
’ &L~/CIH, 2
0
Fig 5 Chemical structure of the ternary complex Ahzarm Complexan-Ce(III)-F-
576 AURORA NAVAS DIAZ
0 NH2 0 NH
0 0
0 1; II
0 0
Fig 6 Oxldatlon react’on of p-ammohydroxyanthraqu’none
REDOX REACTIONS
Chemical oxldatlon
Anthraqumone derivatives readily undergo reduction-oxidation reactions under proper condittons of acidity. Ammo-, hydroxy- and ammohydroxyanthraqumones are capable of further oxidation to a variety of amon radicals, qumones and qumone-immes. Oxidatton of o- or p-ammo- and ammohydroxyanthraqumone results m the correspondmg o- or p-qumone through the mtermediate ammo- or di-immo- qumone”‘~‘** (e g , Fig 6)
The colour or fluorescence change accom- panying their oxtdation facilitates the use of a number of these AQ derivattves as redox mdicators m titration of reducing agents such as ascorbic acid,‘*’ ‘23-‘27 phenazone,‘*’ arsenic(III),‘2’~‘23-‘27 hydrazme sulphate,‘*’ Fe(II),‘*’ but the reagents decompose m the presence of an excess of oxidizmg agent and hence cannot be used’** m titrations of oxidants.
There appear to be two stages of oxidation,‘28 the first (perhaps a one-electron oxidation to an amon radical) producing a hypsochromtc shift, and the second (perhaps a further one-electron oxidation to give the qumone) producing a bathochromic shift to restore the original colour
The redox reactions of AQ derivatives have been used for kmetic determmation of the oxi- dant, the reductant or a catalyst Catalytic methods give very high sensitivity ‘2g-‘33 Their mechanisms have been reviewed by Bontchev.‘34
AQ derivatives provide good indicator reac- tions for kinetic photometric and fluorimetric methods of analysis, because they give pro- nounced colour”’ ‘34 and fluorescence”* ‘34-‘37 changes m their redox transformation, and extremely low concentrations of the species involved can be determmed.
Kinetic determmations based on the redox reactions of AQ derivatives show a greater selectivity ‘22 ‘30-132 ‘34 '36'37 than those based on
the complexation reactions.
Various AQ derivatives have been used m indicator reactions Thus, o-dihydroxyanthra- qumones are oxidized by hydrogen peroxide m the presence of traces of cobalt,13) ‘38-‘40 m borate buffer. The ahzarm-hydrogen peroxide mdi- cator reaction““’ permits the determmation of cobalt m a range of about l-7 ng/ml, Zn, Cd and Ni interfere
The quinahzarm-H,O, (or sodium perborate) reaction is quoted as an indicator reaction with which the sensitivity for Co at 100” is 20 and 0 2 pg/ml with H,O, and NaBO, respectively as oxidizmg agents. I38 After a detailed optimiz- ation study ‘33 the same reaction has been used at 25” to determine Co (sensitivity 0 5 ng/ml) A mechanism similar to that for enzymatic reac- tions was postulated to explain the optimal conditions found. Tartrate, citrate and oxalate have an mhtbttmg effect.
The reaction between 1 -ammo-4-hydroxy- anthraqumone and V(V)‘36 to yield an oxtdation product of the reagent allows a sensitive (loo-530 ng/ml) and selective [only Ce(IV) interferes seriously] kmettc fluonmetric deterrm- nation of V(V)
Fluorimetric’4’ and kmetic-fluorimetric’37 methods have been proposed for the determt- nation of Fe(I1) and Tl(III), based on the intense green fluorescence that appears when these cations react with 1,4-diammo-2,3-dthydro- anthraqumone. The fluorescence is due to the oxtdative transformatton of the reagent m the presence of these cations.
The blue non-fluorescent reagent 4&diammo- 1,5-dihydroxyanthraqumone-2,6-disulphomc acid is transformed mto a pink, highly fluor- escent, product by oxidation m acid medium This reaction is slow, but m the presence of certain morgamc oxidants tt is accelerated and completed m about 30 mm This allows the kmetic determmation of V(V),12* Fe(III),14* Ce(IV),‘43 Au(III)13* and Mn(I1) ‘35 The com- bined action of Fe(II1) and V(V) notably m- creases the sensitivity of either or both determmations, and concentrations as low as
AnalytIcal appkatlons of l,lO-anthraqumones A review 577
1 ng/ml V(V)“’ and 2 ng/ml Fe(III)13’ can be determined
Oxidation of 1,2,4-trihydroxyanthraquinone- 3-carboxylic acid by bromatelM or iodate’4S in hydrochloric acid medium has served as the basis for their spectrophotometnc determi- nation and for a fluonmetric method for iodate’34 which is more selective and 10 times more sensitive than the spectrophotometric method.
Electrochemrcal reduction
Polarographic studies of analytically import- ant anthraqumones have been made, to investi- gate their redox characteristics.39 Because of their qumonoid structure, anthraquinones display mterestmg electrochemical behaviour.39 When reduced I46 by taking up a smgle electron, they form semiqumones, and the uptake of a further electron results m the formation of hydroqumones In all the redox processes of AQs these three oxidation states are expected to be involved. Whether under given experimental circumstances a single two-electron polaro- graphic wave or two one-electron waves will be observed, depends on the stability of the semiqumone Additionally, each oxidation state can mvolve different degrees of protonation.”
The polarographic behaviour of anthra- qumones depends as much on the nature of the derlvatlve39,146-'58 as on the p~,39,146,147.'50,'5Z,lS7,158
the solvent3’ ‘48~‘49,‘53 and the supportmg electro- lyte solution
For the complexes of Alizarm Red S with Be and Al information has been obtained on the structure of the complexes by polarographic reduction of the llgand.‘s9 Similarly, from voltametric and spectrophotometnc studies it has been deduced that the two adjacent hydroxyl groups are involved m formation of the highly stable Zr-Ahzarm Red S complex.7s
It has also been estabhshedlm that the half- wave potential for the polarographic reduction of some AAQs is correlated with the wavelength of maximum absorption m the visible region and also with the polarizabihty of the carbonyl groups. Each AAQ can be determined m the range 0.1-O 5 mg/ml.
Redox photochemrcal properties
The excited states of some AQ derivatives are very reactive chemical species The photo- chemical reactions mvolvmg these species can compete with lummescence for deactivation of the excited electronic states. The photo-
chemistry of AQs has been useful m analytical chemistry, from the point of view of photo- reaction and of deactivation of excited states The absorption and fluorescence spectra of some AQs have been studied m relation to the photochemical properties.2*‘6’ “*
The photochemical oxidation of anthra- quinones is confined to oxidation of the side- chain, which is characteristic of p-qumones ’
Photochemtcal reduction is the simplest photochemical reaction of anthraqumones. It mvolves3*4*3’ the addition of an electron or a hydrogen atom to the oxygen atom of the carbonyl group under conditions where the analogous dark reactions are imposs’ble The facile reduction of AQs to anthrahydroqumones under the influence of light has long been recog- mzed4 as one of the major causes of the photo- mstabihty and photoreactivity of these dyes
The photochemical reactivity of an AQ de- rivative depends critically upon the nature of the lowest excited electronic state Anthraqumones m which this lowest state is n,rr* are assocl- ated3A*3’*‘63 with high photochemical activity, because m that state the oxygen atom of the carbonyl group is electron-deficient, which ren- ders it4 extremely reactive towards the hydrogen atom or electron abstraction. In the case of x,x * states, and more particularly charge-transfer (C-T) states, photoexcitation causes an electron shift towards the oxygen atom, which lessens ‘ts affinity for the hydrogen atom and electron abstraction. Anthraqumones which possess low- lying x,x* or C-T states are therefore compara- tively unreactive
Anthraqumone derivatives vary widely m their photochemical reactivity They are divided into “strong” and “weak” sensitizers’ ‘63 I64 m the oxidatton of the environment The former give phosphorescence emission and semi- quinone radical formation, while the latter give only fluorescence emission ‘64
AQ and its derivatives with electron-accept- ing substituents (-HS03, -N02, halogens) are very photochemtcally reactive, but the position of the substrtuents can have a profound effect on their photochemical behaviour.4 ‘63 Sodium anthraqumone-2-sulphonate, and 2,6- and 2,7- disulphonates are more active sensitizers than the l- and 1,5-sulphonates, and the 1,8-disul- phonate is mactive.‘63.‘65
Powerful electron-donating groups (-OH, -NH,, -NRR’) diminish the sensit’zmg power of AQs in the photochemical pro- cess ‘.3~‘63 a substituent m the l-position gener- 3
Tab
le
I Ph
otom
etnc
an
d fl
uorl
met
rlc
met
hods
fo
r de
term
mat
lon
of m
orga
mc
soec
les
with
ant
hraq
umon
e de
rlva
tlves
,_
Ion
Rea
gent
T
ype
of
Inte
rfer
ence
s,
3
met
hod
Con
dltlo
ns
Ran
ge
rem
arks
R
efer
ence
Al(
II1)
1,
2DH
AQ
-3S
I ,4D
HA
Q-2
S
1,2,
4TH
AQ
-3s
1,2,
7TH
AQ
A
hzan
n C
ompl
exan
c/Ph
pH
4
8, d
490
nm
0
08-O
76
ngjm
l c/
Ph
MeO
H,
1560
nm
<
I 7
pgf
ml
c/F
pH 4
76,
I,
500,
I,
558
nm
1 l-5
4 ng
/ml
c/Ph
pH
5
5. i
58
0 nm
0
5-3
fig/
ml
c/Ph
Z
500
nm
, st
andm
g tim
e 2
4 hr
O
-2 &
ml
c/Ph
pH
4 I
-4 3
, he
at
at 7
0”, s
tand
mg
l-12
fi
g/m
l
Mn,
Fe
, C
a B
e, S
C, T
h, T
I, Y
, Z
r,
F-,
PO:-
, la
ntha
mde
s
Det
n in
pre
senc
e of
Fe
and
T
I
171
172
173
174
175
176
Au(
III)
IA
DA
AQ
-2JD
S c/
Ph
pH
9,14
25
nm
5-30
~g/
mI
Man
y to
ns
177
B(I
I1)
4,8D
A-I
,jD
HA
Q-2
,6D
S k/
F
I ,4D
HA
Q
c/F
I ,4D
HA
Q-2
S c/
F
I ,8D
HA
Q
c/Ph
1,
2,5,
8TT
HA
Q
c/Ph
C
arm
mlc
ac
ed
c/Ph
1,
8DA
-4,5
DH
AQ
c/
ph
ISD
H-4
,8D
AA
Q
c/Ph
b 15
M H
CI,
t,,
525,
i,
585
nm
91-9
6%
H,S
O,,
A,,
365,
1,
595
nm
cone
H
2S04
, A
,, 52
2, &
, 57
8 nm
, st
andm
g tim
e >
15
mm
co
ne
H,S
O,,
1 58
0 nm
93
%
H,S
O,,
1615
nm
92
-94%
H
ZS
04,
1610
nm
96
%
H&
, 1
525
nm
96%
H-$
0,,
Iz 6
00 n
m
46-2
65
peg
Fe,
Ce,
V
132
4 x
lo-+
-8
x Io
-jM
I-
, C
IO;,
Sb,
Fe
178
25-2
50 n
g/m
l N
O;,
F-
179
0 l-
3 pg
/mI
H,B
O,
Fe,
NI,
Co,
Cr
180
OO
I-O
1%
G
e, A
s, F
- 11
1 0
15-I
6 r
g/m
l 10
5 2-
7 Pg
O
xida
nt
amon
s,
F-,
TI
181
2-10
I.r
g 18
2
NO
1,
2DH
AQ
-3S
1,4D
HA
Q-2
S
I PD
HA
Q-2
,6D
S
1 A-4
HA
Q
1 H-2
CA
Q
4,8D
A-
1,5D
HA
Q2,
6DS
C
arm
mlc
ac
td
Ahz
ann
Com
plex
an
c/F
c/F
c/Ph
c/
F c/
Ph
c/ph
c/
Ph
PhO
z-D
S c/
Ph
c/Ph
c/
Ph
c/F
c/Ph
pH
54-5
6,11
8O
nm
pH 6
, i
575
nm
8 x
IO-l
M
HA
c,
2,
475,
&,,5
75 n
m
pH
7, 1
530
nm
, 7%
Na,
S,O
,, he
at
5 m
m a
t 60
-70”
0
02M
NaO
H,
&
540,
&,,,
620
nm
pH
10
2,
IO-*
M b
-cyc
lode
xtrm
4
x IO
-‘M
N
aOH
, t
4704
80
nm
A,
470,
&,,,
580
nm
00
2N
NaO
H,
i 64
5 nm
pH
4,
1580
nm
pH
7 2
, L 4
80 n
m,
extn
w
ith
Ado
gen
soln
m
tol
uene
D
H 6
. Z
550
nm
0 2-
4 7
pg/m
i I-
20
yg
l-7
ng/m
l 0
I fi
g/m
l
Pb,
Zn,
Cu,
Ce,
Co,
N
I, V
(V),
MO
PO
:-,
F-,
Al
183
184
185
186
0 2
&m
l 10
-70
ng/m
I 0
4-l
2 jig
/ml
3&I
30 n
g/m
l 04
-I
13 &
ml
0 4-
I 6
pg/m
i 0
09-O
36
pg/m
l
Lar
ge a
mts
of
Cu
and
smal
l am
ts
of A
l an
d Fe
Int
erfe
re
LI,
Cr(
VI)
Mg,
AsO
:-
Zn,
A
l, Y
C
u, C
r, C
o, V
(V),
Ag,
Ge,
AI,
NI
Seve
ral
ions
Se
vera
l Io
ns
187
58
188
189
190
191
192
5-35
lie
19
3
1 H-2
CA
Q
c/Ph
50
% E
tOH
, pH
I I
, d
463
nm f
or M
g 0
I-I
5 pg
/ml
Mg
Be
up t
o 0
4 jig
/ml
194
1492
nm
for
Be
004-
04
ue/m
l B
e M
E U
D to
1
5 up
/ml
194
1,2,
4TH
AQ
-3C
rx
/Ph
I 92
M H
CI,
1 5
20 n
m
I-8
pug/
ml
Oxi
dant
s an
d ot
her
Ions
14
4
Ca(
l1)
1,2D
HA
Q-3
S 1,
8DH
AQ
1,
2,4T
HA
Q-3
S 1,
2,3T
HA
Q
1,2,
7TH
AQ
1,
4DA
AQ
Abz
arm
C
ompl
exan
A
nthr
apu~
unn
Com
plex
an
c/Ph
c/
F c/
Ph
c/Ph
c/
Ph
c/Ph
pH
102,
1509
nm
0 O
lM N
H,,
A,,
485,
1,
615
nm
pH
11
pH
10 5
, 80
% D
MF
EtO
H,
1 56
0 nm
50
% H
2SO
d, A
: 400
nm
<O
1.5
mgj
ml
50-5
50 n
g/m
l 0
5-4
5 pg
fml
2-12
fig
/ml
l-6
jig/m
l 14
-35f
lg/m
l
c/P
50%
H,S
O,,
AX
410
, &
,,, 5
80 n
m
150-
400
ng/m
l c/
Ph
pH
10 3
1,1
610
nm
2-10
p&
ml
c/Ph
pH
IO
58,
R 5
80 n
m
2-10
@g/
ml
195
Seve
ral
mns
19
6 19
7 M
any
eons
19
8
No
Inte
rfer
ence
by
Mg,
Sr,
Ba,
PO
:-,
ED
TA
if
201
Ba,
Sr
caus
e po
sitiv
e er
rors
20
2 20
3
Cd(
H)
CeW
)
Co(
H)
Cr(
II1)
Cuf
ll)
F-
Ahz
arm
C
ompl
exan
1,2D
HA
Q-3
S
4,8D
A-1
,5D
HA
Q-2
,6D
S
1,2D
HA
Q
1,2D
HA
Q-3
S 1,
2,5,
8,T
TH
AQ
1,2,
4TH
AQ
-3S
t ,Z
DA
AQ
1,
2DA
AQ
-3S
1,2D
HA
Q-3
S
1,2,
7TH
AQ
1,2,
4TH
AQ
-3C
1 ,Z
DA
AQ
4,
8DA
-1,5
DH
AQ
-2,6
DS
Ant
hrap
urpu
nn
Com
plex
an
1,2D
HA
Q-3
S
1,2D
HA
Q-3
S f
Th
1,4D
HA
Q-3
S +
Zr
1,2,
3,5,
6,7H
HA
Q +
Zr
Abz
arm
C
ompl
exan
c/Ph
pH
8,
i,
620
nm,
stan
dmg
time
30 m
m
2-11
jig
/ml
204
cfPh
pH
9 9
-10
10, L
500
nm
00
7-O
15
%
Impu
ntIe
s ca
n be
ext
ract
ed
at
205
pH 4
-5
with
oxm
e m
chl
orof
orm
k/
P 0
2M &
SO,,
1,
525,
&,,
585
nm
0 02
-O 3
7 /I
glm
l H
g, V
, C
r(V
I)
143
k/ph
pH
9 4
, 0
035M
H,0
2 2
x lo
-‘-2
x
1O-4
fig/
ml
Zn,
Cd,
NI
140
k/Ph
15
10
nm
0 05
&m
l 20
6 k/
Ph
pH
I2,1
56
5 nm
, 25
”, H
,O,
I x
10-s
-2
x lo
-7M
C
N-,
ta
rtra
te,
titra
te,
C,O
$-
133
lOO
”, H
,O,
c20
pg/m
l 13
8 IO
O”,
Na5
B0,
C
O 2
pg/
ml
138
c/Ph
pH
538,
IZX
Wnm
O
-2 5
&m
l N
l 20
7 c/
Ph
0 32
M N
aOH
, d
690
nm
l-3
&m
l St
abdt
zed
with
po
ly(v
my1
alc
ohol
) 20
8 c/
Ph
pH
7 8,
I
580
nm,
stan
dmg
15 m
m
0 95
-3 8
@g/
ml
209
c/Ph
pH
3-
6,15
25
nm
0 2-
10 4
&g/
ml
210
c/Ph
pH
8,
1 52
0 nm
, ex
tn
with
O
-7 ,
g/m
l 21
1 ls
oam
yl
alco
hol
c/Ph
0
02M
NaO
H,
1750
nm
0
l-l
0 &
g/m
l M
any
Ions
21
2 c/
F O
OIl
w N
aOH
, 80
% D
MF,
A
,, 51
5 nm
50
-250
ng/
ml
213
c/Ph
0
32M
NaO
H,
1 65
0 nm
l-
7 pg
/ml
Stab
lhze
d w
ith
poly
(vm
y1 a
lcoh
ol)
214
c/Ph
pH
7
13, 1
690
nm
3-9
jig/m
l 21
5 c/
Ph
pH 4
6,
1 51
5 nm
l-
20
pg/m
l 21
6
c/Ph
pH
2 9
-3 0
.1,
415
nm,
1 14
-l 9
0 m
g/g
217
F-
titra
ted
wtth
0 O
lM Z
r(IV
) ic
/Ph
1% N
H,O
H
HC
l, L
525
nm
0
05-l
fi
g/m
l A
l, SO
;-
218
i 52
5 nm
0
4-4
fig/
m1
D~f
fe~n
tl~I
met
hod
s/Ph
0
1M H
Cl,
1545
nm
O
-3 5
pg/
ml
~25
&g/
ml
SOi-
21
9 Ic
/Ph
IM H
Cl,
1560
nm
G
-7 p
gjm
l 22
0 c/
Ph
pH 4
6,
1. 5
74 n
m,
0 08
-l
2 m
g/l
Flow
-mje
ctio
n de
term
mat
ton
221
Na
dode
cyl
sulp
hate
---c
ontm
ued
Ion
F-
Fe(I
I1)
Ga(
II1)
Tab
le
I-co
ntm
ued
i?
Typ
e of
in
terf
eren
ces,
R
eage
nt
met
hod
Con
dmon
s R
ange
re
mar
ks
Ref
eren
ce
Abz
ann
Com
plex
an
f L
a tc
/Ph
La
com
plex
~r
nrno
b~l~
~d o
n 95
0 pg
N
H:,
Mg,
Ca,
Al.
Fe(I
lI)
222
Am
berh
tc
CG
-400
or
IRA
-938
A
bzar
m
Com
plex
an-S
S +
La
tc/P
h L
a co
mpl
ex
lmm
oblh
zed
on
0 00
3-l
pg/m
l 22
3 A
mbe
rhte
C
G-4
00 o
r IR
A-9
38
Alu
arm
C
ompl
exan
tc
/Ph
pH 5
O-5
2,
i 61
0-62
0 nm
O
-60
pg
Al,
Fe,
Sn,
Ca,
Mg
59-6
1, 2
24
+C
e(IV
) or
La
F’O
i- ,
SO;-
, C
z(Y
4-, o
xrda
nts
1,2D
HA
Q-3
S c/
Ph
pH >
4 2
, I
570
nm,
extn
w
ith
0 02
-l
5 fi
g/m
l 22
5 A
hqua
t 33
6 so
ln
m C
HC
I,
t ,2,
4TH
AQ
-F-
c/Ph
pH
8 1
, il
595
nm,
extn
m
to
MIB
K
0 02
5-O
250
pg/
ml
Mas
ked
with
CN
- 22
6 1,
4DA
-2,3
DH
yAQ
=
JF
pH49
0
28-O
6 &
ml
Au,
Tl,
Ce,
Pt
141
k/F
pH
3 4,
1,40
0,
&,
470
nm
0 O
S-0
6 pg
/ml
Au,
Tl,
Ce,
Pt,
V(V
) I3
7 4,
8DA
-l,S
DH
AQ
-2,6
DS
k/F
0012
M
HC
I, ,I_
525
, &
,,, 5
85 n
m
2 5-
25 f
ig
Au,
C
e, V
(V),
Th,
F-
142
k/F
25 p
ug V
(V)
I 5-
25 j
Lg
BrO
;,Tb
131
2
1,2D
HA
Q3S
c,
lPh
pH
3-5,
Z 4
90 n
m
0 55
-14
pgfm
l 22
7 8
1,2D
HA
Q-3
S c/
Ph
pH
3 3,
20%
EtO
H,
1 50
5 nm
, 0
28 c
g/m
I N
o In
terf
eren
ce
by A
l, C
u, I
n,
228
0 04
M h
exad
ecyl
pynd
mm
m
brom
ide
Sb,
Tl,
Ce,
Zn
; 1,
2,5,
8’IT
HA
Q
c/P
h
pH
5, N
H,O
Ac,
N
aF,
heat
at
80”
0 l-
10
fig
Man
y Io
ns
229
2 G
e(IV
) i,2
DH
AQ
3S
c/Ph
pH
7,
A 4
70 n
m,
extn
m
to
CC
&
!%-4
fl Pcc
g I ,
2,3T
HA
Q
c/Ph
90
%
MeO
H,
4 x
IO”‘
*M, 1
490
nm
1-5
jfg/
ml
1,2,
4TH
AQ
c/
Ph
40%
E
tOH
, pH
l-
4,
I, 4
90 n
m
0 4-
12 7
pg/
ml
1,2,
7TH
AQ
A
hzan
n C
ompl
exan
Ahz
arm
C
ompl
exan
+
Rh~
amln
e 6G
A
hzar
m
Red
S (
II)
+D
PhG
(I
) O
~ina
ll~rl
n +
DPh
G
. H
NIV
I
c/Ph
c/
Ph
c/Ph
c/
Ph
tc/P
h tc
/F
tc/P
b
tc/P
h
cone
H
,SO
., 90
%
EtO
H,
4 x
10v4
M N
H,,
k 47
0 nm
pH
7,
d 4
45
pH 8
, A
450
nm
pH
S-6,
A 5
20 n
m
A,._
543
nm
pH 4
, I
475
nm,
extn
m
to
CH
CI,
ac
eton
e (1
4)
at p
H
7-8
oH 4
. A
500
nm
. ex
tn
with
CH
Cl,
0 4-
15 f
ig/m
l 0
5-4
pg/m
l 0
2-4
jig/m
l G
eG,
0 5-
6 pg
/ml
Ge
0 02
-l
@g/
ml G
eO,
2-10
0 ng
/ml
GeO
, O
OIW
63
pg/
ml
0 l-
2 u&
ml
-
BO
;, S@
-, N
O;,
OA
c-,
PO:-
do
not
in
terf
ere
4 1
(R
Ge)
com
plex
fo
rmed
4 1
(R
Ge)
com
plex
fo
rmed
C
l-,
Br-
, I-
, N
O;,
ClO
;
230
231
232
233
234
235
236
237
Ion
asso
c w
ith G
e (I
) (I
I)
ratlo
1
2 2
238
239
$ l-4
-
1,2D
HA
Q-3
S c/
Ph
O-8
0 m
gjl
Hm
z 24
0
i ,2R
HA
Q-3
S
c/P
h
pH
3 8-
4 5,
L 5
30 n
m
0 23
-27
pg/m
l 24
1 A
hzar
m
Com
plex
an
c/Ph
pH
4 3
, A
520
nm
l-
9 fi
g/m
l Se
vera
l io
ns
242
1,2-
DH
AQ
-3S
+ D
PhG
tc
/Ph
pH
5 3-
5 9,
,l
525
nm,
extn
m
to C
HC
I?
0 3-
2 8
@g/
ml
243
10;
1,2,
4TH
AQ
-2C
rx
/Ph
70%
EtO
H,
1 !%
A4 H
CI,
i:
520
nm
50-3
50 /
Jg
Oxi
dant
s an
d ot
her
ions
14
5 rx
/F
1 20
M H
CI,
ii,,
515
, &
, 62
5 nm
S-
50 p
g O
xida
nts
and
othe
r Io
ns
244
Laf
III)
1 H
AQ
-2C
c/
Ph
pH 4
9,8
0%
EtO
H,
&,,
465,
1,,
520
nm
0 1-
1 jig
/ml
Seve
ral
ions
1,
2DH
AQ
-3S
45
C/P
h pH
35_6
5,15
20nm
0
42-1
0 fi
g/m
l M
any
Ions
1,
2,5,
8TT
HA
Q
246
c/Ph
pH
6-8
, 1
570
nm
0 08
-l
6 fig/ml
1,2D
HA
Q-3
S +
phe
nazo
ne
In p
rese
nce
of b
one
acid
24
7 tc
/Ph
pH
5, I
540
nm
, ex
tn
mto
I-
6 j&
W
66
buta
nol
or r
sobu
tyl
alco
hol
1,2D
HA
Q-3
S tc
/Ph
rl 5
30 n
m,
extn
m
to b
utan
ol
30.-
-so
pg
64
f I-
hydr
oxyq
umoh
ne
W
c/Ph
pH
7
6,40
%
DM
F,
,? 6
00 n
m
2 x
10-5
-J
x 10
-4M
94
LI(
I)
1,8D
HA
Q
c/F
90%
E
tOH
, /1
, 49
5, &
,, 62
5 nm
10
0-70
0 ng
/mf
Sepa
ratio
n of
LI
IS re
com
men
ded
248
>
c/F
90%
ace
tone
, 2
5 x
10s4
M N
aOH
50
-450
ng/
ml
$ A
,, 52
5, &
,, 61
5 nm
4
Lu(
III)
/Pr(
II~)
iii
.
1,4D
HA
Q
c/F
90
%
MeO
H,
pH 4
5,
A 5
60 n
m f
or L
u I-
100
mg
Lu
Pr t
oler
ance
fr
om
1 5
to 5
1
71
pl
1 56
4 fo
r Pr
3
Mg(
W
L
D
1,4D
HA
Q-2
S ‘d
F
g
pH
10, 6
0% E
tOH
, E
.,, 5
45,
a,,,
610
nm
20-2
00 n
g/m
l 1 ,
SDH
AQ
Fe
(H),
B
e 24
9 c/
F Z
? p
H
9 1-
9 6,
A,,
490,
&,
610
nm
I ,SD
HA
Q
10-1
00 n
g/m
l M
any
tons
25
0 c/
Ph
90%
EtO
H,
8 x
IW’M
N
H,,
I 51
0 nm
0
25-2
00
p&/m
l 0,
1,2,
7TH
AQ
M
any
fan
s 25
1 c/
Ph
40%
E
tOH
, 4
x 10
s3M
NaO
H,
l-6
fig/
ml
Man
y Io
ns
252
em
L 5
40 n
m
e
lH-2
CA
Q
c/Ph
90
%
EtO
H,
0 04
M N
H,,
1 53
0 nm
9-
45 j
fgfm
l M
n, Z
n, C
o, C
a 25
3 $
Mn(
I1)
B
i: A
hzan
n C
ompl
exan
c/
Ph
pH
11 I
-116
,157
Onm
l-
8 @
g/m
l 9
Ant
hrap
urpu
rm
Com
plex
an
254
E
c/Ph
pH
11
4-ll8
,n55
Onm
l-
-7 ,
ug/m
l %
4,
g-D
A-l
,SD
HA
Q-2
,6D
S 25
5 0
016M
NaO
H,
0 16
M H
CI,
i!
k/
Ph
1518
or
560
nm
3-
11 j
4g
Oxd
n ,
redn
an
d co
mpl
exm
g ag
ent
k/F
135
L,
525,
&,,
585
nm
0 16
-O 5
4 /~
g 9
Mo
(V1)
2 <
1,2D
HA
Q-3
S
c/Ph
pH
5,
I
525
nm,
extn
w
ith
0 2-
6 5
jig/m
l F-
an
d E
DT
A
adde
d to
25
6 A
4
I,2-
d~hl
oroe
than
e I,
2,5,
8TT
HA
Q
c/Ph
m
ask
Co,
Z
n, C
u, T
h, U
(W)
pH
5, i
54
0 nm
l-
10
yg/m
l uo
:+
Car
mnu
c ac
id
257
c/Ph
pH
4-5
, /,
336
nm
4-11
fig
/ml
258
1 56
5 nm
I
5-8
fig/
ml
c/F
pH
5 2,
E,,
560,
&,,
590
nm
0
1-O
9 p
g/m
l Pr
evto
us
sepa
ratio
n IS
reco
mm
ende
d 2.
59
Nb(
V)
I ,2D
HA
Q-3
S c/
Ph
2M H
?SO
,, A
cn 49
9, A
,,,, 5
62 n
m,
~32
erg
260
hexa
decy
ltr~m
ethy
lam
mon
lum
br
omtd
e,
stan
dmg
time
2 hr
Ni(
II)
I .2,
4TH
AQ
c/
‘Ph
pH 8
5,
A 5
25 n
m,
extn
m
to
MIR
K
o-25
pg
M
any
ions
1,
2,4T
HA
Q-3
S 26
1 ej
Ph
pH
8
1, A
520
nm
O-3
pgi
ml
co
205
Tab
le
I-ro
ntm
ued
Ion
Rea
gent
Ty
pe
o
f In
terf
eren
ces,
ii
met
hod
Con
dltlo
ns
Ran
ge
rem
arks
R
efer
ence
Nl(I
1)
I H-Z
CA
Q
Abz
ann
Com
olex
an
+ L
a c/
Ph
50%
EtO
H,
8 x
10-‘
M
NN
, e/
Ph
DH 45. ,? 5%
nm
2 66
6
fig/
ml
O-1
0-5&
4 Se
vera
l 10
ns
Co.
Cu.
Zn.
Th.
Ce.
Fe
262
263
PdfI
I)
1,2D
HA
Q-3
S 1,
2,4T
HA
Q-J
C
1,5D
AA
Q-2
,6D
S 4,
8DA
-I ,
5DH
AQ
-2,6
DS
I A
DA
-SN
AQ
C
arm
mlc
ac
id
1.2D
~~ph
e~yl
hydr
azon
e
c/Ph
c/
Ph
c/Ph
c/
Ph
c/P
h
c/F
c/Ph
pH 4
, I
450
nm
04-1
1 /I
g/m
l 26
4 80
% E
tOH
, 16
70
nm
0 30
-2 4
0 @
g/m
l M
any
ions
26
5 pH
2
5, A
6.5
0 nm
4-
20 p
g/m
l M
any
Ions
pH
10
5,
1 72
0 nm
4
8-18
2 I
;cg/
ml
ii:
0 64
M
NaO
H,
I 64
0 nm
2-
10 p
g/m
l St
abrh
zed
with
po
ly(v
my1
alc
ohol
) 26
8 pH
5 3
, ac
eton
e,
2,
$46,
&,,
580
nm
0 1-
1 pg
In
terf
eren
ces
rem
oved
by
ppt
n of
Pd
269
0 4M
NH
3, A
675
nm
0
5-2
&m
l 27
0
Rh(
II1)
1,
2DH
AQ
-3S
c/Ph
pH
4,1
45O
nm
, he
at
at
100”
for
1 5
hr
1 5-
8 6
pg/m
l Pd
, C
u, R
u 27
1
I ,5D
HA
Q-2
,6D
S 1,
4DH
AQ
1,2,
7TH
AQ
pH35
-51,
149S
nm
0 3-
4 rg
/ml
272
0 02
M N
aOH
, a,
, 54
5, J
., 60
0 nm
, 3-
4 @
g O
nly
Be
Inte
rfer
es
seno
usly
72
lO
-2 M
B-c
yclo
dext
rm
?Y
DM
F,
&
48.5
, &,,
563
nm
12-2
25 n
g/m
l 62
8 ”
sefW
4
5DA
-1 ,S
DH
AQ
c/
Ph
99 W
OO
%
H2S
04,
2 61
0 nm
O
-4 3
&m
l 87
;; gr
he
at
at 9
0” f
or 2
1 hr
$
Sr(I
1)
3A- 1
,2D
HA
Q i
- eo
sm
Altz
arm
C
ompl
exan
tc/P
h pH
65-7
2,iW
nm
0 14
-2 0
fig
/ml
Al,
CN
- A
dd
ED
TA
to
mas
k A
l 27
3
M
cjPh
pH
10
9, I
610
nm
2-12
pg/
ml
Man
y so
ns
274
-wlV
f
T@
V)
Tl(
II1)
1,2D
HA
Q-3
S 1,
2,7T
HA
Q
1,2,
5,8T
TH
AQ
1,
2,3,
5,6,
7HH
AQ
4,
8DA
- I ,
5DH
AQ
-2,6
DS
BM
AnA
Q
3A-1
,2D
HA
Q
+ S
-sul
phos
ahcy
hc
acid
1,2D
HA
Q-3
S 1,
2DH
AQ
-3S
1,4D
A-2
,3D
HyA
Q
c/Ph
c/
Ph
c/Ph
c/
Ph
c/Ph
c/‘P
h tc
/Ph
c/Ph
c/
Ph
k/F
rx
jF
pH
3 2-
-8
0 23
-16
7 pg
/ml
256
EtO
H,
I 54
0 nm
, st
andm
g tim
e 2
hr
7-21
p&
/ml
275
1 57
0 nm
25
-250
/ig
27
6 1
530
nm,
lOM
HC
I 5-
12 j
ig/m
l 27
7 pH
3 5
, ,l
68.5
nm
7 5-
22 5
jig
/m!
As,
Au,
Al,
Fe,
Cr,
Zn
278
UO
g*,
Ba
F-
pH 4
6,4
0%
DM
F,
I 62
0 nm
4
7-18
5 k
g/m
1 27
9 pH
4 6
-S 5
, 1
580
nm,
20%
EtO
H
60-5
60 /
_tg
CN
-,
NO
;, H
PO
;- ,
F-
70
i, 66
0 nm
10
-100
/Ig
28
0 p
H
3 5,
/
51.5
nm
, st
andi
ng
time
1.5 m
m
~24
/rg
260
hexa
de~y
ltr~m
ethy
lam
mon
~um
br
omid
e
pH
3 4,
J.,,
400
, ie
m 4
70 n
m
0 05
-O 4
jfg
jml
Au,
F
e, C
e 13
7 pH
3
6, s
tand
mg
90 m
m
0 l-
3 #g
/ml
Au,
Fe,
Ce,
V
141
;!
r T
m(l
l~)/
Nd(
Il~)
IP
DH
AQ
c/
F M
eOH
, pH
4 5
, i
557
nm f
or N
d 0
4-12
0 #g
/ml
Tm
T
m
Nd
tole
ranc
e 73
I
559
nm f
or T
m
0 4-
l 20
pg/
ml
Nd
from
2
5 1
to 1
2 5
Wi)
I ,
2DH
AQ
-3S
c/Pb
pH
4 5
-5 5
, L
550
nm
40
-250
p&
ml
Cl-
, N
O,,
SO;-
28
1 1,
4DH
AQ
-3S
c/P
h
I 55
0-59
0 nm
50
fig
C
e an
d T
h m
ust
be a
bsen
t 28
2 1,
2,5,
8TT
HA
Q
c/Ph
pH
5
5,L
63
0660
nm
3
5-21
p&
ml
MO
and
ot
hers
25
7, 2
83
V(V
) 1,
2DH
AQ
-3S
C/P
h pH
35_5
8,R
455n
m
0 l-
3 67
/@
/ml
Var
ious
io
ns
284
iA4H
AQ
k/
F 0
Ski
HC
I, 1
,480
, ;I
, 57
5 nm
0
l-o
5 fi
g/m
l C
e 13
6 1,
4DA
-SN
AQ
c/
F 2M
HC
I, ;
len 4
75,
E.,
550
nm
100-
800
ng/m
l 93
4,
8DA
- 1,
5DH
AQ
-2,6
DS
k/F
04M
H
Cl,
A,,
524,
&,,
582
nm
0 04
-a 5
lrg
/ml
Ce,
Fe,
I-
122
4,8D
A-1
,5D
HA
Q-2
,6D
S k/
F 0
4M H
Cl,
il,
524,
&,,,
582
nm
l-
10
ng/m
l C
e, F
e(B
),
I-
130
5 ue
fml
Fe(I
II1
1,2D
HA
Q-3
S
I ,2D
HA
Q-3
S
Car
mnu
c ac
td
c/Ph
C
/F
c/Ph
c/F
pH
3 5-
5 8,
147O
nm
pH
48-
62
pH 4
, L
483
at
30”
, nm
, he
xad~
yltn
met
hyla
mm
on~u
m
pH 4
6,
,$,,
515,
rZ
, 58
5 nm
0 4-
13 3
jig
/ml
Man
y Io
ns
285
0 5-
4 fi
g/m
l A
l m
ust
be a
bsen
t <
: 10
pg/m
l 28
6
0 04
-O 3
6 p&
/ml
Prev
ious
se
para
tton
IS re
com
men
ded
259
Y(I
I1)
w
c/Ph
pH
7 7
,40%
D
MF
7 12
-28
5 pg
/ml
60
Zn(
II)
Zr(
IV)
Ahz
ann
Com
plex
an
I A4H
AQ
4,
8DA
-1 ,S
DH
AQ
-2,6
DS
c/Ph
c/Ph
c/
Ph
pH 4
3,
d 50
0 nm
, st
andi
ng
ttme
30 m
m
0 13
-O 5
pg/
mI
287
pH35
,16W
nm
24-l
13
pg
lnte
rfer
ents
m
aske
d w
tth C
N-
288
0 17
M H
CI,
J. 7
00 n
m
20-2
00 p
g PO
:-,
F-,
BrQ
;, H
,PQ
;, 28
9 E
DT
A,
Fe,
C,C
@
l,ZD
HA
Q-F
- tc
/Ph
pH 8
9,1
556
nm,
MB
K
<20
iu
g In
terf
eren
ts
mas
ked
wtth
ED
TA
29
0 1,
2DH
AQ
-3S
c/
Ph
0 1M
HC
I, A
510
nm
01
-03m
g 75
, 97
c/
Ph
O-8
0 m
g/l
ZrQ
, 24
0 I ,
2,4-
TH
AQ
-3S
c/Ph
pH
O75
_093
,160
9nm
n-
7 lr
glm
l 20
7 1,
2,3,
5,6,
7HH
AQ
c,
!Ph
IM
HC
I, d
560
nm
3-
9 pg
/ml
220
Abb
revt
atto
ns
used
A
liza
rin
Com
plex
an,
[(3,
4-dl
hydr
oxy-
2-an
thra
quln
olyl
)met
hyl]
lmln
odla
cetlc
ac
td,
Ant
hrap
urpu
rin
Com
plex
an,
[(1,
2,7-
trth
ydro
xy-3
-ant
hraq
umyl
)met
hyl]
tmm
o-
dtac
etrc
acr
d, 3
A-1
,2R
HA
Q,
3-am
ino-
1,2-
dihy
drox
yant
hraq
uIno
ne,
lA-4
HA
Q,
I-am
ino-
~hyd
roxy
anth
raqu
lnon
e,
BM
AnA
Q,
I,~B
~~~m
ethy
lanl
Ilno
)ant
hraq
utno
ne,
e, c
ompl
ex
form
atto
n,
Car
min
ic a
cid,
7-a
-a-g
luco
pyra
nosy
l-3,
5,6&
tetr
ahyd
roxy
- I-
met
hyla
nthr
aqum
one-
2-ca
rbox
yhc
actd
, 1,
2DA
AQ
, 1,2
-dta
mm
oant
hraq
umon
e,
1,2D
AA
Q-p
heny
kyd
razo
w,
1,2-
d~am
lnoa
nthr
aqul
none
ph
enyl
hydr
azon
e,
1,2D
AA
Q-3
%
1,2-
d~am
inoa
nthr
aqu~
none
-3-~
ulph
on~c
ac
td,
1,4D
AA
Q2,
3DS,
l,~
dlam
inoa
nthr
aq~l
none
-2,3
-dls
ulph
onlc
ac
td,
1,5D
AA
Q_2
,6D
S,
1,5-
dtam
moa
nthr
aqum
one-
2,6-
dtsu
lpho
mc
acid
, 1,
4DA
-2,3
DH
yAQ
, I ,
4-dt
amm
o-2,
3-dt
hydr
oant
hraq
umon
e,
1,8D
A-&
SDH
AQ
, I,8
dtam
tno-
4,5-
dthy
drox
y-
anth
raqu
Inon
e,
4,8D
A-l
,5D
HA
Q-2
,6D
~,
4.8-
dtam
mo-
i,5-d
~hyd
roxy
anth
raqu
mon
e-2,
6-d~
sulp
hon~
~ ac
td,
1,4D
A-S
NA
Q,
1,4-
diam
lno-
5-nl
troa
nthr
aqui
none
, df
, d~
~ere
ntla
l m
etho
d,
1,2D
HA
Q,
1,2d
lhyd
roxy
anth
raqu
lnon
e,
1,4D
HA
Q-2
,6D
S,
l.~!h
ydro
xyan
thra
quin
one-
2,6-
d~su
lpho
ntc
acid
, 1,
2DH
AQ
GS
, 1,
2-dl
hydr
oxya
nthr
aqui
none
-3-s
ulpb
onlc
an
d,
1,4D
HA
Q-2
S,
I ,4-
drhy
drox
yant
hraq
umon
e-2-
sulp
hom
c ac
td,
1,5D
H-4
,8 D
AA
Q,
I ,5-
dthy
drox
y4,8
_dta
mm
oant
hraq
mno
ne,
DPh
G,
drph
enyl
guam
dmru
m,
F, f
luon
met
nc
met
hod,
IH
-ZC
AQ
, I-
hydr
oxy-
2car
boxy
anth
raqu
mon
e,
1,2,
3,5,
6,7H
HA
Q, 1
,2,3
.5,6
-hex
ahyd
roxy
anth
raqu
mon
e,
ic, m
dtre
ct m
etho
d,
k, k
met
tc m
etho
d,
Ph,
phot
omet
rrc
met
hod,
Ph
QrD
S,
2-ph
enox
yqui
n~za
~n-3
,4-d
~sul
phon
~c
acid
, Q
G,
1,4-
bls-
(~-s
ulph
o-4-
met
hyla
nll~
no)a
nthr
aqul
none
, Q
uina
lizar
in,
1,4,
5,8t
etra
hydr
oxya
nthr
aqm
none
, T
X, re
dox
reac
tron
, tc
, te
rnar
y co
mpl
ex.
1,2,
3TH
AQ
, 1,
2,3-
t~hy
drox
yant
hraq
uin~
ne,
1,2,
4TH
AQ
-2C
, 1,
2,4-
trlh
ydro
xy-2
~arb
oxya
nthr
aqut
none
, I,
2,4T
?iA
Q-3
S,
1,2,
4-tr
lhyd
roxy
anth
raqu
inon
e-3-
sulp
honl
c ac
id,
1,2,
5$T
’lM
AQ
, 1,
2,5,
8~et
rahy
drox
yant
hraq
urno
ne
584 AURORA NAVM DIAZ
ally having a much more pronounced effect than one m the 2-position.‘q4
In the absence of a hydrogen donor, photo- excited AQs can undergo photoreduction by the abstraction of an electron. Aminoanthra- qumones that are relatively unreactive towards hydrogen-atom abstraction, because of the C-T character of the lowest excited state, can undergo photoreduction by electron transfeP2 from hydroxide ions m solutions of high pH.
The photochemistry of anthraquinone-Zsul- phonate and anthraqumone-2,6-disulphonate has received much attention2” and various re- action mechanisms have been proposed. These photoreactions have been used in ltqutd chro- matography to detect compounds’66-168 that do not absorb ultraviolet-visible radiation at all. An anthraqumone-sensitized photo-oxygen- ation reaction produces hydrogen peroxide during the oxidation of the analytes (alcohols, aldehydes, ethers and saccharides) by hydrogen- atom abstraction Once formed, the hydrogen peroxide is measured by a chemilummescence reaction. The photoreduction of anthraquinone- 2,6-disulphonate to dihydroxyanthracene-2,6- disulphonate has been used for the determmation of several herbicides.“’
Anthraqumone-2-sulphonates which have been reduced photochemically can serve as elec- tron donors, and thus can behave as sensitizers of the reduction of electron acceptors.13
Another aspect of the photochemistry of anthraqumones is concerned with the gener- ation of singlet oxygen. Energy transfer between the triplet state of a dye and molecular oxygen occurs as follows
sens* + 302(3Z) + sens + ‘02(‘A)
Anthraqumones which posses relatively long- lived triplet states are likely candidates as sensi- tizers for the formation of singlet oxygen. 1-Ammo-4-hydroxyanthraqumone and its 2- methoxy derivative are extremely efficient sensi- tizers of singlet oxygen production. Seven of the components of the dye C I. Disperse Blue 35 are efficient producers of singlet oxygen under the influence of light, the most photoactive component being 1 &diammo-4,5dihydroxy- anthraqumone.4
CONCLUSION
The anthraqumones are very versatile re- agents A summary of their prmctpal analytical applications is given m Table 1.
Acknowledgement-The Comtston Asesora de Investtgacton Ctenttfica y Tbmca IS thanked for supportmg thts study (kOJC!Ct 3007/83 CO24l2)
5
6
7
8
9 10 11 12
13
14 15 16
17 18
19
20
21
22
23
24
25
26 27
28
29
30
31 32
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