topics 1.h + 2.acids and bases 3.definition of ph 4.reversible reactions, equilibrium, mas action...
TRANSCRIPT
Topics
1. H+
2. Acids and Bases3. Definition of pH4. Reversible reactions, equilibrium, mas action5. HendersonpHasselbalch equation6. Buffers. Buffer capacity
H+
Suppose chloride acid dissolved in water
HCl H+ + Cl-
The entity H+, hydrogen stripped from the electron, is simply a proton, without electronic cloud, with dimensions at least 4 orders smaller than a real atom. Its strong electrical field Impedes a free existence. What really happens, upon dissolution of HCl in water is:
HCl + H2O H3O+ + Cl-
H3O+ H2O + H+
HCl H++ Cl-
[H+]
Acids and Bases
BrΓΈnsted-Lewy Concept (1923)AcidHA H+ + A-
BaseB- + H+ BH
Arrhenius Concept (1890) AcidHA H+ + A-
BaseCOH C+ + OH-
Acid + base salt + water 2NaOH + H2SO4 Na2SO4 + 2H2O
Water has amphoteric character2H2O H3O- + H+
pH, reversible reaction, equilibrium, mass action
ππ»=β πππ10ΒΏpH
Reversible Reactions β Rate constants - Equilibrium
BA B + AK1
k-1
π1 [π΅π΄ ]=πβ 1 ( [π΅ ] [ π΄ ] )
Henderson-Hasselbalch equation
HCl H+ + Cl-K1
k-1
At equilibrium
π1πβ 1
=ΒΏ
βπππΒΏ
π1πβ 1
=πΎ
ππ»=ππΎ +πππ[πΆπβ]
[ π»πΆπ ]
Buffers and Buffer capacity
π½=πππ
πππ»=2.3ΒΏ
In a given pH, Ξ² is a function of pH and buffer concentration
Bibliography
β’ Bockris, J.OβM and Reddy, A.K.N.: Modern Electrochemistry. Plenum Press, 1970. Vol.1, 1970. Chap. 5. Protons in solution.
Questions
1. For a [H+] of 10-10M to 10-1M, in steps fo 10-3M, draw a plot of pH x [H+].
2. Consider 1 L of a solution of a buffer of pK=7.5 amd concentration of 10 mM. Starting with a buffer base concentration of 9,9 mM, add progressively a strong acid, in amounts of 0.05 mmol. At equilibrium draw the curve relating pH to the total amount of acid added. Where is the point of maximal buffering power?
3. Suppose a buffer if pK=7.0 in concentration of 5 mM. What are the concentrations of acid and base for buffering a solution at a pH of 6,0.
Medidas de pH
I. EletrΓ³diosII. Indicadores fluorescentes
BibliografiaKoryta, J.: Ion-Selective Electrodes. 1974. Cambridge University Press.Vanysek, P.> The glass pH electrode.The Electrochemical Society Interface. 2004Lakowicz, J.R.: Principles of fluorescence spectroscopy. 2nd ed., 1999. Fluwer Academy/Plenum Press
Electrochemical potential of a solute in a phase β Macroscopic view
Thermal energy T (K)
C1
1
C2
ΓΈ2
M
C: concentration, mol/lΓ: Electrical potential, V
~ππ (1 )=ππβ
βπ (1 )+π πππππ (1 )+π§ ππΉ β (1)
R= 8.3 J mol-1 K-1
β~ππ β= π½ πππβ1
πΉ=π π΄πβ=1,6022Γ104Γ6.03Γ1023
πΉ=9.6485Γ104πππ’ππππβ 1
~ππ (2 )=ππβ
βπ (2 )+π ππππ π (2 )+π§π πΉβ (2)
β~ππ=π ππππ π (1 )π π (2 ) π
+π§π πΉ (β (1)β β (2))
Campos elΓ©tricos β forΓ§as elΓ©tricas
ForΓ§a elΓ©trica β lei de Coulomb
q
WV
dx
dV
q
f
Campo elΓ©trico
Diferença de potencial elétrico
+-
+
-
221*
r
qqkf
Carga do e- 1,60*10-19 coul
Constante de Faraday
F=NA*e-=
96484 coul/mol
C1
1
C2
ΓΈ2
M
Membrane (M) Properties
1. Impermeable membrane
2. Membrane permeable to solutes
=0
3. Membrane permeable to cations or to anions
=0
ββ =β π ππ§π πΉ
lnππ (1 )ππ (2 )
Ion Exchangers β Glass Electrodes
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H+
H+
H+
H+
H+
H+H+
H+
H+
H+
H+
H+
H+
H+
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H+
H+
ππ€πππ /π πππ’π‘πππ=π ππΉ2.303 πππΒΏ
π πΈππππ‘ππππ=π β²+π ππΉ2.303 (ππ» )