lecture 9
DESCRIPTION
Lecture 9. Acid-Base Equilibria -I. We titrate with strong acids ONLY!. Strong acids:. HCl HBr HI HNO 3 H 2 SO 4 HClO 4. (HO) n E=O. (HO) n EO 2. Weak acid. Strong acid. _. Concentrations below 10 -8 M do not affect the pH value. - PowerPoint PPT PresentationTRANSCRIPT
Lecture 9
Acid-Base Equilibria -I
Strong acids:
HCl HBr HIHNO3 H2SO4 HClO4
O NO
OH ClO O
O
HO
(HO)nE=O
Weak acid
(HO)nEO2
Strong acid
S
O
O
OH
HO
We titrate with strong acids ONLY!
O NO
OH
O NO
O
_
Concentrations below 10-8 Mdo not affect the pH value
10-6 -10-8 require specialtreatment (in practice, this will be still affected mostly by CO2 and NH3 from air)
Only concentrationsabove 10-6 M may changethe pH value – and only inabsence of other acids or bases
Conclusion: we cannottitrate low concentrationsof acids or bases in water
Weak acids and bases:
Ka is a small number (<< 1)
][
]][[
HA
AHKa
NHH
H + H+N+
HH
H
H
NHH
H + H2O N+
HH
H
H
+ OH-
acid base
base acid
][
]][[
HA
AHKa
][
]][[
A
OHHAKb
HA A + H+
A + H2O HA + OH-
HA A + H+
A + H2O HA + OH-+
H2O H+ + OH-
KaKb =
][
]][[
][
]][[
A
OHHA
HA
AH
= [H+][OH-]
pH value of weak acid solution (C> 10-3 M)
The main source of H+ is HA, not H2OHA A + H+
[A] = [H+]
][
]][[
HA
AHKa
[HA] = C - [H+]
A small number
C
HHKa
]][[
[H+]2 = KaC
CKH a ][
)][(][ HCKH aCheck the resulting [H+] and correct if necessary
Any acid is “strong” at very low concentration – but it does notchange the pH!
pH value of weak base solution (C> 10-3 M)
The main source of OH- is A, not H2O
[HA] = [OH-]
][
]][[
A
HAOHKb
[A] = C - [OH-]
A small number
C
OHOHKb
]][[
[OH-]2 = KbC
CKOH b ][
)][(][ OHCKOH bCheck the resulting [OH-] and correct if necessary
A + H2O HA + OH-
KaKb =[H+][OH-]=10-14
pH value of mixture of a weak base and weak acid (C> 10-3 M)
NHH
H + H+N+
HH
H
H
HA A + H+
][
]][[
HA
AHKa
][
][][
A
HAKH aAt high concentrations,
[A]=CA and [HA]=CHA
A
HAa C
CKH ][
acid
basea C
CpKpH log
pH value of mixture of a weak base and weak acid (C> 10-3 M)
A
HAa C
CKH ][
acid
basea C
CpKpH log
buffer - pH does not change when you varyconcentration a little
In practice, one buffer pair (acid+ conjugate base) determines thepH value of the whole multicomponent mixture
acid
basea C
CpKpH log
A complex mixture:
NHH
H + H+N+
HH
H
H
0.1 M 0.1 M
Harris, p. AP12
pKa=9.24
pH= 9.24
][
][log
HA
ApKpH a
All other species in the system(indicator, any admixtures, …)will follow the pH determinedby the buffer
Enzyme activity as a functionof pH
Effect of [A]/[HA] on pH or
Effect of pH on [A]/[HA]
)(
)(
)(
)(_
pHd
Cd
pHd
CdcapacityBuffer AB
pK=5
pH calculations: pH = -log[H+]
KaKb =[H+][OH-]=10-14
K>1 Strong acid or strong base
[H+]=Cacid [OH-]=Cbase
K<<1 Weak acid or weak base
CKOH b ][CKH a ][
A mixture of a weak base and weak acid
acid
basea C
CpKpH log