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Class average for Exam I
70
Fe(OH)3Fe3+
(aq) + 3 OH-(aq)
[Fe3+][OH-]3 = 1.1 x 10-36
[y][3y]3 = 1.1 x 10-36
If there is another source of OH- (NaOH)
that provides a higher [OH-] then that is
the value of [OH-] to be used.
pH and solubility
CaCO3(s) + H3O+(aq) Ca2+
(aq) + HCO3-(aq)
+ H2O(l)
CaCO3(s) + H3O+(aq) Ca2+
(aq) + HCO3-(aq)
+ H2O(l)
Net ionic equation.
CaCO3(s) + H3O+(aq) Ca2+
(aq) + HCO3-(aq)
+ H2O(l)
CaCO3 calcium carbonate, present in
both limestone and marble.
CaCO3(s) + H3O+(aq) Ca2+
(aq) + HCO3-(aq)
+ H2O(l)
CaCO3(s) + H2O(l) Ca2+(aq) + CO3
2-(aq)
CaCO3(s) + H3O+(aq) Ca2+
(aq) + HCO3-(aq)
+ H2O(l)
CaCO3(s) + H2O(l) Ca2+(aq) + CO3
2-(aq)
CO32-(aq) + H3O+(aq) H2O(l) +
HCO3-(aq)
Ksp = [Ca2+][CO32-]
CaCO3(s) + H3O+(aq) Ca2+
(aq) + HCO3-(aq)
+ H2O(l)
CaCO3(s) + H2O(l) Ca2+(aq) + CO3
2-(aq)
CO32-(aq) + H3O+(aq) H2O(l) +
HCO3-(aq)
Any reaction favoring the formation of HCO3-
favors the solution of a solid carbonate .
Ksp = [Ca2+][CO32-]
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
Increase solubility of Zn(OH)2 by
lowering pH.
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
Increase solubility of Zn(OH)2 by
lowering pH.
Removal of product, OH-, shifts equilibriumto right.
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 7
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 7
[Zn2+] = y
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 7
[Zn2+] = y
(y)(2y)2 = Ksp
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 7
[Zn2+] = y
(y)(2y)2 = Ksp = 4y3 = 4.5 x 10-17
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 7
[Zn2+] = y
(y)(2y)2 = Ksp = 4y3 = 4.5 x 10-17
[Zn2+] = 2.2 x 10-6 M [OH-] = 4.4 x 10-6 M
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 6
[Zn2+] = y
buffered
pH = 6, [H3O+] = 10-6
[OH-] = Kw
[H3O+]
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = ? @ pH = 6
[Zn2+] = y
buffered
pH = 6, [H3O+] = 10-6
[OH-] = Kw
[H3O+]=
1 x 10-14
10-6= 10-8
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[OH-] = 1 x 10-8
(y)(1 x 10-8)2 = 4.5 x 10-17
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[OH-] = 1 x 10-8
(y)(1 x 10-8)2 = 4.5 x 10-17
y = 4.5 x 10-17
1 x 10-16
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[OH-] = 1 x 10-8
(y)(1 x 10-8)2 = 4.5 x 10-17
y = 4.5 x 10-17
1 x 10-16= 4.5 x 10-1
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[OH-] = 1 x 10-8
(y)(1 x 10-8)2 = 4.5 x 10-17
y = 4.5 x 10-17
1 x 10-16= 4.5 x 10-1
[Zn2+] = 0.45 M
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = 0.45 MpH = 6
pH = 7 [Zn2+] = 0.0000022 M
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = 0.45 MpH = 6
pH = 7 [Zn2+] = 0.0000022 M
[OH-] = 2[Zn2+]
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = 0.45 MpH = 6
pH = 7 [Zn2+] = 0.0000022 M
[OH-] = 2[Zn2+] = 4.4 x 10-6 M
Zn(OH)2(s) Zn2+(aq) + 2 OH-
(aq)
[Zn2+][OH-]2 = Ksp = 4.5 x 10-17
[Zn2+] = 0.45 MpH = 6
pH = 8.6 [Zn2+] = 0.0000022 M
[OH-] = 2[Zn2+] = 4.4 x 10-6 M
Solubility of salts of
weak acids
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
Reduce pH, increase [H3O+]
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
Reduce pH, increase [H3O+]
Increase [H3O+] : equilibrium
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
NaA(s) Na+(aq) + A-
(aq)
conjugatebase
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
NaA(s) Na+(aq) + A-
(aq)
A-(aq) + H3O+
(aq) HA(aq) + H2O(l)
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
NaA(s) Na+(aq) + A-
(aq)
A-(aq) + H3O+
(aq) HA(aq) + H2O(l)
Reduce pH, increase [H3O+]
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
NaA(s) Na+(aq) + A-
(aq)
A-(aq) + H3O+
(aq) HA(aq) + H2O(l)
Reduce pH, increase [H3O+], reduce [A-]
Solubility of salts of
weak acids
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
NaA(s) Na+(aq) + A-
(aq)
A-(aq) + H3O+
(aq) HA(aq) + H2O(l)
Reduce pH, increase [H3O+], reduce [A-], increase [Na+]
Using common ions to separate
mixtures of ions.
Using common ions to separate
mixtures of ions.
Separating ions which share a
group is difficult - they have
very similar chemistries.
Using common ions to separate
mixtures of ions.
I II VII
Na+ Ca2+ Cl-
K+ Ba2+ I-
M1X M1+ + X-
M2X M2+ + X-
M1X M1+ + X-
M2X M2+ + X-
If the solution is not saturated for
either M1X or M2X, there will
be no solid present.
M1X M1+ + X-
M2X M2+ + X-
As [X-] is increased, at some point
precipitation will occur.
M1X M1+ + X-
M2X M2+ + X-
If Ksp for M1X and Ksp for M2X
differ by a large enough amount,
one will precipitate and the other
will remain in solution.
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Q < Ksp no precipitate
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Q = [Ba2+][F-]2 < 1.7 x 10-6
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Q = [Ba2+][F-]2 < 1.7 x 10-6
Q < Ksp no precipitate
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Q = [Ba2+][F-]2 < 1.7 x 10-6
Q < Ksp no precipitate
Q = [Ca2+][F-]2 > 3.9 x 10-11
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Q = [Ba2+][F-]2 < 1.7 x 10-6
Q < Ksp no precipitate
Q = [Ca2+][F-]2 > 3.9 x 10-11
Q > Ksp precipitate
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Q = [Ba2+][F-]2 < 1.7 x 10-6
Q < Ksp no precipitate
Q = [Ca2+][F-]2 > 3.9 x 10-11
Q > Ksp precipitate
Adjust [F-]so maximumCa2+ precipitateswith no Ba2+
precipitate.
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Q < Ksp no precipitate
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Q < Ksp no precipitate
[F-]2 < 1.7 x 10-6
[Ba2+]
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Q < Ksp no precipitate
[F-]2 < 1.7 x 10-6
[Ba2+]=
1.7 x 10-6
0.10
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Q < Ksp no precipitate
[F-]2 < 1.7 x 10-6
[Ba2+]=
1.7 x 10-6
0.10= 1.7 x 10-5
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Q < Ksp no precipitate
[F-]2 < 1.7 x 10-6
[Ba2+]=
1.7 x 10-6
0.10= 1.7 x 10-5
[F-] < 4.1 x 10-3
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6Ksp (BaF2) = [Ba2+][F-]2 = 1.7 x 10-6
Q < Ksp no precipitate
[F-]2 < 1.7 x 10-6
[Ba2+]=
1.7 x 10-6
0.10= 1.7 x 10-5
[F-] < 4.1 x 10-3 All Ba2+ remains in solution.
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (CaF2) = [Ca2+][F-]2 = 3.9 x 10-11
Q > Ksp precipitate
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
[Ba2+] = [Ca2+] = 0.10 M
Ksp (CaF2) = [Ca2+][F-]2 = 3.9 x 10-11
Q > Ksp precipitate
[F-]2 > 3.9 x 10-11
0.10
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
Ksp (CaF2) = [Ca2+][F-]2 = 3.9 x 10-11
Q > Ksp precipitate
[F-]2 > 3.9 x 10-11
0.10= 3.9 x 10-10
[F-] > 2.0 x 10-5 CaF2(s) starts toprecipitate
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
[F-] > 2.0 x 10-5 CaF2(s) starts toprecipitate
[F-] < 4.1 x 10-3 All Ba2+ remains in solution.
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
[F-] > 2.0 x 10-5 CaF2(s) starts toprecipitate
[F-] < 4.1 x 10-3 All Ba2+ remains in solution.
How to reduce [Ca2+] to as low a levelas possible without BaF2 precipitation?
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
[F-] < 4.1 x 10-3 All Ba2+ remains in solution.
Adjust [F-] to 0.0041 M
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
[F-] < 4.1 x 10-3 All Ba2+ remains in solution.
Adjust [F-] to 0.0041 M
How much Ca2+ remains in solution?
CaF2(s) Ca2+(aq) + 2 F-
(aq)
BaF2(s) Ba2+(aq) + 2 F-
(aq)
CaF2(s) Ca2+(aq) + 2 F-
(aq)
Adjust [F-] to 0.0041 M
Ksp = [Ca2+][F-]2 = 3.9 x 10-11
[Ca2+] =3.9 x 10-11
[F-]2
CaF2(s) Ca2+(aq) + 2 F-
(aq)
Adjust [F-] to 0.0041 M
Ksp = [Ca2+][F-]2 = 3.9 x 10-11
[F-]2=
3.9 x 10-113.9 x 10-11
(4.1 x 10-3)2
2.3 x 10-6[Ca2+] =
[Ca2+] =
Adjust [F-] to 0.0041 M
0.10 M CaF2(s) Ca2+(aq) + 2 F-
(aq)
0.10 M BaF2(s) Ba2+(aq) + 2 F-
(aq)
[Ba2+] = 1.7 x 10-6
(4.1 x 10-3)2= 0.10 M
2.3 x 10-6[Ca2+] =
CaF2 Ksp = 3.9 x 10-11
BaF2 Ksp = 1.7 x 10-6
Metal sulfides in acidic solution
MS M2+(aq) + S2-
(aq)
Ksp = [M2+][S2-]
Metal sulfides in acidic solution
MS M2+(aq) + S2-
(aq)
Ksp = [M2+][S2-]
S2- Is a strong base
Metal sulfides in acidic solution
MS M2+(aq) + S2-
(aq)
Ksp = [M2+][S2-]
S2- Is a strong base
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Kb =[HS-][OH-]
[S2-]
Metal sulfides in acidic solution
MS M2+(aq) + S2-
(aq)
Ksp = [M2+][S2-]
S2- Is a strong base
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Kb =[HS-][OH-]
[S2-] 105
Metal sulfides in acidic solution
MS M2+(aq) + S2-
(aq)
Ksp = [M2+][S2-]
S2- Is a strong base
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Kb =[HS-][OH-]
[S2-] 105
Ksp = [M2+][HS-][OH-]
Metal sulfides in acidic solution
MS M2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [M2+][HS-][OH-]
Lower pH, lower [OH-], higher [M2+]
Ksp metal sulfides < 10-10
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Buffer solution to pH = 2
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Buffer solution to pH = 2
[H3O+] = 1 x 10-2
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Buffer solution to pH = 2
[H3O+] = 1 x 10-2 [OH-] =1 x 10-14
1 x 10-2
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Buffer solution to pH = 2
[OH-] =1 x 10-14
1 x 10-2= 1 x 10-12
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Buffer solution to pH = 2
[OH-] = 1 x 10-12
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
Buffer solution to pH = 2
[OH-] = 1 x 10-12
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-12
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
Ka =[H3O+][HS-]
[H2S]= 9.1 x 10-8
Buffer solution to pH = 2 [H2S] = 0.10 M
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-12
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
Ka =(0.01)[HS-]
(0.10)= 9.1 x 10-8
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-12
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
Ka =(0.01)[HS-]
(0.10)= 9.1 x 10-8
[HS-] = (0.10)(9.1 x 10-8)/(0.01) = 9.1 x 10-7
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-12
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
[HS-] = 9.1 x 10-7
[Cd2+] = (7 x 10-28)/(9.1 x 10-7)(1 x 10-12)
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-12
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
[HS-] = 9.1 x 10-7
[Cd2+] = (7 x 10-28)/(9.1 x 10-7)(1 x 10-12) = 8 x 10-10
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-7
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
Ka =(1 x 10-7)[HS-]
(0.10)= 9.1 x 10-8
[HS-] = (0.1)(9.1 x 10-8)/(1 x 10-7) = 9.1 x 10-2
pH = 7
Metal sulfides in acidic solution
CdS(s) Cd2+(aq) + S2-
(aq)
S-2(aq) + H2O(l) HS-
(aq) + OH-(aq)
Ksp = [Cd2+][HS-][OH-] = 7 x 10-28
[OH-] = 1 x 10-7
H2S(aq) + H2O(l) H3O+(aq) + HS-
(aq)
[HS-] = 9.1 x 10-2
[Cd2+] = (7 x 10-28)/(9.1 x 10-2)(1 x 10-7) = 8 x 10-20
Complex ions
Complex ions
Metals coordinated to ligands which
can exist independantly as
molecules or ions.
Ammonia, NH3, and water are
common ligands in complex ions.
Cobalt(II) chloride
Cobalt(II) chloride
CoCl2.6H2O
CoCl2.2H2O
Cobalt(II) chloride
CoCl2.6H2O
[Co(H2O)6]2+ (Cl-)2
CoCl2.2H2O
blue
purple
magenta
2+
[Co(H2O)6]2+
Solubilities of complex ions
Equilibria involving complex ions
may involve multi-step processes
in which individual ligands are
added or removed.
Cobalt(II) chloride
CoCl2.6H2O
[Co(H2O)6]2+ (Cl-)2
CoCl2.2H2O
blue
purple
magenta
These species are quite soluble.
Ag+(aq) + NH3(aq) Ag(NH3)+
Ag+(aq) + NH3(aq) Ag(NH3)+(aq)
[Ag(NH3)+]
[Ag+][NH3]= 2.1 x 103K1 =
[Ag(NH3)+]
[Ag+][NH3]= 2.1 x 103K1 =
Ag(NH3)+(aq) + NH3(aq) Ag(NH3)2
+(aq)
Ag+(aq) + NH3(aq) Ag(NH3)+
(aq)
[Ag(NH3)+]
[Ag+][NH3]= 2.1 x 103K1 =
Ag(NH3)+(aq) + NH3(aq) Ag(NH3)2
+(aq)
Ag+(aq) + NH3(aq) Ag(NH3)+
(aq)
K2 =[Ag(NH3)2
+]
[Ag(NH3)+][NH3]= 8.2 x 103
K1, K2 > 103 - large
K1, K2 > 103 - large
Ag+ in the presence of excess NH3
is converted to 100% Ag(NH3)2+
K1, K2 > 103 - large
Ag+ in the presence of excess NH3
is converted to 100% Ag(NH3)2+.
Add 0.1 M AgNO3 to 1 L of 1 M NH3
K1, K2 > 103 - large
Ag+ in the presence of excess NH3
is converted to 100% Ag(NH3)2+.
Add 0.1 M AgNO3 to 1 L of 1 M NH3
Initial condition: [Ag(NH3)2+] = 0.10 M
[NH3] = 0.80 M
Ag(NH3)2+
( aq) Ag(NH3)+(aq) + NH3(aq)
K = 1
K2[Ag(NH3)2
+]
[Ag(NH3)+] [NH3] =
Init 0.100 M 0 0.80
Ag(NH3)2+
( aq) Ag(NH3)+(aq) + NH3(aq)
K = 1
K2[Ag(NH3)2
+]
[Ag(NH3)+] [NH3] =
Init 0.100 M 0 0.80
-y +y + y
Eq 0.100-y y 0.80 + y
Ag(NH3)2+
( aq) Ag(NH3)+(aq) + NH3(aq)
K = 1
8.2 x 103(0.100-y)
(y)(0.80+y)=
Init 0.100 M 0 0.80
-y +y + y
Eq 0.100-y y 0.80 + y
K = 1
8.2 x 103(0.100-y)
(y)(0.80+y)=
Assume y is small
8y = 1.2 x 10-4
y = 1.5 x 10-5 M/L
Ag(NH3)2+
( aq) Ag(NH3)+(aq) + NH3(aq)
Init 0.100 M 0 0.80
-y +y + y
Eq 0.100 1.5 x 10-5 0.80
Ag(NH3)+( aq) Ag+
(aq) + NH3(aq)
[Ag+][NH3]
[Ag(NH3)+]=
1
K1
= 4.8 x 10-4
Eq 0.100 1.5 x 10-5 0.80
Ag(NH3)+( aq) Ag+
(aq) + NH3(aq)
[Ag+][NH3]
[Ag(NH3)+]=
1
K1
= 4.8 x 10-4
Eq 0.100 1.5 x 10-5 0.80
[Ag+] =(1.5 x 10-5)(4.8 x 10-4)
0.80
Ag(NH3)+( aq) Ag+
(aq) + NH3(aq)
[Ag+][NH3]
[Ag(NH3)+]=
1
K1
= 4.8 x 10-4
Eq 0.100 1.5 x 10-5 0.80
[Ag+] =(1.5 x 10-5)(4.8 x 10-4)
0.80=
9 x 10-9 M/L
Ag+(aq) + NH3(aq) Ag(NH3)+
(aq)
Ag(NH3)+(aq) + NH3(aq) Ag(NH3)2
+(aq)
9 x 10-9 0.80 1.5 x 10-5
1.5 x 10-5 0.80 0.10
Formation of complex ions starting
with AgCl.
AgCl(s) Ag+(aq) + Cl-
(aq)
Ksp = 1.6 x 10-10
By adding NaCl, increase in [Cl-]
(common ion effect) causes shift
to AgCl(s)
Ksp = 1.6 x 10-10
Ag+(s) + 2 Cl-
(aq) AgCl2-
(aq)
AgCl(s) Ag+(aq) + Cl-
(aq)
[AgCl2-]
[Ag+][Cl-]2K = 1.8 x 105 =
Ksp = 1.6 x 10-10
Ag+(s) + 2 Cl-
(aq) AgCl2-
(aq)
AgCl(s) Ag+(aq) + Cl-
(aq)
[AgCl2-]
[Ag+][Cl-]2K = 1.8 x 105 =
[Ag+] = [Cl-] = 1.3 x 10-5
Ksp = 1.6 x 10-10
Ag+(s) + 2 Cl-
(aq) AgCl2-
(aq)
AgCl(s) Ag+(aq) + Cl-
(aq)
[AgCl2-] [Ag+][Cl-]2 = (1.8 x 105)
[Ag+] = [Cl-] = 1.3 x 10-5
Ksp = 1.6 x 10-10
Ag+(s) + 2 Cl-
(aq) AgCl2-
(aq)
AgCl(s) Ag+(aq) + Cl-
(aq)
[Ag+] = [Cl-] = 1.3 x 10-5
[AgCl2-] (1.3 x 10-5)3 =
4 x 10-10
= (1.8 x 105)
[AgCl2-] [Ag+][Cl-]2 = (1.8 x 105)
Ksp = 1.6 x 10-10
Ag+(s) + 2 Cl-
(aq) AgCl2-
(aq)
AgCl(s) Ag+(aq) + Cl-
(aq)
[Ag+] = 1.3 x 10-5
[AgCl2-] (1.3 x 10-5) =
2.34 M = (1.8 x 105)
[AgCl2-] [Ag+][Cl-]2 = (1.8 x 105)
Change [Cl-] 1 M
Hydrolysis by complex ions
+ H2O(l)
+ H3O+
+ H2O(l)
+ H3O+
Ka = [H3O+][Fe(H2O)5OH2+]
[Fe(H2O)63+]
=
7.7 x 10-3