Test Bank General Chemistry, 10th edition 1
Chapter 17 – Solubility and Complex-Ion Equilibria
1. Cation C and anion A form an ionic compound for which Ksp = s2, where s is the molar
solubility of the ionic compound. Which of Figures I–III represent(s) possible results of the
mixing of an aqueous solution containing cation C with an aqueous solution containing
anion A?
A)
only I
B)
only III
C)
both I and III
D)
both I and II
E)
only II
2. Cation C and anion A form an ionic compound for which Ksp = 4s3, where s is the molar
solubility of the ionic compound. Which of Figures I–III represent(s) possible results of the
mixing of an aqueous solution containing cation C with an aqueous solution containing
anion A?
A)
only III
B)
only II
C)
both I and II
D)
only I
E)
both I and III
3. Which of the following particulate views is/are consistent with a heterogeneous
equilibrium?
I
II
III
A)
I only
B)
II only
C)
III only
D)
II and III
E)
I, II, and III
4. What is the solubility product expression for Al(OH)3?
A)
Ksp = [Al3+][3OH–]
B)
Ksp = 3[Al3+][OH–]3
C)
Ksp = [Al3+][OH–]3
D)
Ksp = [Al3+][3OH–]3
E)
Ksp = [Al3+][OH–]
5. What is the solubility product expression for Th(IO3)4?
A)
Ksp = [Th4+][4IO3–]4
B)
Ksp = [Th4+][IO3–]
C)
Ksp = [Th][IO3]4
D)
Ksp = [Th4+][IO3–]4
E)
Ksp = [Th4+][IO3–]
6. What is the solubility product expression for Zn3(PO4)2?
A)
Ksp = [Zn32+][(PO43–)2]
B)
Ksp = [3Zn2+]3[2PO43–]2
C)
Ksp = [Zn2+][2PO43–]
D)
Ksp = [Zn3+]2[PO42–]3
E)
Ksp = [Zn2+]3[PO43–]2
7. What is the solubility product expression for mercury(I) iodide, Hg2I2?
A)
Ksp = [Hg22+][2I–]2
B)
Ksp = [Hg22+][I–]2
C)
Ksp = [Hg22+][2I– ]
D)
Ksp = [Hg2][I2]
E)
Ksp = [Hg+]2[I–]2
8. What is the solubility product expression for La2(CO3)3?
A)
Ksp = [2La3+]2[3CO32–]3
B)
Ksp = [La2+]2[CO32–]3
C)
Ksp = [2La3+]2[CO32–]3
D)
Ksp = [2La3+][3CO32–]
E)
Ksp = [La3+]2[CO32–]3
9. What is the solubility product expression for Pb3(PO4)4?
A)
Ksp = [Pb3+]4[PO44–]3
B)
Ksp = [3Pb3+][4PO43–]
C)
Ksp = [3Pb3+]3[4PO43–]4
D)
Ksp = [Pb2+]3[PO43–]2
E)
Ksp = [Pb4+]3[PO43–]4
Test Bank General Chemistry, 10th edition 4
10. What is the solubility product expression for Sn(IO3)2?
A)
Ksp = [Sn2+][IO3–]2
B)
Ksp = [Sn4+][2IO32–]2
C)
Ksp = [Sn2+][2IO3–]
D)
Ksp = [Sn4+][IO32–]2
E)
Ksp = [Sn2+][2IO3–]2
11. Figures I–IV represent ionic compounds formed upon the mixing of an aqueous solution
containing cation C with an aqueous solution containing anion A. Identify the figure(s) that
represent(s) products for which Ksp = s2, where s is the molar solubility of the ionic
compound.
A)
only I
B)
only II
C)
only IV
D)
only III
E)
both I and II
12. Figures I–IV represent ionic compounds formed upon the mixing of an aqueous solution
containing cation C with an aqueous solution containing anion A. Identify the figure(s) that
represent(s) products for which Ksp = 4s3, where s is the molar solubility of the ionic
compound.
Test Bank General Chemistry, 10th edition 5
A)
both I and II
B)
only II
C)
only IV
D)
only I
E)
only III
13. Figures I–IV represent ionic compounds formed upon the mixing of an aqueous solution
containing cation C with an aqueous solution containing anion A. Identify the figure(s) that
represent(s) products for which Ksp = 108s5, where s is the molar solubility of the ionic
compound.
A)
only II
B)
both I and II
C)
only IV
D)
only III
E)
only I
14. What is the relationship between molar solubility (s) and Ksp for calcium fluoride?
A)
B)
C)
D)
E)
15. What is the correct mathematical expression for finding the molar solubility (s) of Sn(OH)2?
A)
2s3 = Ksp
B)
4s3 = Ksp
C)
108s5 = Ksp
D)
2s2 = Ksp
E)
8s3 = Ksp
16. The concentration of calcium carbonate in a saturated aqueous solution of the salt at 25°C is
6.71 10−5
M. What is the Ksp of this sparingly soluble salt?
A)
4.50 10−9
B)
C)
D)
8.19 10−3
E)
4.06 10−2
17. The solubility of strontium carbonate in water at 25°C is
4.50 10−3
g/L. What is the Ksp of
this sparingly soluble salt?
A)
B)
C)
D)
5.52 10−3
E)
3.12 10−2
Test Bank General Chemistry, 10th edition 7
18. After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium
concentration of Pb2+ is 1.6 10–2 M. What is Ksp for PbCl2?
A)
4.0 10–6
B)
1.6 10–5
C)
2.5 10–4
D)
4.8 10–2
E)
1.0 10–6
19. The solubility of lead(II) sulfate is 4.0 10–2 g/L. What is the solubility product constant
for lead(II) sulfate?
A)
1.7 10–8
B)
1.3 10–4
C)
1.6 10–3
D)
4.6 10–15
E)
8.9 10–12
20. The solubility of silver(I) carbonate is 3.6 10–2 g/L. What is the solubility product
constant for silver(I) carbonate?
A)
4.4 10–15
B)
8.9 10−12
C)
1.7 10–8
D)
1.3 10–4
E)
1.3 10–3
21. The hydroxide ion concentration of a saturated solution of Fe(OH)2 is
1.16 10−5
M. What
is the solubility product constant for Fe(OH)2?
A)
B)
C)
D)
3.41 10−3
E)
2.26 10−2
Test Bank General Chemistry, 10th edition 8
22. The silver-ion concentration in a saturated solution of silver(I) chromate is 1.3 10–4 M.
What is Ksp for silver(I) chromate?
A)
2.9 10–16
B)
4.2 10–9
C)
8.8 10–12
D)
1.1 10−12
E)
1.7 10–8
23. Which of the following salts has the highest molar solubility in water?
A)
SrCO3 (Ksp = 9.3 10–10)
B)
BaSO4 (Ksp = 1.1 10–10 )
C)
PbS (Ksp = 2.5 10–27)
D)
BaCrO4 (Ksp = 1.2 10–10)
E)
AgCl (Ksp = 1.8 10–10 )
24. Which of the following salts has the lowest molar solubility?
A)
SrCO3 (Ksp = 9.3 10–10)
B)
MnS (Ksp = 2.5 10–10)
C)
BaF2 (Ksp = 1.0 10–6)
D)
BaSO4 (Ksp = 1.1 10–10)
E)
AgCl (Ksp = 1.8 10–10)
25. Rank the following salts in order of increasing molar solubility.
Salt
Ksp
BaSO4
1.1 10–10
AgCl
1.8 10–10
BaCO3
9.1 10–9
CdS
8 10–27
PbSO4
1.8 10–8
A)
CdS < AgCl < BaSO4 < BaCO3 < PbSO4
B)
CdS < AgCl < BaCO3 < BaSO4 < PbSO4
C)
CdS < BaSO4 < AgCl < BaCO3 < PbSO4
D)
PbSO4 < BaCO3 < AgCl < BaSO4 < CdS
E)
PbSO4 < BaCO3 < BaSO4 < AgCl < CdS
26. A saturated solution of which of the following salts will have the lowest molar concentration
of chromate ion?
A)
BaCrO4 (Ksp = 2.1 10–10)
B)
CuCrO4 (Ksp = 3.6 10-6)
C)
Ag2CrO4 (Ksp = 1.2 10–12)
D)
Hg2CrO4 (Ksp = 2.0 10-9)
E)
Tl2CrO4 (Ksp = 9.8 10–13)
27. A saturated solution of which of the following salts will have the greatest molar
concentration of silver ion?
A)
Ag2S (Ksp = 8 10–51)
B)
AgCl (Ksp = 1.8 10–10)
C)
Ag2CrO4 (Ksp = 1.2 10–12)
D)
Ag2CO3 (Ksp = 8.1 10–12)
E)
Ag4Fe(CN)6 (Ksp = 8.5 10–45)
28. What is the solubility (in g/L) of aluminum hydroxide at 25°C? The solubility product
constant for aluminum hydroxide is 4.6 10–33 at 25°C.
A)
3.6 10–31 g/L
B)
8.2 10–10 g/L
C)
2.8 10–7 g/L
D)
5.3 10–15 g/L
E)
1.8 10–31 g/L
29. What is the solubility (in g/L) of silver(I) bromide at 25°C? The solubility product constant
for silver(I) bromide is 5.0 10–13 at 25°C.
A)
9.4 10–3 g/L
B)
9.4 10–11 g/L
C)
1.3 10–4 g/L
D)
4.7 10–11 g/L
E)
7.9 10–2 g/L
30. Rank the following metal sulfides in order of increasing molar solubility in water.
Salt
Ksp
CoS
4 10–21
CuS
6 10–36
FeS
6 10–18
HgS
1.6 10–52
MnS
2.5 10–10
A)
MnS < FeS < CoS < CuS < HgS
B)
FeS < HgS < CoS < CuS < MnS
C)
HgS < CuS < CoS < FeS < MnS
D)
CuS < CoS < FeS < MnS < HgS
E)
CoS < CuS < FeS < HgS < MnS
31. What is the molar solubility of silver(I) bromide at 25°C? The solubility product constant
for silver(I) bromide is 5.0 10–13 at 25°C.
A)
7.1 10–7 M
B)
2.5 10–13 M
C)
4.2 10–4 M
D)
5.0 10–5 M
E)
5.0 10–13 M
Test Bank General Chemistry, 10th edition 11
32. What is the molar solubility of calcium sulfate at 25°C? The solubility product constant for
calcium sulfate is 2.4 10–5 at 25°C.
A)
2.4 10–5 M
B)
3.5 10–2 M
C)
1.2 10–5 M
D)
1.8 10–2 M
E)
4.9 10–3 M
33. What is the molar solubility of barium fluoride at 25°C? The solubility product constant for
barium fluoride is 1.0 10–6 at 25°C.
A)
6.3 10–3 M
B)
1.0 10–6 M
C)
5.0 10–7 M
D)
1.0 10–3 M
E)
1.6 10–2 M
34. What is the molar solubility of aluminum hydroxide at 25°C? The solubility product
constant for aluminum hydroxide is 4.6 10–33 at 25°C.
A)
2.3 10–33 M
B)
6.8 10–17 M
C)
4.6 10–33 M
D)
3.6 10–9 M
E)
1.0 10–11 M
35. What is the solubility (in g/L) of barium chromate at 25°C? The solubility product constant
for barium chromate is 1.2 10–10 at 25°C.
A)
0.42 g/L
B)
3.0 10–8 g/L
C)
1.5 10–8 g/L
D)
0.079 g/L
E)
0.0028 g/L
36. What is the solubility (in g/L) of calcium fluoride at 25°C? The solubility product constant
for calcium fluoride is 3.4 10–11 at 25°C.
A)
0.00046 g/L
B)
2.7 10–9 g/L
C)
0.016 g/L
D)
1.3 10–9 g/L
E)
0.094 g/L
37. Pure water is saturated with slightly soluble calcium fluoride, CaF2. Which of the following
is true concerning the equilibrium concentration of Ca2+?
A)
B)
[Ca2+] = [F–]
C)
D)
E)
[Ca2+] = Ksp
38. Which of the following salts has the lowest molar solubility in water?
A)
Ni(OH)2 (Ksp = 2.0 10–15)
B)
Fe(OH)2 (Ksp = 8 10–16)
C)
PbI2 (Ksp = 6.5 10–9)
D)
SrCO3 (Ksp = 9.3 10–10)
E)
AgBr (Ksp = 5.0 10–13)
Test Bank General Chemistry, 10th edition 13
39. Which of the following salts has the highest molar solubility in water?
A)
CaCO3 (Ksp = 3.8 10–9)
B)
Ni(OH)2 (Ksp = 2.0 10–15)
C)
Fe(OH)2 (Ksp = 8 10–16)
D)
AgBr (Ksp = 5.0 10–13)
E)
PbI2 (Ksp = 6.5 10–9)
40. Which salt has the highest molar solubility in pure water?
Salt
Ksp
Cd(OH)2
5.3 10–15
Fe(OH)2
8.0 10–16
PbCrO4
1.8 10–14
CdCO3
6.2 10–12
Mn(OH)2
2.0 10–13
A)
CdCO3
B)
Cd(OH)2
C)
Mn(OH)2
D)
PbCrO4
E)
Fe(OH)2
41. Which salt has the lowest molar solubility in pure water?
Salt
Ksp
Cd(OH)2
5.3 10–15
Fe(OH)2
8.0 10–16
PbCrO4
1.8 10–14
CdCO3
6.2 10–12
Mn(OH)2
2.0 10–13
A)
PbCrO4
B)
Fe(OH)2
C)
CdCO3
D)
Cd(OH)2
E)
Mn(OH)2
42. What is the hydroxide-ion concentration of a saturated solution of Ni(OH)2? For Ni(OH)2,
Ksp = 2.0 10–15.
A)
2.8 10–3 M
B)
7.9 10–6 M
C)
1.0 10–7 M
D)
2.7 10–2 M
E)
1.6 10–5 M
43. What is the pH of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp = 2.0 10–15.
A)
4.80
B)
8.90
C)
5.10
D)
9.20
E)
7.00
44. Rank the following salts in order of increasing molar solubility.
Salt
Ksp
AgSCN
1.0 10–12
Ag2CrO4
1.1 10–12
Ag3PO4
1.0 10–16
A)
AgSCN < Ag2CrO4 < Ag3PO4
B)
AgSCN < Ag3PO4 < Ag2CrO4
C)
Ag3PO4 < Ag2CrO4 < AgSCN
D)
Ag3PO4 < AgSCN < Ag2CrO4
E)
Ag2CrO4 < AgSCN < Ag3PO4
45. The insoluble salts AV, B2W, C2X3, DY2, and EZ3, which were formed from the metal ions
A+, B+, C3+, D2+, and E3+ and the nonmetals V1–, W2–, X2–, Y1–, and Z1–, all have the same
Ksp value. Which salt has the highest molar solubility?
A)
AV
B)
EZ3
C)
DY2
D)
B2W
E)
C2X3
46. In which of the following solutions would silver(I) phosphate, Ag3PO4, be least soluble?
A)
0.10 M Na3PO4
B)
0.10 M AgNO3
C)
0.10 M Na2HPO4
D)
0.10 M HNO3
E)
0.10 M NaH2PO4
47. In which of these solutions would silver(I) carbonate have the lowest molar solubility? For
silver(I) carbonate, Ksp = 8.5 10–12.
A)
0.03 M H2CO3
B)
0.1 M AgNO3
C)
0.01 M AgNO3
D)
0.1 M Na2CO3
E)
pure water
48. The figure below represents the result of adding which of the following aqueous solutions to
a filtered, saturated solution of AgCl?
A)
only NaCl(aq)
B)
only HNO3(aq)
C)
HCl(aq) or NaCl(aq)
D)
only HCl(aq)
E)
HCl(aq) or HNO3(aq)
49. What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate
containing 0.0030 M Na2CO3? For Ag2CO3, Ksp = 8.6 10–12.
A)
6.0 10–4 M
B)
2.0 10–9 M
C)
8.0 10–9 M
D)
5.4 10–5 M
E)
8.0 10–4 M
50. What is the molar solubility of MgF2 in a 0.40 M Mg(NO3)2 solution? For MgF2,
Ksp = 8.4 10–8.
A)
8.0 10–8 M
B)
2.3 10–4 M
C)
2.0 10–-8 M
D)
4.6 10–4 M
E)
3.2 10–3 M
Test Bank General Chemistry, 10th edition 17
51. What is the molar solubility of MgF2 in a 0.45 M NaF solution? For MgF2, Ksp = 8.4 10–8.
A)
1.0 10–7 M
B)
1.4 10–4 M
C)
1.9 10–7 M
D)
7.1 10–4 M
E)
4.1 10–7 M
52. Ksp for PbF2 is 4.0 10–8. If a 0.034 M NaF solution is saturated with PbF2, what is [Pb2+] in
solution?
A)
4.6 10–11 M
B)
1.4 10–9 M
C)
1.2 10–6 M
D)
1.0 10–3 M
E)
3.5 10–5 M
53. The solubility of La(IO3)3 in a 0.62 M KIO3 solution is 1.0 10–7 mol/L. Calculate Ksp for
La(IO3)3.
A)
6.2 10–8
B)
2.4 10–22
C)
2.4 10–1
D)
2.4 10–8
E)
none of these
54. Which of the following, when added to a saturated solution of AgCl, will cause a decrease
in the molar concentration of Ag+ relative to the original solution?
1.
HCl(g)
2.
AgCl(s)
3.
MgCl2(s)
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
1, 2, and 3
55. How many moles of CaF2 will dissolve in 3.0 L of 0.051 M NaF solution? (Ksp for
CaF2 = 4.0 10–11)
A)
2.6 10–10
B)
1.5 10–8
C)
4.6 10–8
D)
5.1 10–9
E)
none of these
56. Which of Figures I–IV represent(s) the result of mixing aqueous solutions of Na2S and
NiCl2 in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion)
A)
both I and II
B)
only I
C)
only II
D)
only III
E)
only IV
57. Which Figures I–IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl2
in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion)
A)
only II
B)
both I and II
C)
only IV
D)
only I
E)
only III
58. For which of the following will precipitation be expected?
A)
Qc < Ksp
B)
Qc = 1
C)
Qc = Ksp
D)
Qc > Ksp
E)
Ksp = 1
59. Which of the following will apply to a saturated solution of an ionic compound?
A)
Qc < Ksp
B)
Qc > Ksp
C)
Qc = Ksp
D)
Ksp = 1
E)
Qc = 1