1. What is the molar solubility of iron (II) sulfide?
(Ksp = 5.9 × 10–19)
(A) 3.6 × 10–37 M
(D) 7.7 × 10–10 M
(B) 3.0 × 10–19 M
(E) 6.5 × 10–5 M
–19
(C) 6.0 × 10 M
2. In a saturated solution of Mg3(PO4)2 the [Mg2+] is
1.0 × 10-4 M and the [PO43–] is 1.0 × 10–6 M. The Ksp of
Mg3(PO4)2 is calculated by the expression
(A) (1.0 × 10–4) (1.0 × 10–6)
(B) (1.0 × 10–4)2 (1.0 × 10–6)3
(C) (1.0 × 10–4)3 (1.0 × 10–6)2
(D) (3.0 × 10–4)3 (2.0 × 10–6)2
(E) (3.0 × 10–4) (2.0 × 10–6)2
3. A 25.00 mL sample of a saturated ZnF2 solution was
evaporated to dryness. The mass of the residue
was 0.508 g. What is the solubility product constant of
ZnF2?
(A) 3.04 × 10–2
(D) 3.20 × 10–5
(B) 4.21 × 10–3
(E) 3.20 × 10–5
–4
(C) 4.67 × 10
4. If each of the following salts has a Ksp value of
1.00 × 10–9, which is the least soluble in pure water?
(A) XY
(B) XY2
(C) X3Y
(D) X2Y3
(E) XY4
5. The solubility product of ZnCO3 is approximately
16. × 10–11. What is the the Molar solubility of ZnCO3?
(A) 4.0 × 10–6 Molar
(D) 2.0 × 10–3 Molar
–5
(B) 4.0 × 10 Molar
(E) 1.6 × 10–11 Molar
(C) 2.6 × 10–24 Molar
6. In
solution of manganese (II) hydroxide, [Mn
2+ a saturated
] 4.5 × 10–5 M. What is the Ksp of Mn(OH)2?
(A) 4.3 × 10–7
(D) 4.1 × 10–9
(B) 3.6 × 10–13
(E) 3.6 × 10–13
(C) 2.0 × 10–9
7. At a certain temperature, the solubility of BaF2 is
7.4 × 10–3 moles per liter. The Ksp of BaF2 is
(A) 1.6 × 10–6
(D) 5.5 × 10–2
(B) 5.5 × 10–5
(E) 1.1 × 10–4
–3
(C) 7.4 × 10
8. The solubility of barium oxalate, BaC2O4, is 4.8 × 10–4
M. The value of Ksp is
(A) 2.3 × 10–7
(D) 2.2 × 10–2
–4
(B) 4.8 × 10
(E) 2.6 × 10–1
(C) 2.4 × 10–4
9. A saturated solution of BaF2 has a [Ba2+] of 3.6 × 10–3 M.
What is the Ksp value?
(A) 3.6 × 10–3
(D) 2.1 × 10–8
(B) 7.2 × 10–3
(E) 3.6 × 10–10
–7
(C) 1.9 × 10
10. The solubility of AgBrO3 is
(Ksp = 5.33 × 10–5)
(A) 2.8 × 10–9 M
(D) 7.3 × 10–3 M
–5
(B) 5.3 × 10 M
(E) 9.2 × 10–2 M
(C) 1.1 × 10–4 M
11. The molar solubility of AgIO3 in water at 9.4oC is
9.59 × 10–5 M. What is the Ksp?
(A) 9.59 × 10–5
(D) 1.83 × 10–8
(B) 9.20 × 10–9
(E) 4.60 × 10–9
(C) 8.46 × 10–17
12. What is the molar solubility of magnesium hydroxide in
water (Ksp for Mg(OH)2 at 291 K is 1.00 × 10–11)?
(A) (0.25 × 10–11)1/3
(D) (0.25 × 10–11)1/2
(B) (1.00 × 10–11)1/3
(E) (0.50 × 10–11)1/2
–11 1/3
(C) (0.50 × 10 )
13. The [OH–] is measured to be 3.3 × 10–3 M in a 100. mL
sample of a saturated solution of Al(OH)3. What is the
solubilty of Al(OH)3?
(A) 1.1 × 10–4 M
(D) 3.3 × 10–3 M
–4
(B) 3.3 × 10 M
(E) 1.1 × 10–3 M
(C) 1.1 × 10–2 M
14. 25 mL of 2.0 M Li2SO3 is mixed with 25 mL of 2.0 M
CuNO3. A precipitate forms and the concentration of Cu+
becomes negligible. Which order correctly lists the ions
remaining in solution in order of decreasing
concentration?
(A) [Li+] >[NO3–] > [SO3–2]
(B) [NO3–] > [Li+] > [SO3–2]
(C) [NO3–] > [SO3–2] > [Li+]
(D) [Li+] > [SO3–2] > [NO3–]
(E) [SO3–2] > [NO3–] > [Li+]
15. A saturated solution of AgCH3COO was evaporated to
dryness. The 250.0 mL sample was found to contain
1.84 g AgCH3COO. What is the solubility product
constant for AgCH3COO?
(A) 4.41 × 10–2
(D) 2.02 × 10–3
–2
(B) 1.10 × 10
(E) 1.57 × 10–3
(C) 1.94 × 10–3
16. What is the molar solubility in water of calcium sulfate
(Ksp for CaSO4 at 299 K is 2.50 × 10–5)?
(A) (2.50 × 10–5)1/2
(D) (1.25 × 10–5)1/4
(B) (1.25 × 10–11)1/2
(E) (2.50 × 10–11)1/4
(C) (5.00 × 10–11)1/2
23. The solubility of MnS is 4.8 × 10–7 M, at 25o C. The Ksp
value is
(A) 2.3 × 10–13
(D) 6.9 × 10–4
–7
(B) 4.8 × 10
(E) 7.2 × 10–2
(C) 9.6 × 10–7
17. How many moles of NaCl must dissolve into 1.00 L of a
saturated solution of AgCl to reduce the silver ion
concentration to 8.00 × 10–8 M?
(Ksp AgCl = 1.6 × 10–10)
(A) 0.002 mol
(D) 0.040 mol
(B) 0.004 mol
(E) 0.008 mol
(C) 0.020 mol
24. The solubility of FeF2 is 8.4 × 10–3 M. What is the Ksp
value for this substance?
(A) 5.9 × 10–7
(D) 8.4 × 10–3
(B) 2.4 × 10–6
(E) 2.6 × 10–1
–5
(C) 7.1 × 10
18. If the Ksp for PbBr2 is 6.0 × 10–6. What is the molar
solubility in water of PbBr2?
(A) 6.0 × 10–6 moles/liter
(B) 1.5 × 10–6 moles/liter
(C) (6.0 × 10–6)½ moles/liter
(D) (6.0 × 10–6)¢ moles/liter
(E) (1.5 × 10–6)¢ moles/liter
19. In a saturated solution of zinc hydroxide, at 40ºC, the
[Zn2+] = 1.8 × 10–5 M. The Ksp of Zn(OH)2 is
(A) 5.8 × 10–15
(D) 6.5 × 10–10
(B) 2.3 × 10–14
(E) 7.2 × 10–8
–14
(C) 1.8 × 10
20. When 1.00 L of a saturated solution of CaF2 was
evaporated to dryness, 2.66 × 10–2 g of residue was
formed. What is the value of Ksp for this reaction?
(A) 6.82 × 10–4
(D) 1.56 × 10–3
–10
(B) 1.58 × 10
(E) 4.22 × 10–5
(C) 2.65 × 10–2
21. The solubility of manganese (II) sulfide is 1.7 × 10–7 M
at 25ºC. What is the solubility product constant for this
reaction?
(A) 2.9 × 10–14
(D) 1.5 × 10–3
(B) 1.7 × 10–7
(E) 4.1 × 10–4
–7
(C) 3.4 × 10
22. The Ksp expression for a saturated solution of Ca3(PO4)2
is
(A) Ksp = [Ca2+][PO43–]
(B) Ksp = [Ca2+]3[PO43–]2
(C) Ksp = [3Ca2+][2PO43–]
(D) Ksp = [3Ca2+]3[2PO43–]2
(E) Ksp= [2Ca2+]3[3PO43–]2
25. The solubility of barium fluoride is 3.6 × 10–3 M. The
solubility product constant is
(A) 5.7 × 10–3
(D) 2.6 × 10–5
(B) 4.7 × 10–8
(E) 1.9 × 10–7
–5
(C) 1.3 × 10
26. The solubility of BaSO4 in water is 3.9 × 10–5 mol/liter.
What is the solubility product (Ksp)?
(A) 1.6 × 10–9
(D) 16. × 10–9
–5
(B) 3.9 × 10
(E) 6. × 10–3
(C) 7.8 × 10–5
27. The solubility of silver bromide is 7. × 10–7 M. What is
the solubility product (Ksp)?
(A) 7. × 10–7
(D) 7. × 10–13
(B) 50 × 10–7
(E) 9. × 10–4
(C) 5. × 10–13
28. How many grams of CaSO4 are dissolved in 100.0 mL of
a saturated CaSO4 solution at 25ºC?
(Ksp for CaSO4 = 8.4 × 10–3)
(A) 6.4 × 10–3 g
(D) 4.7 × 10–1 g
(B) 1.0 × 10–2 g
(E) 5.2 g
(C) 1.1 × 10–1 g
29. The solubility of magnesium carbonate (Ksp = 6.8 × 10–6)
is
(A) 4.6 × 10–11 M
(D) 2.6 × 10–3 M
–6
(B) 3.4 × 10 M
(E) 1.8 × 10–2 M
(C) 6.8 × 10–6 M
30. What is the ion product when 90.0 mL of 1.00 × 10–2 M
Cu(NO3)2 and 10.0 mL of 1.00 × 10–2 NaIO3 are mixed?
(A) 9.00 × 10–3
(D) 6.90 × 10–3
(B) 1.00 × 10–3
(E) 9.00 × 10–9
(C) 1.50 × 10–3
31. The solubility product expression for a saturated solution
of Fe2(SO4)3 is
(A)
(B)
(C)
(D)
(E)
32. The molar solubility of magnesium carbonate
(Ksp = 2.6 × 10–5) is
(A) 4.6 × 10–11 M
(D) 2.6 × 10–3 M
–6
(B) 6.8 × 10 M
(E) 5.1 × 10–2 M
(C) 1.4 × 10–5 M
33. The Ksp of calcium fluoride in water is 3.40 × 10–11 at
18.oC. What is the molar solubility of Ca2+?
(A) 4.08 × 10–4 M
(D) 2.04 × 10–4 M
(B) 6.14 × 10–34 M
(E) 1.05 × 10–11 M
(C) 3.23 × 10–4 M
34. At 25oC, the solubility of AgBr
(Ksp = 7.7 × 10–13 M) is
(A) 2.9 × 10–25 M
(D) 8.8 × 10–7 M
–13
(B) 5.4 × 10 M
(E) 1.5 × 10–5 M
(C) 2.7 × 10–13 M
35. The Ksp expression for a saturated solution of Ag2CO3 is
(A) Ksp = [Ag2+][CO32–]
(B) Ksp = [Ag2+]2[CO32–]
(C) Ksp = [2Ag+][CO32–]
(D) Ksp = [2Ag+]2[CO32–]
(E) Ksp = [Ag+]2[CO32–]
36. How many moles of KI must dissolve into 1.00 L of a
saturated solution of PbI2 to reduce the lead ion
concentration to 2.00 × 10–6 M?
(Ksp PbI2 = 1.40 × 10–8)
(A) 0.200 mol
(D) 0.400 mol
(B) 4.00 mol
(E) 0.800 mol
(C) 2.00 mol
37. What is the maximum amount of sodium sulfate, Na2SO4
, that will dissolve in 1.0 L of 0.10 M Pb(NO3)2 without
forming a precipitate? (Ksp for PbSO4 = 1.06 × 10–8)
(A) 1.8 × 10–8 mol
(D) 1.0 × 10–1 mol
(B) 1.8 × 10–7 mol
(E) 2.5 × 10–1 mol
–4
(C) 1.3 × 10 mol
FeSCN2+ ↔Fe3+ + SCN–
38.
The above dissociation reaction starts out at equilibrium.
If 1.5 moles of Fe+3 are precipitated out of the solution,
which graph best represents how the individual
concentrations of all the ions react?
(A)
(B)
(C)
39. The molar solubility of Al(OH)3 in water at 18.oC is
7.99 × 10–5M. What is the Ksp?
(A) 1.10 × 10–15
(D) 5.10 × 10–13
(B) 4.08 × 10–17
(E) 8.85 × 10–15
(C) 2.96 × 10–6
40. The solubility product constant, Ksp for silver bromide,
AgBr, is 5.3 × 10–13 at room temperature. When equal
volumes of 2.0 × 10–3 M AgNO3 and 2.0 × 10–3 M NaBr
are mixed at room temperature, the mixing produces
(A) no visible precipitate
(B) a visible precipitate of AgBr
(C) a visible precipitate of NaNO3
(D) a visible precipitate of AgNO3
(E) a visbile precipitate of NaBr
41. The Ksp of magnesium carbonate in water is 2.60 × 10–5
at 12.oC. What is the molar solubility of Mg2+?
(A) 2.60 × 10–5
(D) 1.27 × 10–3
(B) 5.09 × 10-3
(E) 6.50 × 10–6
(C) 6.76 × 10–10
42. At 25ºC, the maximum [Zn2+] that exist in 0.250 M Na2S
is (Ksp for ZnS at 25ºC = 2.0 × 10–25)
(A) 5.0 × 10–26 M
(D) 2.6 × 10–13 M
(B) 2.0 × 10–25 M
(E) 8.0 × 10–25 M
–13
(C) 4.5 × 10 M
43. Chromium (II) chloride has a hypothetical
Ksp = 1.2 × 10–25. What is the molar solubility of
chromium chloride?
(A) 3 × 10–26
(D) 3.5 × 10–13
–26
(B) 1.2 × 10
(E) 3.1 × 10–9
(C) 8.8 × 10–14
(D)
(E)
44. A 100.00 mL sample of a saturated solution of Ca(OH)2
is evaporated to dryness. The mass of the solid residue is
0.125 g. What is the solubility product of Ca(OH)2?
(A) Ksp = 1.68 × 10–2
(B) Ksp = 5.69 × 10–4
(C) Ksp = 3.37 × 10–2
(D) Ksp = 9.60 × 10–6
(E) Ksp = 1.92 × 10–5
45. The solubility of PbS is 2.9 × 10–14 M. What is the value
of Ksp for PbS?
(A) 3.4 × 10–7
(D) 1.7 × 10–7
–14
(B) 2.9 × 10
(E) 8.4 × 10–28
(C) 5.8 × 10–14
46. What is the maximum [Mg2+] that can exist in a solution
with a pOH of 2.00?
(Ksp for Mg(OH)2 = 1.2 × 10–11)
(A) 5.6 × 10–12
(D) 5.2 × 10–2
–8
(B) 3.0 × 10
(E) 5.6 × 10–3
(C) 1.0 × 10–2
47. When equal volumes of 0.20 M K2CrO4 and 0.20 M
AgNO3 are mixed, a red precipitate is formed. What is
the formula of the net ionic equation for this reaction?
(A) K+(aq) + NO3–(aq) → KNO3(s)
(B) 2 Ag+(aq) + CrO42–(aq) → Ag2CrO4(s)
(C) K2CrO4(aq) + AgNO3(aq) →
Ag2CrO4(aq) + 2 KNO3(s)
(D) 2 Ag+(aq) + CrO42–(aq) + 2 K+(aq) +
2 NO3–(aq) → Ag2CrO4(aq) + 2 KNO3(s)
(E) 2 Ag+(aq) + K2CrO4(aq) →
Ag2CrO4(aq) + 2 KNO3(s)
48. Which of the following compounds could be used to
prepare a 0.20 M solution of hydroxide ion?
(A) KOH
(B) Fe(OH)3
(C) Mg(OH)2
(D) Zn(OH)2
(E) Mn(OH)2
49. In 0.20 M Na2CrO4, the ion concentrations are
(A) [Na+] = 0.40 M; [CrO42–] = 0.20 M
(B) [Na+] = 0.20 M; [CrO42–] = 0.20 M
(C) [Na+] = 0.20 M; [CrO42–] = 0.40 M
(D) [Na+] = 0.40 M; [CrO42–] = 0.80 M
(E) [Na+] = 0.40 M; [CrO42–] = 0.40 M
50. Which of the following oxides will dissolve in water to
form an acidic solution?
(A) SO2
(D) MgO
(B) TiO
(E) Na2O
(C) K2O
51. Which of the following represents the equilibrium in a
saturated solution of Cr2(SO4)3?
(A) Cr2(SO4)3(s) ↔ Cr3+(aq) + SO43–(aq)
(B) Cr2(SO4)3(s) ↔ Cr2+(aq) + SO43–(aq)
(C) Cr2(SO4)3(s) ↔ Cr3+(aq) + SO42–(aq)
(D) Cr2(SO4)3(s) ↔ 2 Cr2+(aq) + 3 SO43–(aq)
(E) Cr2(SO4)3(s) ↔ 2 Cr3+(aq) + 3 SO42–(aq)
52. When 250. mL of 0.36 M Sr(OH)2 are added to 750. mL
of water, the resulting ion concentrations are
(A) [Sr2+] = 0.12 M and [OH–] = 0.12 M
(B) [Sr2+] = 0.12 M and [OH–] = 0.24 M
(C) [Sr2+] = 0.090 M and [OH–] = 0.090 M
(D) [Sr2+] = 0.090 M and [OH–] = 0.180 M
(E) [Sr2+] = 0.090 M and [OH–] = 0.24 M
53. Saturated solutions of CuS, Na2S, SnS and Al2S are
prepared at 25ºC. The [S2–] will be greatest in the
solution of
(A) CuS
(B) Na2S
(C) SnS
(D) Al2S
(E) Concentrations will be equal in all solutions
54. If the solubility of Pb(OH)2 is 0.155 g/L, then the
concentration of each ion in a saturated solution
of Pb(OH)2 is
(A) [Pb2+] = 0.155 g/L and [OH–] = 0.155 g/L
(B) [Pb2+] = 0.052 g/L and [OH–] = 0.103 g/L
(C) [Pb2+] = 6.43 × 10–4 M and [OH–] = 1.29 × 10–3 M
(D) [Pb2+] = 6.43 × 10–4 M and [OH–] = 6.43 × 10–4 M
(E) [Pb2+] = 6.43 × 10–2 M and [OH–] = 2.50 × 10–2 M
55. A 200.0 mL solution contains 0.050 mol of Ba(NO3)2.
The [NO3–] is
(A) 0.050 M
(D) 0.50 M
(B) 0.10 M
(E) 0.75 M
(C) 0.25 M
56. A saturated solution of NiCO3 was evaporated to
dryness. A 250.0 mL sample was found to contain 1.1 ×
10–2 g of NiCO3. The molar mass of NiCO3 is 118.7
g/mol. What is the molar solubility of NiCO3?
(A) 9.3 × 10–5 M
(D) 1.4 × 10–7 M
–4
(B) 3.7 × 10 M
(E) 2.5 × 10–5 M
(C) 4.4 × 10–2 M
57. In 1.5 M (NH4)2SO4, the ion concentrations are
(A) [NH4+] = 1.5 M and [SO42–] = 1.5 M
(B) [NH4+] = 1.5 M and [SO42–] = 3.0 M
(C) [NH4+] = 3.0 M and [SO42–] = 1.5 M
(D) [NH4+] = 3.0 M and [SO42–] = 3.0 M
(E) [NH4+] = 3.0 M and [SO42–] = 4.5 M
58. Al(OH)3(s) → Al3+(aq) + 3OH–(aq)
If aluminum hydroxide is completely ionized in water
according to the equation above, which of the following
equations is true?
(A) [Al3+] = [OH–] = [Al(OH)3]
(B) 3×[Al3+] = [OH–]
(C) [Al3+]3 = [OH–]
(D) [Al3+] = 3×[OH–]
(E) [Al3+] = [OH–]3
59. Potassium sulfide is completely ionized in water:
K2S(s) → 2 K+(aq) + S2–(aq) Which of the following
equations is true?
(A) [K+] = [S2–] = 2 × [K2S] (D) [K+] = 2 × [S2–]
(B) [K+]2 = [S2–]
(E) 2 × [K+] = [S2–]
(C) [K+] = [S2–]2
60. Calculate the ion product if 30.0 mL–4of 0.054 M Ca(NO3)
2 is mixed with 60.0 mL of 8.1 × 10 M Na2SO4?
(A) 2.7 × 10–9
(D) 1.6 × 10–7
–9
(B) 1.5 × 10
(E) 9.7 × 10–6
(C) 4.6 × 10–7
61. The greatest mass of solid SnS will dissolve in 1.0 L of
(A) 0.10 M H2O
(B) 0.10 M NH3
(C) 0.10 M MgS
(D) 0.10 M (NH4)2S
(E) 0.10 M Sn(NO3)2
62.
MgCO3(s) ↔ Mg2+(aq) + CO32–(aq)
The addition of which of the following substances in the
above equilibrium would decrease the solubility of
MgCO3?
(A) H2O
(D) OH–
(B) NaCl
(E) Na2CO3
(C) NaOH
63. To remove Mg2+ from a solution by precipitation, a
student should add
(A) NaI
(B) KOH
(C) Li2SO4
(D) H2O
(E) (NH4)2S
64. Silver chloride is least soluble in a 0.02–molar solution
of which of the followinng?
(A) AgNO3
(B) NaCl
(C) MgCl2
(D) AlCl3
(E) KOH
65. When 200 mL of 0.10 M NaOH is added to 800 mL of
0.10 M Ba(OH)2. What is the resulting concentration of
OH–(aq)? (Assume that all the volumes are additive)
(A) 0.06 M
(B) 0.10 M
(C) 0.12 M
(D) 0.18 M
(E) 0.34 M
66.
2 CrO42–(aq) + H2O(l) ↔ Cr2O72–(aq) + 2 OH–(aq)
(yellow)
(orange)
When HCl is added drop-by-drop to the yellow solution
above, the solution turns orange. What is the reason for
this color change?
(A) [OH–] decreases, therefore equilibrium shifts right
(B) [OH–] increases, therefore equilibrium shifts right
(C) [OH–] decreases, therefore equilibrium shifts left
(D) [OH–] increases, therefore equilibrium shifts left
(E) [OH–] remains constant, therefore equilibrium shifts
left
Answer Key
1.
D
30.
A
59.
D
2.
C
31.
A
60.
E
3.
A
32.
D
61.
A
4.
A
33.
D
62.
E
5.
A
34.
D
63.
B
6.
B
35.
E
64.
D
7.
A
36.
A
65.
D
8.
A
37.
A
66.
A
9.
C
38.
A
10.
D
39.
A
11.
B
40.
B
12.
A
41.
B
13.
E
42.
E
14.
A
43.
E
15.
D
44.
E
16.
A
45.
E
17.
A
46.
B
18.
E
47.
B
19.
B
48.
A
20.
B
49.
A
21.
A
50.
A
22.
B
51.
E
23.
A
52.
D
24.
B
53.
B
25.
E
54.
C
26.
A
55.
D
27.
C
56.
B
28.
C
57.
C
29.
D
58.
B