Question 1

If Qsp is larger than Ksp, precipitation should occur.

Accepted Answer

A) True 
 B)False

Question 2

The solubility product constant of silver sulfate is 1.6 × 10-5. What is the molar solubility of this compound?

Accepted Answer

A)  1.6 × 10-5 
B)  (16/2)1/2 × 10-2 
C)  (16/4)1/3 × 10-2 
D)  (16)1/2 × 10-3 
E)  (16/4)2/3 × 10-2 
A)  1.6 × 10-5 
B)  (16/2)1/2 × 10-2 
C)  (16/4)1/3 × 10-2 
D)  (16)1/2 × 10-3 
E)  (16/4)2/3 × 10-2

Question 3

Equal volumes of a 0.020 M Zn2+ solution and a 2.0 M NH3 solution are mixed. Kf for [Zn(NH3)4]2+ is 4.1 × 108. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC2O4 precipitate? What is Q? Ksp ZnC2O4 = 2.7 × 10-8

Accepted Answer

A)  yes, Q = 11 
B)  yes, Q = 2.9 × 10-12 
C)  no, Q = 2.9 × 10-12 
D)  yes, Q = 2.4 × 10-9 
E)  no, Q = 2.4 × 10-9 
A)  yes, Q = 11 
B)  yes, Q = 2.9 × 10-12 
C)  no, Q = 2.9 × 10-12 
D)  yes, Q = 2.4 × 10-9 
E)  no, Q = 2.4 × 10-9

Question 4

A solute's molar solubility and its molarity are not the same in a saturated aqueous solution.

Accepted Answer

A) True 
 B)False

Question 5

The solubility product constant for iron(III) hydroxide at 22 °C is 6.0 × 10-38. What mass of this compound will dissolve in 100 mL of 0.20 M sodium hydroxide, assuming no complex formation?

Accepted Answer

A)  6 × 10-39 g 
B)  7 × 10-37 g 
C)  8 × 10-35 g 
D)  9 × 10-33 g 
E)  1 × 10-30 g 
A)  6 × 10-39 g 
B)  7 × 10-37 g 
C)  8 × 10-35 g 
D)  9 × 10-33 g 
E)  1 × 10-30 g

Question 6

The solubility product constant of silver bromide is 5.0 × 10-13. What is the molar solubility of this compound?

Accepted Answer

A)  5.0 × 10-13 
B)  (50)1/2 × 10-6 
C)  (50)1/2 × 10-7 
D)  (5.0/2)1/2 × 10-7 
E)  (5.0 × 10-13)2 
A)  5.0 × 10-13 
B)  (50)1/2 × 10-6 
C)  (50)1/2 × 10-7 
D)  (5.0/2)1/2 × 10-7 
E)  (5.0 × 10-13)2

Question 7

Which of the following has the largest molar solubility?

Accepted Answer

A)  BaSO4, Ksp = 1.1 × 10-10 
B)  AgCl, Ksp = 1.6 × 10-10 
C)  Mg(OH)2, Ksp = 2 × 10-11 
D)  Cr(OH)2, Ksp = 6.3 × 10-11 
E)  Fe(OH)3, Ksp = 4 × 10-38 
A)  BaSO4, Ksp = 1.1 × 10-10 
B)  AgCl, Ksp = 1.6 × 10-10 
C)  Mg(OH)2, Ksp = 2 × 10-11 
D)  Cr(OH)2, Ksp = 6.3 × 10-11 
E)  Fe(OH)3, Ksp = 4 × 10-38

Question 8

The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is ________.

Accepted Answer

A)  Ksp = 9[Ag+]3 
B)  Ksp = 27[Ag+]4 
C)  Ksp = [Ag+]1/3 
D)  Ksp = 0.125[Ag+] 
E)  Ksp = 0.333[Ag+]4 
A)  Ksp = 9[Ag+]3 
B)  Ksp = 27[Ag+]4 
C)  Ksp = [Ag+]1/3 
D)  Ksp = 0.125[Ag+] 
E)  Ksp = 0.333[Ag+]4

Question 9

A saturated solution of silver chromate has a concentration of 7.4 × 10-5 M. What is the Ksp of this compound?

Accepted Answer

A)  (7.4 × 10-5)2 
B)  (7.4 × 10-5)3 
C)  3(7.4 × 10-5)3 
D)  7.4 × 10-5 
E)  4(7.4 × 10-5)3 
A)  (7.4 × 10-5)2 
B)  (7.4 × 10-5)3 
C)  3(7.4 × 10-5)3 
D)  7.4 × 10-5 
E)  4(7.4 × 10-5)3

Question 10

What is the concentration of free Zn2+ if 0.020 M Zn2+ solution is mixed with an equal volume of 2.0 M NH3? Kf for [Zn(NH3)4]2+ is 4.1 × 108.

Accepted Answer

A)  2.5 × 10-11 
B)  2.9 × 10-11 
C)  1.7 × 10-10 
D)  9.6 × 10-11 
E)  2.4 × 10-9 
A)  2.5 × 10-11 
B)  2.9 × 10-11 
C)  1.7 × 10-10 
D)  9.6 × 10-11 
E)  2.4 × 10-9

Question 11

The solubility of a salt MX2 with a molar mass of 114 g/mole is 3.42 g/liter. Calculate the Ksp.

Accepted Answer

A)  2.70 × 10-5 
B)  1.08 × 10-4 
C)  9.00 × 10-4 
D)  2.25 × 10-4 
E)  6.75 × 10-8 
A)  2.70 × 10-5 
B)  1.08 × 10-4 
C)  9.00 × 10-4 
D)  2.25 × 10-4 
E)  6.75 × 10-8

Question 12

When 100 mL each of 2.0 × 10-5 M Ca2+ and 2.0 × 10-3 M CO32- are mixed, what is the remaining Ca2+ ion concentration and is precipitation complete? The solubility product constant of CaCO3 is 2.8 × 10-9.

Accepted Answer

A)  2.8 × 10-6, no 
B)  1.0 × 10-3, no 
C)  6.9 × 10-5, no 
D)  2.8 × 10-3, no 
E)  2.8 × 10-6, yes 
A)  2.8 × 10-6, no 
B)  1.0 × 10-3, no 
C)  6.9 × 10-5, no 
D)  2.8 × 10-3, no 
E)  2.8 × 10-6, yes

Question 13

Write the solubility product constant expression for the following salt: Ca(OH)2.

Accepted Answer

A)  [Ca2+][OH-] 
B)  [Ca2+]2[OH-] 
C)  [Ca2+]3[OH-] 
D)  [Ca2+]2[OH-]2 
E)  [Ca2+][OH-]2 
A)  [Ca2+][OH-] 
B)  [Ca2+]2[OH-] 
C)  [Ca2+]3[OH-] 
D)  [Ca2+]2[OH-]2 
E)  [Ca2+][OH-]2

Question 14

The solubility product constant of M2CrO4(s) is 7.11 × 10-15. How many moles of M2CrO4(s) will dissolve in 744 mL of solution in which [CrO42-] = 0.056 M?

Accepted Answer

A)  2.7 × 10-7 mol 
B)  1.7 × 10-7 mol 
C)  1.2 × 10-5 mol 
D)  9.0 × 10-5 mol 
E)  3.6 ⊥ 10-7 mol 
A)  2.7 × 10-7 mol 
B)  1.7 × 10-7 mol 
C)  1.2 × 10-5 mol 
D)  9.0 × 10-5 mol 
E)  3.6 ⊥ 10-7 mol

Question 15

When 100 mL each of 2.0 × 10-4 M Ag+ and 2.0 × 10-1 M CO32- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of Ag2CO3 is 8.5 × 10-12.

Accepted Answer

A)  4.2 × 10-8, yes 
B)  2.0 × 10-4, no 
C)  9.2 × 10-6, no 
D)  1.0 × 10-3, no 
E)  8.5 × 10-9, yes 
A)  4.2 × 10-8, yes 
B)  2.0 × 10-4, no 
C)  9.2 × 10-6, no 
D)  1.0 × 10-3, no 
E)  8.5 × 10-9, yes

Question 16

The solubility of magnesium fluoride in water at 18 °C is tabulated as 0.0076 g per 100 mL. What is the solubility product for this salt?

Accepted Answer

A)  7.6 × 10-6 
B)  6.8 × 10-7 
C)  8.0 × 10-8 
D)  7.3 × 10-9 
E)  3.8 × 10-10 
A)  7.6 × 10-6 
B)  6.8 × 10-7 
C)  8.0 × 10-8 
D)  7.3 × 10-9 
E)  3.8 × 10-10

Question 17

A swimming pool was sufficiently alkaline so that the carbon dioxide absorbed from the air produced a solution in the pool that was 2 × 10-4 M in carbonate ion. If the pool originally contained 4 × 10-3 M Mg2+, 6 × 10-4 M Ca2+, and 8 × 10-7 M Fe2+, then the precipitate that was formed consisted of ________. [Ksp values are: CaCO3, 4.7 × 10-9; MgCO3, 4.0 × 10-5; FeCO3, 2.0 × 10-11]

Accepted Answer

A)  only MgCO3 
B)  only CaCO3 
C)  only FeCO3 
D)  only CaCO3 and FeCO3 
E)  MgCO3, CaCO3, and FeCO3 
A)  only MgCO3 
B)  only CaCO3 
C)  only FeCO3 
D)  only CaCO3 and FeCO3 
E)  MgCO3, CaCO3, and FeCO3

Question 18

Which of the following should dissolve the smallest amount of silver sulfide per liter, assuming no complex formation?

Accepted Answer

A)  0.1 M HNO3 
B)  0.1 M Na2S 
C)  0.1 M AgNO3 
D)  0.10 M NaNO3 
E)  pure water 
A)  0.1 M HNO3 
B)  0.1 M Na2S 
C)  0.1 M AgNO3 
D)  0.10 M NaNO3 
E)  pure water

Question 19

The pH of a solution may affect solubility only if the salt contains the OH- ion.

Accepted Answer

A) True 
 B)False

Question 20

Concentrated solutions of sodium sulfate, ammonium carbonate, and nickel (II) nitrate are mixed together. The precipitate which forms is ________.

Accepted Answer

A)  nickel (II) carbonate 
B)  nothing precipitates 
C)  nickel (II) sulfate 
D)  sodium carbonate 
E)  ammonium sulfate 
A)  nickel (II) carbonate 
B)  nothing precipitates 
C)  nickel (II) sulfate 
D)  sodium carbonate 
E)  ammonium sulfate

Exam 18: Solubility and Complex-Ion Equilibria

If Qsp is larger than Ksp, precipitation should occur.

The solubility product constant of silver sulfate is 1.6 × 10-5. What is the molar solubility of this compound?

Equal volumes of a 0.020 M Zn2+ solution and a 2.0 M NH3 solution are mixed. Kf for [Zn(NH3)4]2+ is 4.1 × 108. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC2O4 precipitate? What is Q? Ksp ZnC2O4 = 2.7 × 10-8

A solute's molar solubility and its molarity are not the same in a saturated aqueous solution.

The solubility product constant for iron(III) hydroxide at 22 °C is 6.0 × 10-38. What mass of this compound will dissolve in 100 mL of 0.20 M sodium hydroxide, assuming no complex formation?

The solubility product constant of silver bromide is 5.0 × 10-13. What is the molar solubility of this compound?

Which of the following has the largest molar solubility?

The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is ________.

A saturated solution of silver chromate has a concentration of 7.4 × 10-5 M. What is the Ksp of this compound?

What is the concentration of free Zn2+ if 0.020 M Zn2+ solution is mixed with an equal volume of 2.0 M NH3? Kf for [Zn(NH3)4]2+ is 4.1 × 108.

The solubility of a salt MX2 with a molar mass of 114 g/mole is 3.42 g/liter. Calculate the Ksp.

When 100 mL each of 2.0 × 10-5 M Ca2+ and 2.0 × 10-3 M CO32- are mixed, what is the remaining Ca2+ ion concentration and is precipitation complete? The solubility product constant of CaCO3 is 2.8 × 10-9.

Write the solubility product constant expression for the following salt: Ca(OH)2.

The solubility product constant of M2CrO4(s) is 7.11 × 10-15. How many moles of M2CrO4(s) will dissolve in 744 mL of solution in which [CrO42-] = 0.056 M?

When 100 mL each of 2.0 × 10-4 M Ag+ and 2.0 × 10-1 M CO32- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of Ag2CO3 is 8.5 × 10-12.

The solubility of magnesium fluoride in water at 18 °C is tabulated as 0.0076 g per 100 mL. What is the solubility product for this salt?

Which of the following should dissolve the smallest amount of silver sulfide per liter, assuming no complex formation?

The pH of a solution may affect solubility only if the salt contains the OH- ion.

Concentrated solutions of sodium sulfate, ammonium carbonate, and nickel (II) nitrate are mixed together. The precipitate which forms is ________.

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

Equal volumes of a 0.020 M Zn²⁺ solution and a 2.0 M NH₃ solution are mixed. Kf for [Zn(NH₃)₄]²⁺ is 4.1 × 10⁸. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC₂O₄ precipitate? What is Q? Ksp ZnC₂O₄= 2.7 × 10^-8

The solubility product constant for iron(III) hydroxide at 22 °C is 6.0 × 10^-38. What mass of this compound will dissolve in 100 mL of 0.20 M sodium hydroxide, assuming no complex formation?

The solubility product constant of silver bromide is 5.0 × 10^-13. What is the molar solubility of this compound?

A saturated solution of silver chromate has a concentration of 7.4 × 10^-5M. What is the Ksp of this compound?

What is the concentration of free Zn²⁺ if 0.020 M Zn²+ solution is mixed with an equal volume of 2.0 M NH₃? Kf for [Zn(NH₃)₄]²⁺ is 4.1 × 10⁸.

When 100 mL each of 2.0 × 10^-5 M Ca²⁺ and 2.0 × 10^-3M CO₃^2- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaCO₃ is 2.8 × 10^-9.

Write the solubility product constant expression for the following salt: Ca(OH)₂.

The solubility product constant of M₂CrO₄(s) is 7.11 × 10^-15. How many moles of M₂CrO₄(s) will dissolve in 744 mL of solution in which [CrO₄^2-] = 0.056 M?

When 100 mL each of 2.0 × 10^-4 M Ag⁺ and 2.0 × 10-1 M CO₃^2- are mixed, what is the remaining Ag⁺ ion concentration and is precipitation complete? The solubility product constant of Ag₂CO₃ is 8.5 × 10^-12.