Question 1

Which of the following cations is most likely to form insoluble chlorides?

Accepted Answer

A)  Na+ 
B)  Ca2+ 
C)  Mg2+ 
D)  Pb2+ 
E)  Fe3+ 
A)  Na+ 
B)  Ca2+ 
C)  Mg2+ 
D)  Pb2+ 
E)  Fe3+

Question 2

_____ is the universally used compound for developing black-and-white film.

Accepted Answer

The answer of _____ is the universally used compound for...

Question 3

Which of the following cations is most likely to form base-insoluble sulfides?

Accepted Answer

A)  Zn2+ 
B)  Ba3+ 
C)  Cu2+ 
D)  Li+ 
E)  Sn2+ 
A)  Zn2+ 
B)  Ba3+ 
C)  Cu2+ 
D)  Li+ 
E)  Sn2+

Question 4

If the Ksp for zinc carbonate (ZnCO3) is 1.46×10-10 at $25 ^ { \circ } \mathrm { C }$ , what is its aqueous solubility in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

Accepted Answer

A)  4.98×10-4 
B)  2.87×10-5 
C)  1.52×10-4 
D)  7.35×10-5 
E)  9.14×10-4 
A)  4.98×10-4 
B)  2.87×10-5 
C)  1.52×10-4 
D)  7.35×10-5 
E)  9.14×10-4

Question 5

Fe(II) forms the complex ion [Fe(OH)4]2− through equilibrium reactions in which hydroxide replaces water in a stepwise manner. If log K1 = 6.89, log K2 = 5.42, log K3 = −0.36, and log K4 = −1.78, what is its Kf?

Accepted Answer

A)  8.5×1042 
B)  6.8×1040 
C)  2.1×1041 
D)  1.2×1040 
E)  4.5×1041 
A)  8.5×1042 
B)  6.8×1040 
C)  2.1×1041 
D)  1.2×1040 
E)  4.5×1041

Question 6

Calcium oxalate monohydrate [Ca(O2CCO2).H2O] is a sparingly soluble salt. If its solubility in water at $30 ^ { \circ } \mathrm { C }$ is 8.25×10-4 g/100mL, what is its Ksp?

Accepted Answer

A)  3.65×10-10 
B)  7.24×10-9 
C)  5.85×10-8 
D)  3.19×10-9 
E)  9.63×10-8 
A)  3.65×10-10 
B)  7.24×10-9 
C)  5.85×10-8 
D)  3.19×10-9 
E)  9.63×10-8

Question 7

A molecular solute may be more soluble than predicted by the measured concentrations of ions in solution due to _____.

Accepted Answer

incomplete

Question 8

The formation of ion pairs decreases the solubility of a salt.

Accepted Answer

A) True 
 B)False

Question 9

Metal ions that precipitate together can be separated by changing the pH of the solution.

Accepted Answer

A) True 
 B)False

Question 10

If the ion product of a salt exceeds its solubility product, the solution becomes unsaturated.

Accepted Answer

A) True 
 B)False

Question 11

Which of the following is the chemical equation that describes the dissolution of aluminum hydroxide in a base?

Accepted Answer

A)  $\mathrm { Al } ( \mathrm { OH } ) _ { 3 } + \mathrm { OH } ^ { - } \rightarrow \left[ \mathrm { Al } ( \mathrm { OH } ) _ { 4 } \right] ^ { - }$ 
B)  $\mathrm { Al } ( \mathrm { OH } ) _ { 3 } + 3 \mathrm { H } ^ { + } \rightarrow \mathrm { Al } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \mathrm { O }$ 
C)  $2 \mathrm { Al } ( \mathrm { OH } ) _ { 3 } + 2 \mathrm { H } ^ { + } \rightarrow 2 \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } + 2 \mathrm { H } _ { 2 }$ 
D)  $2 \mathrm { Al } ( \mathrm { OH } ) _ { 3 } + 2 \mathrm { OH } ^ { - } \rightarrow \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } + 4 \mathrm { H } _ { 2 } \mathrm { O }$ 
E)  $\mathrm { Al } ( \mathrm { OH } ) _ { 3 } \rightarrow \mathrm { Al } ^ { 3 + } + 3 \mathrm { OH } ^ { - }$ 
A)  $\mathrm { Al } ( \mathrm { OH } ) _ { 3 } + \mathrm { OH } ^ { - } \rightarrow \left[ \mathrm { Al } ( \mathrm { OH } ) _ { 4 } \right] ^ { - }$ 
B)  $\mathrm { Al } ( \mathrm { OH } ) _ { 3 } + 3 \mathrm { H } ^ { + } \rightarrow \mathrm { Al } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \mathrm { O }$ 
C)  $2 \mathrm { Al } ( \mathrm { OH } ) _ { 3 } + 2 \mathrm { H } ^ { + } \rightarrow 2 \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } + 2 \mathrm { H } _ { 2 }$ 
D)  $2 \mathrm { Al } ( \mathrm { OH } ) _ { 3 } + 2 \mathrm { OH } ^ { - } \rightarrow \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } + 4 \mathrm { H } _ { 2 } \mathrm { O }$ 
E)  $\mathrm { Al } ( \mathrm { OH } ) _ { 3 } \rightarrow \mathrm { Al } ^ { 3 + } + 3 \mathrm { OH } ^ { - }$

Question 12

Ksp is usually expressed in terms of mass of solute per 100mL of solvent.

Accepted Answer

A) True 
 B)False

Question 13

The larger the value of the equilibrium constant, the more stable the product.

Accepted Answer

A) True 
 B)False

Question 14

When Hard water is heated, CO2 gas is released, and the carbonate salts precipitate from solution and produce a solid called _____.

Accepted Answer

Question 15

If a complex ion has a large Kf, the formation of a complex ion can dramatically decrease the solubility of sparingly soluble salts.

Accepted Answer

A) True 
 B)False

Question 16

The formation of an ion pair is a dynamic process.

Accepted Answer

A) True 
 B)False

Question 17

If the Ksp for calcium phosphate [Ca3(PO4)2] at $25.0 ^ { \circ } \mathrm { C }$ is 2.07×10-33,  what is its solubility in 0.500M CaCl2?

Accepted Answer

A)  8.38×10-16 M 
B)  3.62×10-16 M 
C)  1.77×10-16 M 
D)  9.51×10-17 M 
E)  6.43×10-17 M 
A)  8.38×10-16 M 
B)  3.62×10-16 M 
C)  1.77×10-16 M 
D)  9.51×10-17 M 
E)  6.43×10-17 M

Question 18

Which of the following cations is most likely to form base-insoluble hydroxides?

Accepted Answer

A)  Ag+ 
B)  Mg2+ 
C)  Cu2+ 
D)  Al3+ 
E)  Ca2+ 
A)  Ag+ 
B)  Mg2+ 
C)  Cu2+ 
D)  Al3+ 
E)  Ca2+

Question 19

The solubility product of an ionic compound describes the concentrations of _____ in equilibrium with a solid.

Accepted Answer

The answer of The solubility product of an ionic compound...

Question 20

During the formation of a complex ion, the ligand acts as a Lewis acid.

Accepted Answer

A) True 
 B)False

Exam 17: Solubility and Complexation Equilibriums

Which of the following cations is most likely to form insoluble chlorides?

_____ is the universally used compound for developing black-and-white film.

Which of the following cations is most likely to form base-insoluble sulfides?

If the Ksp for zinc carbonate (ZnCO3) is 1.46×10-10 at 25∘C25 ^ { \circ } \mathrm { C }25∘C , what is its aqueous solubility in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

Fe(II) forms the complex ion [Fe(OH)4]2− through equilibrium reactions in which hydroxide replaces water in a stepwise manner. If log K1 = 6.89, log K2 = 5.42, log K3 = −0.36, and log K4 = −1.78, what is its Kf?

Calcium oxalate monohydrate [Ca(O2CCO2).H2O] is a sparingly soluble salt. If its solubility in water at 30∘C30 ^ { \circ } \mathrm { C }30∘C is 8.25×10-4 g/100mL, what is its Ksp?

A molecular solute may be more soluble than predicted by the measured concentrations of ions in solution due to _____.

The formation of ion pairs decreases the solubility of a salt.

Metal ions that precipitate together can be separated by changing the pH of the solution.

If the ion product of a salt exceeds its solubility product, the solution becomes unsaturated.

Which of the following is the chemical equation that describes the dissolution of aluminum hydroxide in a base?

Ksp is usually expressed in terms of mass of solute per 100mL of solvent.

The larger the value of the equilibrium constant, the more stable the product.

When Hard water is heated, CO2 gas is released, and the carbonate salts precipitate from solution and produce a solid called _____.

If a complex ion has a large Kf, the formation of a complex ion can dramatically decrease the solubility of sparingly soluble salts.

The formation of an ion pair is a dynamic process.

If the Ksp for calcium phosphate [Ca3(PO4)2] at 25.0∘C25.0 ^ { \circ } \mathrm { C }25.0∘C is 2.07×10-33, what is its solubility in 0.500M CaCl2?

Which of the following cations is most likely to form base-insoluble hydroxides?

The solubility product of an ionic compound describes the concentrations of _____ in equilibrium with a solid.

During the formation of a complex ion, the ligand acts as a Lewis acid.

Introduction to Chemistry

Molecules, Ions, and Chemical Formulas

Chemical Reactions

Reactions in Aqueous Solution

Energy Changes in Chemical Reactions

The Structure of Atoms

The Periodic Table and Periodic Trends

Ionic Versus Covalent Bonding

Molecular Geometry and Covalent Bonding Models

Gases

Liquids

Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Acidbase Equilibriums

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Periodic Trends and the S-Block Elements

The P-Block Elements

The D-Block Elements

Organic Compounds

Filters

If the K_sp for zinc carbonate (ZnCO₃) is 1.46×10^-1⁰ at $25 ^ { \circ } \mathrm { C }$ , what is its aqueous solubility in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

Fe(II) forms the complex ion [Fe(OH)₄]²⁻ through equilibrium reactions in which hydroxide replaces water in a stepwise manner. If log K₁ = 6.89, log K₂ = 5.42, log K₃ = −0.36, and log K₄ = −1.78, what is its K_f?

Calcium oxalate monohydrate [Ca(O₂CCO₂).H₂O] is a sparingly soluble salt. If its solubility in water at $30 ^ { \circ } \mathrm { C }$ is 8.25×10^-4 g/100mL, what is its K_sp?

K_sp is usually expressed in terms of mass of solute per 100mL of solvent.

When Hard water is heated, CO₂ gas is released, and the carbonate salts precipitate from solution and produce a solid called _____.

If a complex ion has a large K_f, the formation of a complex ion can dramatically decrease the solubility of sparingly soluble salts.

If the K_spfor calcium phosphate [Ca₃(PO₄)₂] at $25.0 ^ { \circ } \mathrm { C }$ is 2.07×10^-33, what is its solubility in 0.500M CaCl₂?