Question 1

Which below best describe(s)the behavior of an amphoteric hydroxide in water?

Accepted Answer

A) With conc. aq. NaOH, its suspension dissolves. 
B) With conc. aq. HCl, its suspension dissolves. 
C) With conc. aq. NaOH, its clear solution forms a precipitate. 
D) With conc. aq. HCl, its clear solution forms a precipitate. 
E) With both conc. aq. NaOH and conc. aq. HCl, its suspension dissolves. 
A) With conc. aq. NaOH, its suspension dissolves. 
B) With conc. aq. HCl, its suspension dissolves. 
C) With conc. aq. NaOH, its clear solution forms a precipitate. 
D) With conc. aq. HCl, its clear solution forms a precipitate. 
E) With both conc. aq. NaOH and conc. aq. HCl, its suspension dissolves.

Question 2

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 4.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M.

Accepted Answer

A) 0.0862 
B) 0.0876 
C) 0.0980 
D) 0.0848 
E) 0.00253 
A) 0.0862 
B) 0.0876 
C) 0.0980 
D) 0.0848 
E) 0.00253

Question 3

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Accepted Answer

A) pure water 
B) 0.020 M BaCl2 
C) 0.015 NaCl 
D) 0.020 AgNO3 
E) 0.020 KCl 
A) pure water 
B) 0.020 M BaCl2 
C) 0.015 NaCl 
D) 0.020 AgNO3 
E) 0.020 KCl

Question 4

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A) 1.12 × 10-4 
B) 0.0450 
C) 4.25 
D) 0.342 
E) 5.53 
A) 1.12 × 10-4 
B) 0.0450 
C) 4.25 
D) 0.342 
E) 5.53

Question 5

Which one of the following is not amphoteric?

Accepted Answer

A) Al(OH)3 
B) Ca(OH)2 
C) Cr(OH)3 
D) Zn(OH)2 
E) Sn(OH)2 
A) Al(OH)3 
B) Ca(OH)2 
C) Cr(OH)3 
D) Zn(OH)2 
E) Sn(OH)2

Question 6

The addition of hydrochloric acid and __________ to water produces a buffer solution.

Accepted Answer

A) HC6H5O 
B) NaOH 
C) NH3 
D) HNO3 
E) NaNO3 
A) HC6H5O 
B) NaOH 
C) NH3 
D) HNO3 
E) NaNO3

Question 7

Which compound listed below has the greatest molar solubility in water?

Accepted Answer

A) CdCO3 
B) Cd(OH)2 
C) AgI 
D) CaF2 
E) ZnCO3 
A) CdCO3 
B) Cd(OH)2 
C) AgI 
D) CaF2 
E) ZnCO3

Question 8

The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is __________.

Accepted Answer

A) 6.29 
B) 7.00 
C) 8.11 
D) 5.78 
E) 0.00 
A) 6.29 
B) 7.00 
C) 8.11 
D) 5.78 
E) 0.00

Question 9

The pH of a solution prepared by mixing 55.0 mL of 0.183 M KOH and 30.0 mL of 0.145 M HC2H3O2 is __________.

Accepted Answer

A) 9.97 
B) 7.74 
C) 1.172 
D) 12.828 
E) none of the above 
A) 9.97 
B) 7.74 
C) 1.172 
D) 12.828 
E) none of the above

Question 10

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH3NH3Cl)in 1.00 L of 1.10 M methylamine (CH3NH2)is __________. The Kb for methylamine is 4.40 × 10-4. (Assume the final volume is 1.00 L.)

Accepted Answer

A) 1.66 
B) 2.86 
C) 10.28 
D) 11.14 
E) 10.61 
A) 1.66 
B) 2.86 
C) 10.28 
D) 11.14 
E) 10.61

Question 11

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO2H)and 0.230 mol of sodium formate (NaCO2H)in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 2.099 
B) 10.318 
C) 3.682 
D) 2.307 
E) 3.952 
A) 2.099 
B) 10.318 
C) 3.682 
D) 2.307 
E) 3.952

Question 12

Which compound listed below has the smallest molar solubility in water?

Accepted Answer

A) ZnCO3 
B) Cd(OH)2 
C) CdCO3 
D) AgI 
E) CaF2 
A) ZnCO3 
B) Cd(OH)2 
C) CdCO3 
D) AgI 
E) CaF2

Question 13

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.30 × 10-5.

Accepted Answer

A) 2.516 
B) 3.892 
C) 4.502 
D) 10.158 
E) 4.195 
A) 2.516 
B) 3.892 
C) 4.502 
D) 10.158 
E) 4.195

Question 14

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Accepted Answer

A) 14.28 
B) 10.43 
C) 5.48 
D) 3.57 
E) 4.13 
A) 14.28 
B) 10.43 
C) 5.48 
D) 3.57 
E) 4.13

Question 15

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

Accepted Answer

A) True 
 B)False

Question 16

The addition of hydrofluoric acid and __________ to water produces a buffer solution.

Accepted Answer

A) HCl 
B) NaNO3 
C) NaF 
D) NaCl 
E) NaBr 
A) HCl 
B) NaNO3 
C) NaF 
D) NaCl 
E) NaBr

Question 17

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

Accepted Answer

A) pure water 
B) 0.20 M NaBr 
C) 0.10 M AgNO3 
D) 0.15 M KBr 
E) 0.10 M LiBr 
A) pure water 
B) 0.20 M NaBr 
C) 0.10 M AgNO3 
D) 0.15 M KBr 
E) 0.10 M LiBr

Question 18

Which of the following could be added to a solution of acetic acid to prepare a buffer?

Accepted Answer

A) sodium hydroxide 
B) hydrochloric acid 
C) nitric acid 
D) more acetic acid 
E) None of the above can be added to an acetic acid solution to prepare a buffer. 
A) sodium hydroxide 
B) hydrochloric acid 
C) nitric acid 
D) more acetic acid 
E) None of the above can be added to an acetic acid solution to prepare a buffer.

Question 19

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 8.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M.

Accepted Answer

A) 0.0979 
B) 0.0930 
C) 0.129 
D) 0.123 
E) 0.00976 
A) 0.0979 
B) 0.0930 
C) 0.129 
D) 0.123 
E) 0.00976

Question 20

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

Exam 17: Additional Aspects of Aqueous Equilibria

Which below best describe(s)the behavior of an amphoteric hydroxide in water?

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 4.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M.

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Which one of the following is not amphoteric?

The addition of hydrochloric acid and __________ to water produces a buffer solution.

Which compound listed below has the greatest molar solubility in water?

The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is __________.

The pH of a solution prepared by mixing 55.0 mL of 0.183 M KOH and 30.0 mL of 0.145 M HC2H3O2 is __________.

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH3NH3Cl)in 1.00 L of 1.10 M methylamine (CH3NH2)is __________. The Kb for methylamine is 4.40 × 10-4. (Assume the final volume is 1.00 L.)

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO2H)and 0.230 mol of sodium formate (NaCO2H)in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10-4.

Which compound listed below has the smallest molar solubility in water?

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.30 × 10-5.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

The addition of hydrofluoric acid and __________ to water produces a buffer solution.

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

Which of the following could be added to a solution of acetic acid to prepare a buffer?

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 8.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10-5.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

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Molecular Geometry and Bonding Theories

Gases

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Chemistry of the Environment

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Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

The pH of a solution prepared by mixing 55.0 mL of 0.183 M KOH and 30.0 mL of 0.145 M HC₂H₃O₂ is __________.

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH₃NH₃Cl)in 1.00 L of 1.10 M methylamine (CH₃NH₂)is __________. The K_b for methylamine is 4.40 × 10^-4. (Assume the final volume is 1.00 L.)

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO₂H)and 0.230 mol of sodium formate (NaCO₂H)in water sufficient to yield 1.00 L of solution. The K_a of formic acid is 1.77 × 10^-4.

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K_a of benzoic acid is 6.30 × 10^-5.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The K_a of acetic acid is 1.77 × 10^-5.