Question 1

The pH of a solution that contains 0.800 M acetic acid (Ka = 1.76 × 10-5)and 0.172 M sodium acetate is ________.

Accepted Answer

A) 4.087 
B) 5.422 
C) 8.578 
D) 8.370 
E) 9.913 
A) 4.087 
B) 5.422 
C) 8.578 
D) 8.370 
E) 9.913 A

Question 2

Of the following solutions, which has the greatest buffering capacity?

Accepted Answer

A) 0.521 M HC2H3O2 and 0.217 M NaC2H3O2 
B) 0.821 M HC2H3O2 and 0.713 M NaC2H3O2 
C) 0.365M HC2H3O2 and 0.497 M NaC2H3O2 
D) 0.121 M HC2H3O2 and 0.116 M NaC2H3O2 
A) 0.521 M HC2H3O2 and 0.217 M NaC2H3O2 
B) 0.821 M HC2H3O2 and 0.713 M NaC2H3O2 
C) 0.365M HC2H3O2 and 0.497 M NaC2H3O2 
D) 0.121 M HC2H3O2 and 0.116 M NaC2H3O2 B

Question 3

-A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?

Accepted Answer

A) methyl red 
B) bromthymol blue 
C) thymol blue 
D) phenolpthalein 
E) bromocresol purple 
A) methyl red 
B) bromthymol blue 
C) thymol blue 
D) phenolpthalein 
E) bromocresol purple B

Question 4

The addition of sodium hydroxide and ________ to water produces a buffer solution.

Accepted Answer

A) HCl 
B) NaC2H3O2 
C) NaF 
D) NH3 
E) none of the above 
A) HCl 
B) NaC2H3O2 
C) NaF 
D) NH3 
E) none of the above

Question 5

Which of the following could be added to a solution of sodium acetate to produce a buffer?

Accepted Answer

A) acetic acid only 
B) acetic acid or hydrochloric acid 
C) hydrochloric acid only 
D) potassium acetate only 
E) sodium chloride or potassium acetate 
A) acetic acid only 
B) acetic acid or hydrochloric acid 
C) hydrochloric acid only 
D) potassium acetate only 
E) sodium chloride or potassium acetate

Question 6

The Henderson-Hasselbalch equation is ________.

Accepted Answer

A) [H+] = Ka +   
B) pH = pKa - log   
C) pH = pKa + log   
D) pH = pKa + log   
E) pH = log   
A) [H+] = Ka +   
B) pH = pKa - log   
C) pH = pKa + log   
D) pH = pKa + log   
E) pH = log

Question 7

Which is the correct Ksp expression for PbCl2 (s)dissolving in water?

Accepted Answer

A) Ksp = [Pb2+] [Cl-]2 
B) Ksp = [Pb2+] [Cl-] 
C) Ksp = [Pb2+]2 [Cl-] 
D) Ksp = [PbCl+] [Cl-] 
E) Ksp = [Pb+] [Cl2-]2 
A) Ksp = [Pb2+] [Cl-]2 
B) Ksp = [Pb2+] [Cl-] 
C) Ksp = [Pb2+]2 [Cl-] 
D) Ksp = [PbCl+] [Cl-] 
E) Ksp = [Pb+] [Cl2-]2

Question 8

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of KOH is ________ M.

Accepted Answer

A) 0.4 
B) 1 × 10-7 
C) 0.7 
D) 3 × 10-13 
E) 4 × 10-2 
A) 0.4 
B) 1 × 10-7 
C) 0.7 
D) 3 × 10-13 
E) 4 × 10-2

Question 9

The Ksp for Zn(OH)2 is 5.0 × 10-17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.

Accepted Answer

A) 5.0 × 106 
B) 1.2 × 10-12 
C) 1.6 × 10-14 
D) 5.0 × 10-12 
E) 5.0 × 10-17 
A) 5.0 × 106 
B) 1.2 × 10-12 
C) 1.6 × 10-14 
D) 5.0 × 10-12 
E) 5.0 × 10-17

Question 10

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

Accepted Answer

A) True 
 B)False

Question 11

Consider the following table of   values.  
-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 12

Which one of the following pairs cannot be mixed together to form a buffer solution?

Accepted Answer

A) NH3, NH4Cl 
B) NaC2H3O2, HCl (C2H3O2- = acetate) 
C) RbOH, HBr 
D) KOH, HF 
E) H3PO4, KH2PO4 
A) NH3, NH4Cl 
B) NaC2H3O2, HCl (C2H3O2- = acetate) 
C) RbOH, HBr 
D) KOH, HF 
E) H3PO4, KH2PO4

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

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

Accepted Answer

A) True 
 B)False

Question 15

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO3 is ________.

Accepted Answer

A) 13.29 
B) 7.00 
C) 8.11 
D) 11.00 
E) 12.14 
A) 13.29 
B) 7.00 
C) 8.11 
D) 11.00 
E) 12.14

Question 16

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

Accepted Answer

A) NaF 
B) HF 
C) NaNO3 
D) NaBr 
E) KI 
A) NaF 
B) HF 
C) NaNO3 
D) NaBr 
E) KI

Question 17

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 10.2 mL of the base is added. The concentration of acetic acid in the sample was ________ M.

Accepted Answer

A) 0.365 
B) 0.175 
C) 0.119 
D) 0.0714 
E) none of the above 
A) 0.365 
B) 0.175 
C) 0.119 
D) 0.0714 
E) none of the above

Question 18

Of the following solutions, which has the greatest buffering capacity?

Accepted Answer

A) 0.543 M NH3 and 0.555 M NH4Cl 
B) 0.087 M NH3 and 0.088 M NH4Cl 
C) 0.234 M NH3 and 0.100 M NH4Cl 
D) 0.100 M NH3 and 0.455 M NH4Cl 
E) They are all buffer solutions and would all have the same capacity. 
A) 0.543 M NH3 and 0.555 M NH4Cl 
B) 0.087 M NH3 and 0.088 M NH4Cl 
C) 0.234 M NH3 and 0.100 M NH4Cl 
D) 0.100 M NH3 and 0.455 M NH4Cl 
E) They are all buffer solutions and would all have the same capacity.

Question 19

In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?

Accepted Answer

A) 0.020 M BaCl2 
B) 0.020 M Pb(NO3)2 
C) 0.020 M NaCl 
D) 0.020 M KCl 
E) pure water 
A) 0.020 M BaCl2 
B) 0.020 M Pb(NO3)2 
C) 0.020 M NaCl 
D) 0.020 M KCl 
E) pure water

Question 20

Of the following solutions, which has the greatest buffering capacity?

Accepted Answer

A) 1.15 M HF and 0.624 M NaF 
B) 0.574 M HF and 0.312 M NaF 
C) 0.287 M HF and 0.156 M NaF 
D) 0.189 M HF and 0.103 M NaF 
E) They are all buffer solutions and would all have the same capacity. 
A) 1.15 M HF and 0.624 M NaF 
B) 0.574 M HF and 0.312 M NaF 
C) 0.287 M HF and 0.156 M NaF 
D) 0.189 M HF and 0.103 M NaF 
E) They are all buffer solutions and would all have the same capacity.

Exam 17: Additional Aspects of Aqueous Equilibria

The pH of a solution that contains 0.800 M acetic acid (Ka = 1.76 × 10-5)and 0.172 M sodium acetate is ________.

Of the following solutions, which has the greatest buffering capacity?

-A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?

The addition of sodium hydroxide and ________ to water produces a buffer solution.

Which of the following could be added to a solution of sodium acetate to produce a buffer?

The Henderson-Hasselbalch equation is ________.

Which is the correct Ksp expression for PbCl2 (s)dissolving in water?

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of KOH is ________ M.

The Ksp for Zn(OH)2 is 5.0 × 10-17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

Consider the following table of values. -Which compound listed below has the greatest molar solubility in water?

Which one of the following pairs cannot be mixed together to form a buffer solution?

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.

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO3 is ________.

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

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 10.2 mL of the base is added. The concentration of acetic acid in the sample was ________ M.

Of the following solutions, which has the greatest buffering capacity?

In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?

Of the following solutions, which has the greatest buffering capacity?

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

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

The pH of a solution that contains 0.800 M acetic acid (K_a = 1.76 × 10^-⁵)and 0.172 M sodium acetate is ________.

Which is the correct K_sp expression for PbCl₂ (s)dissolving in water?

A 25.0 mL sample of 0.723 M HClO₄ is titrated with a 0.27 M KOH solution. The H₃O⁺ concentration after the addition of 80.0 mL of KOH is ________ M.

The K_sp for Zn(OH)₂ is 5.0 × 10^-17. Determine the molar solubility of Zn(OH)₂ in a buffer solution with a pH of 11.5.

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.

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO₃ is ________.

In which of the following aqueous solutions would you expect PbCl₂ to have the lowest solubility?