Question 1

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

Accepted Answer

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

Question 2

In which one of the following solutions is silver chloride the most soluble?

Accepted Answer

A)  0.744 M LiNO3 
B)  0.181 M HCl 
C)  0.181 M NaCl 
D)  0.0176 M NH3 
E)  pure water 
A)  0.744 M LiNO3 
B)  0.181 M HCl 
C)  0.181 M NaCl 
D)  0.0176 M NH3 
E)  pure water

Question 3

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

Question 4

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is
4)50 × 10- 4.

Accepted Answer

A)  2.78 × 10- 3 
B)  55.6 
C)  0.161 
D)  15.5 
E)  3.448 
A)  2.78 × 10- 3 
B)  55.6 
C)  0.161 
D)  15.5 
E)  3.448

Question 5

The Ka of acetic acid is 1.76 × 10- 5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is _ .

Accepted Answer

A)  0.85 
B)  2.38 
C)  4.77 
D)  1.70 
E)  3.40 
A)  0.85 
B)  2.38 
C)  4.77 
D)  1.70 
E)  3.40

Question 6

A solution is prepared by dissolving 0.23 mol of chloroacetic acid and 0.27 mol of sodium chloroacetate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the _ present in the buffer solution. The Ka of chloroacetic acid is 1.36 × 10- 3.

Accepted Answer

A)  H3O+ 
B)  chloroacetic acid 
C)  H2O 
D)  This is a buffer solution:
The pH does not change upon addition of acid or base. 
E)  chloroacetate ion 
A)  H3O+ 
B)  chloroacetic acid 
C)  H2O 
D)  This is a buffer solution:
The pH does not change upon addition of acid or base. 
E)  chloroacetate ion

Question 7

Which one of the following is not amphoteric?

Accepted Answer

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

Question 8

The common- ion effect refers to the observation _ .

Accepted Answer

A)  ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00 
B)  that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X- ) that produces a compound (AgX) with a very low solubility 
C)  that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria 
D)  common ions, such as Na+ (aq), don't affect equilibrium constants 
E)  that common ions precipitate all counter- ions 
A)  ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00 
B)  that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X- ) that produces a compound (AgX) with a very low solubility 
C)  that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria 
D)  common ions, such as Na+ (aq), don't affect equilibrium constants 
E)  that common ions precipitate all counter- ions

Question 9

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 66.2 mL of KOH is M.

Accepted Answer

A)  0.439 
B)  2.81 × 10- 13 
C)  0.273 
D)  0.723 
E)  1.00 × 10- 7 
A)  0.439 
B)  2.81 × 10- 13 
C)  0.273 
D)  0.723 
E)  1.00 × 10- 7

Question 10

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

Accepted Answer

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

Question 11

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO2). The Ka of formic acid is 1.77 ×10- 4.

Accepted Answer

A)  0.0952 
B)  1.06 × 10- 3 
C)  11.3 
D)  3.529 
E)  37.8 
A)  0.0952 
B)  1.06 × 10- 3 
C)  11.3 
D)  3.529 
E)  37.8

Question 12

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.

Accepted Answer

A)  2.86 
B)  1.66 
C)  11.1 
D)  10.6 
E)  10.2 
A)  2.86 
B)  1.66 
C)  11.1 
D)  10.6 
E)  10.2

Question 13

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO) and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.81 × 10- 8.

Accepted Answer

A)  7.30 
B)  7.54 
C)  8.49 
D)  6.46 
E)  13.88 
A)  7.30 
B)  7.54 
C)  8.49 
D)  6.46 
E)  13.88

Question 14

What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?

Accepted Answer

A)  The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase. 
B)  The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase. 
C)  The concentration of hydronium ions will increase significantly. 
D)  The fluoride ions will precipitate out of solution as its acid salt. 
E)  The concentration of fluoride ions will increase as will the concentration of hydronium ions. 
A)  The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase. 
B)  The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase. 
C)  The concentration of hydronium ions will increase significantly. 
D)  The fluoride ions will precipitate out of solution as its acid salt. 
E)  The concentration of fluoride ions will increase as will the concentration of hydronium ions.

Question 15

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

Accepted Answer

A) True 
 B)False

Question 16

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

Question 17

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is M.

Accepted Answer

A)  1.00 × 10- 7 
B)  0.273 
C)  0.723 
D)  0.440 
E)  2.81 × 10- 13 
A)  1.00 × 10- 7 
B)  0.273 
C)  0.723 
D)  0.440 
E)  2.81 × 10- 13

Question 18

A 25.0- mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hydrazoic acid is 1.9 × 10- 5.

Accepted Answer

A)  4.66 
B)  4.78 
C)  3.03 
D)  1.34 
E)  4.45 
A)  4.66 
B)  4.78 
C)  3.03 
D)  1.34 
E)  4.45

Question 19

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.01 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10- 5.

Accepted Answer

Question 20

Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 ×
10- 4 M.

Accepted Answer

A)  3.9 × 10- 8 
B)  1.1 × 10- 11 
C)  2.7 × 10- 12 
D)  1.4 × 10- 4 
E)  2.0 × 10- 8 
A)  3.9 × 10- 8 
B)  1.1 × 10- 11 
C)  2.7 × 10- 12 
D)  1.4 × 10- 4 
E)  2.0 × 10- 8

Exam 17: Additional Aspects of Equilibria

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

In which one of the following solutions is silver chloride the most soluble?

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.

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4)50 × 10- 4.

The Ka of acetic acid is 1.76 × 10- 5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is _ .

Which one of the following is not amphoteric?

The common- ion effect refers to the observation _ .

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 66.2 mL of KOH is M.

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

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO2). The Ka of formic acid is 1.77 ×10- 4.

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.

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO) and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.81 × 10- 8.

What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?

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

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

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is M.

A 25.0- mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hydrazoic acid is 1.9 × 10- 5.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.01 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10- 5.

Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 × 10- 4 M.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

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

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

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.

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂) and 0.278 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4)50 × 10^-⁴.

The K_aof acetic acid is 1.76 × 10^-⁵. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is _ .

A 25.0 mL sample of 0.723 M HClO₄is titrated with a 0.273 M KOH solution. The H₃O⁺ concentration after the addition of 66.2 mL of KOH is M.

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO₂). The K_aof formic acid is 1.77 ×10^-⁴.

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_bfor methylamine is 4.40 × 10^-⁴.

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO) and 0.333 M in sodium hypochlorite? The K_aof hypochlorous acid is 3.81 × 10^-⁸.

A 25.0 mL sample of 0.723 M HClO₄is titrated with a 0.273 M KOH solution. The H₃O⁺ concentration after the addition of 10.0 mL of KOH is M.

A 25.0- mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The K_aof hydrazoic acid is 1.9 × 10^-⁵.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.01 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10^-⁵.

Determine the K_spfor magnesium hydroxide (Mg(OH)₂) where the solubility of Mg(OH)₂is 1.4 × 10^-⁴M.