Question 1

The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 × 10-17.

Accepted Answer

A) 3.8 × 10-11 
B) 3.0 × 10-10 
C) 9.1 × 10-9 
D) 3.5 × 10-9 
E) 1.4 × 10-8 
A) 3.8 × 10-11 
B) 3.0 × 10-10 
C) 9.1 × 10-9 
D) 3.5 × 10-9 
E) 1.4 × 10-8

Question 2

A solution containing which one of the following pairs of substances will be a buffer solution?

Accepted Answer

A) KI, HI 
B) AgBr, HBr 
C) CuCl, HCl 
D) CsI, HI 
E) none of the above 
A) KI, HI 
B) AgBr, HBr 
C) CuCl, HCl 
D) CsI, HI 
E) none of the above

Question 3

What is the solubility (in M)of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10-5.

Accepted Answer

A) 2.0 × 10-3 
B) 1.1 × 10-4 
C) 1.8 × 10-4 
D) 7.1 × 10-4 
E) 1.6 × 10-5 
A) 2.0 × 10-3 
B) 1.1 × 10-4 
C) 1.8 × 10-4 
D) 7.1 × 10-4 
E) 1.6 × 10-5

Question 4

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

Accepted Answer

A) 0.040 M SrBr2 
B) pure water 
C) 0.040 M NaBr 
D) 0.040 M KBr 
E) 0.010 M AgNO3 
A) 0.040 M SrBr2 
B) pure water 
C) 0.040 M NaBr 
D) 0.040 M KBr 
E) 0.010 M AgNO3

Question 5

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

Accepted Answer

A) 0.0953 
B) 0.0900 
C) 0.130 
D) 0.122 
E) 0.00976 
A) 0.0953 
B) 0.0900 
C) 0.130 
D) 0.122 
E) 0.00976

Question 6

The solubility of manganese (II)hydroxide (Mn(OH)2)is 2.2 × 10-5 M. What is the Ksp of Mn(OH)2?

Accepted Answer

A) 1.1 × 10-14 
B) 4.3 × 10-14 
C) 2.1 × 10-14 
D) 4.8 × 10-10 
E) 2.2 × 10-5 
A) 1.1 × 10-14 
B) 4.3 × 10-14 
C) 2.1 × 10-14 
D) 4.8 × 10-10 
E) 2.2 × 10-5

Question 7

Calculate the percent ionization of formic acid (HCO2H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO2). The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 35.6 
B) 0.1011 
C) 10.8 
D) 1.03 × 10-3 
E) 3.488 
A) 35.6 
B) 0.1011 
C) 10.8 
D) 1.03 × 10-3 
E) 3.488

Question 8

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H)and 0.150 mol of sodium benzoate (NaC7H5O2)in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10-5.

Accepted Answer

A) 4.409 
B) 3.965 
C) 10.035 
D) 9.591 
E) 5.190 
A) 4.409 
B) 3.965 
C) 10.035 
D) 9.591 
E) 5.190

Question 9

Calculate the percent ionization of nitrous acid in a solution that is 0.260 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A) 1.17 × 10-4 
B) 0.0450 
C) 4.16 
D) 0.314 
E) 5.78 
A) 1.17 × 10-4 
B) 0.0450 
C) 4.16 
D) 0.314 
E) 5.78

Question 10

What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood?

Accepted Answer

A) kidneys, liver 
B) lungs, kidneys 
C) spleen, liver 
D) lungs, skin 
E) brain stem, heart 
A) kidneys, liver 
B) lungs, kidneys 
C) spleen, liver 
D) lungs, skin 
E) brain stem, heart

Question 11

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF2 is 1.7 × 10-6.

Accepted Answer

A) 3.8 × 10-4 
B) 3.0 × 10-3 
C) 1.5 × 10-2 
D) 7.5 × 10-3 
E) 1.4 × 10-4 
A) 3.8 × 10-4 
B) 3.0 × 10-3 
C) 1.5 × 10-2 
D) 7.5 × 10-3 
E) 1.4 × 10-4

Question 12

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

Accepted Answer

A) pure water 
B) 0.050 M BaI2 
C) 0.050 M NaI 
D) 0.050 M KI 
E) 0.010 M AgNO3 
A) pure water 
B) 0.050 M BaI2 
C) 0.050 M NaI 
D) 0.050 M KI 
E) 0.010 M AgNO3

Question 13

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH3)2NH2Cl)in 1.00 L of 1.10 M dimethylamine ((CH3)2NH)is ________. The Kb for methylamine is 5.40 × 10-4. (Assume the final volume is 1.00 L.)

Accepted Answer

A) 1.66 
B) 2.77 
C) 11.23 
D) 11.14 
E) none of the above 
A) 1.66 
B) 2.77 
C) 11.23 
D) 11.14 
E) none of the above

Question 14

Calculate the maximum concentration (in M)of silver ions (Ag+)in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1 × 10-12.

Accepted Answer

A) 1.8 × 10-5 
B) 1.4 × 10-6 
C) 2.8 × 10-6 
D) 3.2 × 10-10 
E) 8.1 × 10-12 
A) 1.8 × 10-5 
B) 1.4 × 10-6 
C) 2.8 × 10-6 
D) 3.2 × 10-10 
E) 8.1 × 10-12

Question 15

Consider the following table of   values.  
-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 16

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is ________ M.

Accepted Answer

A) 11.7 
B) 0.00214 
C) 0.0856 
D) 0.267 
E) 0.139 
A) 11.7 
B) 0.00214 
C) 0.0856 
D) 0.267 
E) 0.139

Question 17

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

Accepted Answer

A) 0.0735 
B) 0.0762 
C) 0.0980 
D) 0.0709 
E) 0.00253 
A) 0.0735 
B) 0.0762 
C) 0.0980 
D) 0.0709 
E) 0.00253

Question 18

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

Accepted Answer

A) HONH2, HONH3Cl 
B) NaCl, HCl 
C) RbOH, HF 
D) KOH, HNO2 
E) H2SO3, KHSO3 
A) HONH2, HONH3Cl 
B) NaCl, HCl 
C) RbOH, HF 
D) KOH, HNO2 
E) H2SO3, KHSO3

Question 19

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

Accepted Answer

A) sodium acetate only 
B) sodium acetate or sodium hydroxide 
C) nitric acid only 
D) hydrofluoric acid or nitric acid 
E) sodium hydroxide only 
A) sodium acetate only 
B) sodium acetate or sodium hydroxide 
C) nitric acid only 
D) hydrofluoric acid or nitric acid 
E) sodium hydroxide only

Question 20

Calculate the maximum concentration (in M)of magnesium ions (Mg+2)in a solution that contains 0.025 M of CO32-. The Ksp of MgCO3 is 3.5 × 10-8.

Accepted Answer

A) 1.8 × 10-5 
B) 1.4 × 10-6 
C) 2.8 × 10-6 
D) 3.2 × 10-10 
E) 8.1 × 10-12 
A) 1.8 × 10-5 
B) 1.4 × 10-6 
C) 2.8 × 10-6 
D) 3.2 × 10-10 
E) 8.1 × 10-12

Exam 17: Additional Aspects of Aqueous Equilibria

The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 × 10-17.

A solution containing which one of the following pairs of substances will be a buffer solution?

What is the solubility (in M)of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10-5.

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

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

The solubility of manganese (II)hydroxide (Mn(OH)2)is 2.2 × 10-5 M. What is the Ksp of Mn(OH)2?

Calculate the percent ionization of formic acid (HCO2H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO2). The Ka of formic acid is 1.77 × 10-4.

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H)and 0.150 mol of sodium benzoate (NaC7H5O2)in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10-5.

Calculate the percent ionization of nitrous acid in a solution that is 0.260 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood?

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF2 is 1.7 × 10-6.

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

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH3)2NH2Cl)in 1.00 L of 1.10 M dimethylamine ((CH3)2NH)is ________. The Kb for methylamine is 5.40 × 10-4. (Assume the final volume is 1.00 L.)

Calculate the maximum concentration (in M)of silver ions (Ag+)in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1 × 10-12.

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

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is ________ M.

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

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

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

Calculate the maximum concentration (in M)of magnesium ions (Mg+2)in a solution that contains 0.025 M of CO32-. The Ksp of MgCO3 is 3.5 × 10-8.

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

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The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 × 10^-1⁷.

What is the solubility (in M)of PbCl₂ in a 0.15 M solution of HCl? The K_sp of PbCl₂ is 1.6 × 10^-5.

The solubility of manganese (II)hydroxide (Mn(OH)₂)is 2.2 × 10^-5 M. What is the K_sp of Mn(OH)₂?

Calculate the percent ionization of formic acid (HCO₂H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO₂). The K_a of formic acid is 1.77 × 10^-4.

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C₇H₅O₂H)and 0.150 mol of sodium benzoate (NaC₇H₅O₂)in water sufficient to yield 1.00 L of solution. The K_a of benzoic acid is 6.50 × 10^-5.

Calculate the percent ionization of nitrous acid in a solution that is 0.260 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF₂ is 1.7 × 10^-⁶.

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH₃)₂NH₂Cl)in 1.00 L of 1.10 M dimethylamine ((CH₃)₂NH)is ________. The K_b for methylamine is 5.40 × 10^-4. (Assume the final volume is 1.00 L.)

Calculate the maximum concentration (in M)of silver ions (Ag⁺)in a solution that contains 0.025 M of CO₃^2-. The K_sp of Ag₂CO₃ is 8.1 × 10^-12.

Calculate the maximum concentration (in M)of magnesium ions (Mg⁺²)in a solution that contains 0.025 M of CO₃^2-. The K_sp of MgCO₃ is 3.5 × 10^-8.