Question 1

In a solution, when the concentrations of a weak acid and its conjugate base are equal,

Accepted Answer

A) the system is not at equilibrium. 
B) the buffering capacity is significantly decreased. 
C) the -log of the [H+] and the -log of the Ka are equal. 
D) all of the above are true. 
A) the system is not at equilibrium. 
B) the buffering capacity is significantly decreased. 
C) the -log of the [H+] and the -log of the Ka are equal. 
D) all of the above are true.

Question 2

An assembly of a metal ion and the Lewis bases bonded to it is called a __________.

Accepted Answer

The answer of An assembly of a metal ion and...

Question 3

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 4

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

Question 5

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is __________ M.

Accepted Answer

A) 0.234 
B) 0.469 
C) 0.150 
D) 0.300 
E) 0.938 
A) 0.234 
B) 0.469 
C) 0.150 
D) 0.300 
E) 0.938

Question 6

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

Question 7

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

Accepted Answer

A) HC6H5O 
B) NaOH 
C) NaCl 
D) C2H5NH2 
E) none of the above 
A) HC6H5O 
B) NaOH 
C) NaCl 
D) C2H5NH2 
E) none of the above

Question 8

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A) 2.83 
B) 1.5 × 10-3 
C) 4.82 
D) 4.00 
E) 1.0 × 104 
A) 2.83 
B) 1.5 × 10-3 
C) 4.82 
D) 4.00 
E) 1.0 × 104

Question 9

In which of the following aqueous solutions would you expect AgCl to have the highest 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 10

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 11

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

Question 12

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

Question 13

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) 55.6 
B) 0.162 
C) 15.5 
D) 2.78 × 10-3 
E) 3.448 
A) 55.6 
B) 0.162 
C) 15.5 
D) 2.78 × 10-3 
E) 3.448

Question 14

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 15

The solubility of manganese (II)hydroxide (Mn(OH)2)is 2.2 × 10-5 M. What is the Ksp of MnOH)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 16

Calculate the percent ionization of formic acid (HCO2H)in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 3.94 × 10-5 
B) 0.0180 
C) 2.84 
D) 0.280 
E) 12.2 
A) 3.94 × 10-5 
B) 0.0180 
C) 2.84 
D) 0.280 
E) 12.2

Question 17

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

Accepted Answer

A) True 
 B)False

Question 18

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 19

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 20

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be __________.

Accepted Answer

The answer of Metal oxides and hydroxides that are relatively...

Exam 17: Additional Aspects of Aqueous Equilibria

In a solution, when the concentrations of a weak acid and its conjugate base are equal,

An assembly of a metal ion and the Lewis bases bonded to it is called a __________.

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.

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

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is __________ M.

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 hydrochloric acid and __________ to water produces a buffer solution.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

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

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

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

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.

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.

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

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

Calculate the percent ionization of formic acid (HCO2H)in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10-4.

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

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

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be __________.

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

A 50.0 mL sample of an aqueous H₂SO₄ solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄ is __________ M.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The K_a of butanoic acid is 1.5 × 10^-5.

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

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

Calculate the percent ionization of formic acid (HCO₂H)in a solution that is 0.219 M in formic acid. The K_a of formic acid is 1.77 × 10^-4.

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.