Question 1

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 2

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 3

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

Accepted Answer

A) sodium hydroxide 
B) potassium acetate 
C) hydrochloric acid 
D) sodium fluoride 
E) ammonia 
A) sodium hydroxide 
B) potassium acetate 
C) hydrochloric acid 
D) sodium fluoride 
E) ammonia

Question 4

A result of the common-ion effect is __________.

Accepted Answer

A) that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria 
B) that common ions, such as Na+ (aq), don't affect equilibrium constants 
C) 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 
D) that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00 
E) that common ions precipitate all counter-ions 
A) that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria 
B) that common ions, such as Na+ (aq), don't affect equilibrium constants 
C) 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 
D) that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00 
E) that common ions precipitate all counter-ions

Question 5

Which one of the following will cause hemoglobin to release oxygen?

Accepted Answer

A) increase in pH 
B) decrease in pH 
C) decrease in temperature 
D) decrease in CO2 concentration 
E) increase in O2 concentration 
A) increase in pH 
B) decrease in pH 
C) decrease in temperature 
D) decrease in CO2 concentration 
E) increase in O2 concentration

Question 6

A 25.0 mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of hydrazoic acid is 4.50 × 10-4.

Accepted Answer

A) 11.72 
B) 9.28 
C) 4.72 
D) 7.00 
E) 8.80 
A) 11.72 
B) 9.28 
C) 4.72 
D) 7.00 
E) 8.80

Question 7

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.350 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5.

Accepted Answer

A) 5.137 
B) 4.367 
C) 9.633 
D) 8.781 
E) 8.863 
A) 5.137 
B) 4.367 
C) 9.633 
D) 8.781 
E) 8.863

Question 8

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10-4.

Accepted Answer

Question 9

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

Question 10

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds __________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10-6.

Accepted Answer

A) 5.9 × 10-5 
B) 1.1 × 10-2 
C) 2.4 × 10-8 
D) 2.7 × 10-3 
E) 1.2 × 10-4 
A) 5.9 × 10-5 
B) 1.1 × 10-2 
C) 2.4 × 10-8 
D) 2.7 × 10-3 
E) 1.2 × 10-4

Question 11

Calculate the pH of a solution prepared by dissolving 0.350 mol of benzoic acid (C7H5O2H)and 0.250 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) 4.333 
B) 4.041 
C) 9.959 
D) 9.667 
E) 5.190 
A) 4.333 
B) 4.041 
C) 9.959 
D) 9.667 
E) 5.190

Question 12

The solubility of lead (II)chloride (PbCl2)is 1.6 × 10-2 M. What is the Ksp of PbCl2?

Accepted Answer

A) 5.0 × 10-4 
B) 4.1 × 10-6 
C) 3.1 × 10-7 
D) 1.6 × 10-5 
E) 1.6 × 10-2 
A) 5.0 × 10-4 
B) 4.1 × 10-6 
C) 3.1 × 10-7 
D) 1.6 × 10-5 
E) 1.6 × 10-2

Question 13

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 14

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 15

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 16

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A) 4.90 
B) 50.0 
C) 41.6 
D) 60.1 
E) 4.65 
A) 4.90 
B) 50.0 
C) 41.6 
D) 60.1 
E) 4.65

Question 17

What is the molar solubility of silver chloride (AgCl)in water? The solubility-product constant for AgCl is 1.8 × 10-10 at 25°C.

Accepted Answer

A) 9.0 × 10-11 
B) 3.6 × 10-10 
C) 9.74 
D) 1.9 × 10-5 
E) 1.3 × 10-5 
A) 9.0 × 10-11 
B) 3.6 × 10-10 
C) 9.74 
D) 1.9 × 10-5 
E) 1.3 × 10-5

Question 18

Of the substances below, __________ will decrease the solubility of Pb(OH)2 in a saturated solution.

Accepted Answer

A) NaNO3 
B) H2O2 
C) HNO3 
D) Pb(NO3)2 
E) NaCl 
A) NaNO3 
B) H2O2 
C) HNO3 
D) Pb(NO3)2 
E) NaCl

Question 19

The pH of a solution prepared by mixing 40.0 mL of 0.125 M Mg(OH)2 and 150.0 mL of 0.125 M HCl is __________.

Accepted Answer

A) 6.29 
B) 4.11 
C) 1.14 
D) 5.78 
E) 1.34 
A) 6.29 
B) 4.11 
C) 1.14 
D) 5.78 
E) 1.34

Question 20

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

Exam 17: Additional Aspects of Aqueous Equilibria

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

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.

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

A result of the common-ion effect is __________.

Which one of the following will cause hemoglobin to release oxygen?

A 25.0 mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of hydrazoic acid is 4.50 × 10-4.

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.350 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10-4.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds __________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10-6.

Calculate the pH of a solution prepared by dissolving 0.350 mol of benzoic acid (C7H5O2H)and 0.250 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.

The solubility of lead (II)chloride (PbCl2)is 1.6 × 10-2 M. What is the Ksp of PbCl2?

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.

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

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

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The Ka of butanoic acid is 1.5 × 10-5.

What is the molar solubility of silver chloride (AgCl)in water? The solubility-product constant for AgCl is 1.8 × 10-10 at 25°C.

Of the substances below, __________ will decrease the solubility of Pb(OH)2 in a saturated solution.

The pH of a solution prepared by mixing 40.0 mL of 0.125 M Mg(OH)2 and 150.0 mL of 0.125 M HCl is __________.

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.

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

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

A 25.0 mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_a of hydrazoic acid is 4.50 × 10^-4.

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH₃ and 0.350 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_b of ammonia is 1.77 × 10^-5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The K_a of hydrofluoric acid is 6.80 × 10^-4.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺. When the concentration of F^- exceeds __________ M, BaF₂ will precipitate. Neglect volume changes. For BaF₂, K_sp = 1.7 × 10^-6.

Calculate the pH of a solution prepared by dissolving 0.350 mol of benzoic acid (C₇H₅O₂H)and 0.250 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.

The solubility of lead (II)chloride (PbCl₂)is 1.6 × 10^-2 M. What is the K_sp of PbCl₂?

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.

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5.

What is the molar solubility of silver chloride (AgCl)in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25°C.

Of the substances below, __________ will decrease the solubility of Pb(OH)₂ in a saturated solution.

The pH of a solution prepared by mixing 40.0 mL of 0.125 M Mg(OH)₂ and 150.0 mL of 0.125 M HCl is __________.

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.