Question 1

What is the percent ionization of nitrous acid in a solution that is 0.189 M in nitrous acid? The acid dissociation constant of nitrous acid is

Accepted Answer

A) 0.0450 
B) 8.51 × 10-5 
C) 0.594 
D) 4.20 
E) 4.88 
A) 0.0450 
B) 8.51 × 10-5 
C) 0.594 
D) 4.20 
E) 4.88 E

Question 2

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

Accepted Answer

A) True 
 B)False  True

Question 3

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 A

Question 4

Calculate the percent ionization of formic acid (   H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (   ).The   of formic acid is 1.77 ×   .

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 5

Which of the following could be added to a solution of HC2H3O2 to prepare a buffer?

Accepted Answer

A) HBr 
B) HNO3 
C) KOH 
D) more HC2H3O2 
E) None of the above can be added to an acetic acid solution to prepare a buffer. 
A) HBr 
B) HNO3 
C) KOH 
D) more HC2H3O2 
E) None of the above can be added to an acetic acid solution to prepare a buffer.

Question 6

________ analysis determines how much of a given substance is present.

Accepted Answer

The answer of ________ analysis determines how much of a...

Question 7

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 8

Calculate the maximum concentration (in M)of calcium ions (Ca2+)in a solution that contains   of CO32-.The Ksp of CaCO3 is

Accepted Answer

A) 5.8 × 10-5 
B) 6.8 × 10-9 
C) 3.4 × 10-9 
D) 6.2 × 10-8 
E) 1.9 × 10-10 
A) 5.8 × 10-5 
B) 6.8 × 10-9 
C) 3.4 × 10-9 
D) 6.2 × 10-8 
E) 1.9 × 10-10

Question 9

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

Question 10

A buffer solution with a pH of 4.31 is prepared with   and   The Ka of H       is

Accepted Answer

A) 0.37 
B) 0.74 
C) 4.2 × 10-6 
D) 8.8 × 10-10 
E) 0.18 
A) 0.37 
B) 0.74 
C) 4.2 × 10-6 
D) 8.8 × 10-10 
E) 0.18

Question 11

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 12

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 13

A 25.0 mL sample of 0.723 M HCl   is titrated with a   KOH solution.The     concentration after the addition of   of KOH is ________ M.

Accepted Answer

A) 0.0181 
B) 0.430 
C) 0.723 
D) 0.273 
E) none of the above 
A) 0.0181 
B) 0.430 
C) 0.723 
D) 0.273 
E) none of the above

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

What is the molar solubility of silver carbonate ( Ag2CO3 )in water? The Ksp for Ag2CO3 is 8.1 × 10-12 at

Accepted Answer

A) 1.3 × 10-4 
B) 1.4 × 10-6 
C) 2.0 × 10-4 
D) 4.0 × 10-6 
E) 2.7 × 10-12 
A) 1.3 × 10-4 
B) 1.4 × 10-6 
C) 2.0 × 10-4 
D) 4.0 × 10-6 
E) 2.7 × 10-12

Question 16

CaCO3 is very soluble in the presence of ________.

Accepted Answer

Question 17

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a   NaOH solution.The equivalence point is reached with   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 18

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 19

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 20

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution.The titration curve above was obtained.The unknown compound is ________.

Accepted Answer

A) a strong acid 
B) a strong base 
C) a weak acid 
D) a weak base 
E) neither an acid nor a base 
A) a strong acid 
B) a strong base 
C) a weak acid 
D) a weak base 
E) neither an acid nor a base

Exam 17: Additional Aspects of Aqueous Equilibria

What is the percent ionization of nitrous acid in a solution that is 0.189 M in nitrous acid? The acid dissociation constant of nitrous acid is

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

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

Calculate the percent ionization of formic acid ( H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate ( ).The of formic acid is 1.77 × .

Which of the following could be added to a solution of HC2H3O2 to prepare a buffer?

________ analysis determines how much of a given substance is present.

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.

Calculate the maximum concentration (in M)of calcium ions (Ca2+)in a solution that contains of CO32-.The Ksp of CaCO3 is

The ________ and ________ are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood.

A buffer solution with a pH of 4.31 is prepared with and The Ka of H is

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?

Which compound listed below has the greatest molar solubility in water?

A 25.0 mL sample of 0.723 M HCl is titrated with a KOH solution.The concentration after the addition of of KOH is ________ M.

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

What is the molar solubility of silver carbonate ( Ag2CO3 )in water? The Ksp for Ag2CO3 is 8.1 × 10-12 at

CaCO3 is very soluble in the presence of ________.

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

The Henderson-Hasselbalch equation is ________.

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.

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution.The titration curve above was obtained.The unknown compound is ________.

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

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

Which of the following could be added to a solution of HC₂H₃O₂ to prepare a buffer?

Calculate the maximum concentration (in M)of calcium ions (Ca²⁺)in a solution that contains of CO₃^2-.The K_sp of CaCO₃ is

The and are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood.

What is the molar solubility of silver carbonate ( Ag₂CO₃ )in water? The K_sp for Ag₂CO₃ is 8.1 × 10^-12 at

CaCO₃ is very soluble in the presence of ________.

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