Question 1

Amphoteric oxides are compounds that exhibit both acidic and basic behavior.

Accepted Answer

A) True 
 B)False  True

Question 2

What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

Accepted Answer

A)  2.34 × 10-4 M 
B)  2.29 × 10-6 M 
C)  4.37 × 10-9 M 
D)  4.27 × 10-11 M 
E)  8.360 M 
A)  2.34 × 10-4 M 
B)  2.29 × 10-6 M 
C)  4.37 × 10-9 M 
D)  4.27 × 10-11 M 
E)  8.360 M C

Question 3

Weak acids have weak conjugate bases.

Accepted Answer

A) True 
 B)False  False

Question 4

A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

Accepted Answer

A)  0.64 
B)  0.94 
C)  1.13 
D)  2.16 
E)  -0.097 
A)  0.64 
B)  0.94 
C)  1.13 
D)  2.16 
E)  -0.097

Question 5

In the reaction CaO(s) + SO2(g)   CaSO3(s),

Accepted Answer

A)  O2- acts as a Lewis base, and SO2 acts as a Lewis acid. 
B)  Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid. 
C)  SO32- acts as a Lewis base, and SO2 acts as a Lewis acid. 
D)  SO2 acts as a Lewis base, and O2- acts as a Lewis acid. 
E)  SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid. 
A)  O2- acts as a Lewis base, and SO2 acts as a Lewis acid. 
B)  Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid. 
C)  SO32- acts as a Lewis base, and SO2 acts as a Lewis acid. 
D)  SO2 acts as a Lewis base, and O2- acts as a Lewis acid. 
E)  SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid.

Question 6

Which is a basic oxide?

Accepted Answer

A)  CO2 
B)  CaO 
C)  SO2 
D)  H2O 
E)  NO2 
A)  CO2 
B)  CaO 
C)  SO2 
D)  H2O 
E)  NO2

Question 7

Which of the following salts will form an acidic solution when dissolved in water?

Accepted Answer

A)  NaCl 
B)  NaNO2 
C)  NH4NO3 
D)  NH4CN 
E)  More than one of the compounds listed will form an acidic solution 
A)  NaCl 
B)  NaNO2 
C)  NH4NO3 
D)  NH4CN 
E)  More than one of the compounds listed will form an acidic solution

Question 8

List the components in an oxoacid.

Accepted Answer

hydrogen,

Question 9

Which is a Lewis base?

Accepted Answer

A)  BCl3 
B)  Cu2+ 
C)  Cl- 
D)  Mn2+ 
E)  NH4+ 
A)  BCl3 
B)  Cu2+ 
C)  Cl- 
D)  Mn2+ 
E)  NH4+

Question 10

In comparing three solutions with pHs of 2.0, 4.8, and 5.2, which solution is the most acidic?

Accepted Answer

The soluti

Question 11

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2-) = 1.5 × 10-10

Accepted Answer

A)  0.38 
B)  12.00 
C)  10.91 
D)  8.09 
E)  13.62 
A)  0.38 
B)  12.00 
C)  10.91 
D)  8.09 
E)  13.62

Question 12

What is the conjugate acid of CO32- in the reaction below? CO32- + HSO4-   HCO3- + SO42-

Accepted Answer

A)  HCO3- 
B)  HSO4- 
C)  OH- 
D)  H3O+ 
E)  SO42- 
A)  HCO3- 
B)  HSO4- 
C)  OH- 
D)  H3O+ 
E)  SO42-

Question 13

What is the conjugate base of water?

Accepted Answer

A)  H3O+ 
B)  OH- 
C)  H3O 
D)  OH 
E)  H2O2 
A)  H3O+ 
B)  OH- 
C)  H3O 
D)  OH 
E)  H2O2

Question 14

A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this acid?

Accepted Answer

A)  7.2 × 101 
B)  1.6 × 10-1 
C)  9.9 × 10-2 
D)  1.4 × 10-3 
E)  2.7 × 10-4 
A)  7.2 × 101 
B)  1.6 × 10-1 
C)  9.9 × 10-2 
D)  1.4 × 10-3 
E)  2.7 × 10-4

Question 15

Which is the correct statement?

Accepted Answer

A)  A polyprotic acid has more than two ionizable protons. 
B)  H2O is a diprotic acid. 
C)  All protons are lost from a polyprotic acid at the same time. 
D)  NH3 is a diprotic acid. 
E)  NH3 is a polyprotic acid. 
A)  A polyprotic acid has more than two ionizable protons. 
B)  H2O is a diprotic acid. 
C)  All protons are lost from a polyprotic acid at the same time. 
D)  NH3 is a diprotic acid. 
E)  NH3 is a polyprotic acid.

Question 16

A solution is prepared by adding 0.10 mol of sodium fluoride, NaF, to 1.00 L of water. Which statement about the solution is correct?

Accepted Answer

A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is acidic. 
D)  The concentrations of fluoride ions and sodium ions are equal. 
E)  The concentrations of hydronium ions and hydroxide ions are equal. 
A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is acidic. 
D)  The concentrations of fluoride ions and sodium ions are equal. 
E)  The concentrations of hydronium ions and hydroxide ions are equal.

Question 17

Which represents a weak base B with Kb= 2 ×10-3? (Each circle represents 1.0 ×10-3 mol of atoms, and the volume of each box is 1.0 L. Solvent water molecules are not shown for clarity.)

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 18

Find the pH of a 0.20 M aqueous solution of dichloroacetic acid, for which Ka = 3.32 × 10-2.

Accepted Answer

A)  0.75 
B)  2.71 
C)  1.05 
D)  2.35 
E)  1.18 
A)  0.75 
B)  2.71 
C)  1.05 
D)  2.35 
E)  1.18

Question 19

Which is a basic oxide?

Accepted Answer

A)  CO2 
B)  MgO 
C)  As2O3 
D)  SO2 
E)  Cl2O7 
A)  CO2 
B)  MgO 
C)  As2O3 
D)  SO2 
E)  Cl2O7

Question 20

For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13. A 0.10 M aqueous solution of Na3PO4 therefore would be ________.

Accepted Answer

A)  neutral 
B)  weakly basic 
C)  weakly acidic 
D)  strongly acidic 
E)  strongly basic 
A)  neutral 
B)  weakly basic 
C)  weakly acidic 
D)  strongly acidic 
E)  strongly basic

Exam 16: Acids and Bases

Amphoteric oxides are compounds that exhibit both acidic and basic behavior.

What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

Weak acids have weak conjugate bases.

A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

In the reaction CaO(s) + SO2(g) CaSO3(s),

Which is a basic oxide?

Which of the following salts will form an acidic solution when dissolved in water?

List the components in an oxoacid.

Which is a Lewis base?

In comparing three solutions with pHs of 2.0, 4.8, and 5.2, which solution is the most acidic?

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2-) = 1.5 × 10-10

What is the conjugate acid of CO32- in the reaction below? CO32- + HSO4- HCO3- + SO42-

What is the conjugate base of water?

A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this acid?

Which is the correct statement?

A solution is prepared by adding 0.10 mol of sodium fluoride, NaF, to 1.00 L of water. Which statement about the solution is correct?

Which represents a weak base B with Kb= 2 ×10-3? (Each circle represents 1.0 ×10-3 mol of atoms, and the volume of each box is 1.0 L. Solvent water molecules are not shown for clarity.)

Find the pH of a 0.20 M aqueous solution of dichloroacetic acid, for which Ka = 3.32 × 10-2.

Which is a basic oxide?

For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13. A 0.10 M aqueous solution of Na3PO4 therefore would be ________.

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

What is the [H₃O⁺] for a solution at 25°C that has pOH = 5.640?

In the reaction CaO(s) + SO₂(g) CaSO₃(s),

What is the pH of a 0.0100 M sodium benzoate solution? K_b (C₇H₅O₂^-) = 1.5 × 10^-10

What is the conjugate acid of CO₃^2- in the reaction below? CO₃^2- + HSO₄^- HCO₃^- + SO₄^2-

A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of K_a for this acid?

Which represents a weak base B with K_b= 2 ×10^-3? (Each circle represents 1.0 ×10^-3 mol of atoms, and the volume of each box is 1.0 L. Solvent water molecules are not shown for clarity.)

Find the pH of a 0.20 M aqueous solution of dichloroacetic acid, for which K_a = 3.32 × 10^-2.

For H₃PO₄, K_a1 = 7.3 × 10^-3, K_a2 = 6.2 × 10^-6, and K_a3 = 4.8 × 10^-13. A 0.10 M aqueous solution of Na₃PO₄ therefore would be ________.