Question 1

In an acidic solution at 25$\circ$C, which of the following is not true?

Accepted Answer

A)  [H3O+] > 1.0 × 10-7 
B)  [H3O+] > [OH-] 
C)  [OH-] -7 
D)  [H3O+][OH-] > 1.0 × 10-7 
E)  [H3O+][OH-] -7 
A)  [H3O+] > 1.0 × 10-7 
B)  [H3O+] > [OH-] 
C)  [OH-] -7 
D)  [H3O+][OH-] > 1.0 × 10-7 
E)  [H3O+][OH-] -7

Question 2

The acid ionization constant expression for the ionization of the hydrogen sulfate ion,   , in aqueous solution is

Accepted Answer

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

Question 3

In a 1.2 M solution of HClO4, a strong acid, [H3O+] = ____, and [OH-] = ____.

Accepted Answer

A)  1.0 × 10-7 M; 1.0 × 10-7 M 
B)  8.3 × 10-15 M; 1.0 × 10-14 M 
C)  8.3 × 10-15 M; 1.2 M 
D)  1.2 M; 8.3 × 10-15 M 
E)  1.2 M; 1.2 M 
A)  1.0 × 10-7 M; 1.0 × 10-7 M 
B)  8.3 × 10-15 M; 1.0 × 10-14 M 
C)  8.3 × 10-15 M; 1.2 M 
D)  1.2 M; 8.3 × 10-15 M 
E)  1.2 M; 1.2 M

Question 4

Identify which of the hydrohalic acids is unlike the others, and why.

Accepted Answer

A)  HF(aq), because it is the only strong acid 
B)  HCl(aq), because it is the only weak acid 
C)  HBr(aq), because it is a liquid at room temperature 
D)  HI(aq), because it does not display hydrogen bonding 
E)  HF(aq), because it displays hydrogen bonding 
A)  HF(aq), because it is the only strong acid 
B)  HCl(aq), because it is the only weak acid 
C)  HBr(aq), because it is a liquid at room temperature 
D)  HI(aq), because it does not display hydrogen bonding 
E)  HF(aq), because it displays hydrogen bonding

Question 5

For the dissociation of a very weak acid, HA, in water

Accepted Answer

A)  Ka = [HA] [H3O+] [A-] 
B)  Ka = [H3O+] [A-] 
C)  Ka = [H3O+] [A-] / [H2O] 
D)  Ka = [HA] / [A-] [H3O+] 
E)  Ka = [H3O+] [A-] / [HA] 
A)  Ka = [HA] [H3O+] [A-] 
B)  Ka = [H3O+] [A-] 
C)  Ka = [H3O+] [A-] / [H2O] 
D)  Ka = [HA] / [A-] [H3O+] 
E)  Ka = [H3O+] [A-] / [HA]

Question 6

Ammonia is a weak base and perchloric acid is a strong acid. Which statement is true of a solution of ammonium perchlorate?

Accepted Answer

A)  It is strongly acidic 
B)  It is weakly acidic 
C)  It is neutral 
D)  It is weakly basic 
E)  We cannot predict its acid-base properties without more information 
A)  It is strongly acidic 
B)  It is weakly acidic 
C)  It is neutral 
D)  It is weakly basic 
E)  We cannot predict its acid-base properties without more information

Question 7

Arrange the solutions in order of increasing acidity:

Accepted Answer

A)  I < IV < II < III 
B)  II < IV < III < I 
C)  III < II < IV < I 
D)  IV < I < II < III 
E)  III < II < I < IV 
A)  I < IV < II < III 
B)  II < IV < III < I 
C)  III < II < IV < I 
D)  IV < I < II < III 
E)  III < II < I < IV

Question 8

Ammonia is a weak base and acetic acid is a weak acid. Which statement is true of a solution of ammonium acetate?

Accepted Answer

A)  It is strongly acidic 
B)  It is weakly acidic 
C)  It is neutral 
D)  It is weakly basic 
E)  We cannot predict its acid-base properties without more information 
A)  It is strongly acidic 
B)  It is weakly acidic 
C)  It is neutral 
D)  It is weakly basic 
E)  We cannot predict its acid-base properties without more information

Question 9

Which pair of substances represents a conjugate acid-base pair?

Accepted Answer

A)  CH3COO- and H2O 
B)  H3O+ and OH- 
C)  CH3COOH and CH3COO- 
D)  CH3COOH and H3O+ 
E)  CH3COOH and OH- 
A)  CH3COO- and H2O 
B)  H3O+ and OH- 
C)  CH3COOH and CH3COO- 
D)  CH3COOH and H3O+ 
E)  CH3COOH and OH-

Question 10

Typically, for a weak acid and its conjugate base

Accepted Answer

A)  Ka / Kb = 1.0 × 10-14 
B)  Ka × Kb = 1.0 × 10-14 
C)  Ka / Kb = 1.0 
D)  Ka × Kb = 1.0 
E)  Ka × Kb = 14 
A)  Ka / Kb = 1.0 × 10-14 
B)  Ka × Kb = 1.0 × 10-14 
C)  Ka / Kb = 1.0 
D)  Ka × Kb = 1.0 
E)  Ka × Kb = 14

Question 11

In a basic solution at 25$\circ$C,

Accepted Answer

A)  [H3O+] > 1.0 × 10-7. 
B)  [H3O+] > [OH-]. 
C)  [OH-] > 1.0 × 10-7. 
D)  [H3O+][OH-] > 1.0 × 10-14. 
E)  [H3O+][OH-] -14. 
A)  [H3O+] > 1.0 × 10-7. 
B)  [H3O+] > [OH-]. 
C)  [OH-] > 1.0 × 10-7. 
D)  [H3O+][OH-] > 1.0 × 10-14. 
E)  [H3O+][OH-] -14.

Question 12

A Bronsted-Lowry acid is always

Accepted Answer

A)  a highly dissociated acid 
B)  a weak acid 
C)  both an acceptor and donor of hydrogen ions 
D)  a donor of one or more hydrogen ions 
E)  a molecule or ion in which hydrogen is attached to an oxygen atom 
A)  a highly dissociated acid 
B)  a weak acid 
C)  both an acceptor and donor of hydrogen ions 
D)  a donor of one or more hydrogen ions 
E)  a molecule or ion in which hydrogen is attached to an oxygen atom

Question 13

In a neutral polyprotic acid, the value of Ka2 will be ____ the value of Ka1 because ____.

Accepted Answer

A)  smaller than; it is more difficult to remove a hydrogen ion from a cation than from a neutral molecule 
B)  larger than; it is more difficult to remove a hydrogen ion from an anion than from a neutral molecule 
C)  larger than; it is more difficult to remove a hydrogen ion from a cation than from a neutral molecule 
D)  smaller than; it is more difficult to remove a hydrogen ion from an anion than from a neutral molecule 
E)  the same as; both hydrogen ions are bonded to the same anion 
A)  smaller than; it is more difficult to remove a hydrogen ion from a cation than from a neutral molecule 
B)  larger than; it is more difficult to remove a hydrogen ion from an anion than from a neutral molecule 
C)  larger than; it is more difficult to remove a hydrogen ion from a cation than from a neutral molecule 
D)  smaller than; it is more difficult to remove a hydrogen ion from an anion than from a neutral molecule 
E)  the same as; both hydrogen ions are bonded to the same anion

Question 14

A solution is not neutral. Which one of these statements is true?

Accepted Answer

A)  [H3O+] = 1.0 × 10-7 M 
B)  [H3O+] = [OH-] 
C)  [H3O+][OH-] = 1.0 × 10-7 
D)  [OH-] = 1.0 × 10-7 M 
E)  [H3O+][OH-] = 1.0 × 10-14 
A)  [H3O+] = 1.0 × 10-7 M 
B)  [H3O+] = [OH-] 
C)  [H3O+][OH-] = 1.0 × 10-7 
D)  [OH-] = 1.0 × 10-7 M 
E)  [H3O+][OH-] = 1.0 × 10-14

Question 15

Carboxylic acids have the formula

Accepted Answer

A)  R-CH3 
B)  R-CHO 
C)  R-COOH 
D)  R-NH2 
E)  R-OH 
A)  R-CH3 
B)  R-CHO 
C)  R-COOH 
D)  R-NH2 
E)  R-OH

Question 16

Which condition represents the most acidic solution?

Accepted Answer

A)  [H3O+] = .010 M 
B)  [OH-] = 1.0 × 10-13 M 
C)  pH = 3.6 
D)  [OH-] = 1.0 × 10-10 M 
E)  pOH = 8.3 
A)  [H3O+] = .010 M 
B)  [OH-] = 1.0 × 10-13 M 
C)  pH = 3.6 
D)  [OH-] = 1.0 × 10-10 M 
E)  pOH = 8.3

Question 17

Methylamine, CH3NH2, acts as a weak base in water. The products of the reaction are ____ and ____.

Accepted Answer

A)  OH- and CH3NH3+ 
B)  H3O+ and CH3NH3+ 
C)  H3O+ and OH- 
D)  OH- and CH3NH- 
E)  H3O+ and CH3NH- 
A)  OH- and CH3NH3+ 
B)  H3O+ and CH3NH3+ 
C)  H3O+ and OH- 
D)  OH- and CH3NH- 
E)  H3O+ and CH3NH-

Question 18

One water molecule can donate a proton to another in a process called ____; the equilibrium constant expression for this reaction is ____.

Accepted Answer

A)  neutralization;   
B)  autoionization;   
C)  protonation;   
D)  hydrolysis;   
E)  autoionization; Kw = [H3O+][OH-] 
A)  neutralization;   
B)  autoionization;   
C)  protonation;   
D)  hydrolysis;   
E)  autoionization; Kw = [H3O+][OH-]

Question 19

If the hydrogen ion concentration of a solution is increased by a factor of 4, the pH is

Accepted Answer

A)  raised by 4 pH units 
B)  raised by 0.3 pH units 
C)  lowered by 2 pH units 
D)  lowered by 0.6 pH units 
E)  lowered by 0.25 pH units 
A)  raised by 4 pH units 
B)  raised by 0.3 pH units 
C)  lowered by 2 pH units 
D)  lowered by 0.6 pH units 
E)  lowered by 0.25 pH units

Question 20

A solution of acetic acid (Ka = 1.8 × 10-5) has a pH exactly 2 higher than a solution of HCl(aq) of the same concentration. What is that concentration?

Accepted Answer

Let the unknown concentration

In an acidic solution at 25^$\circ$C, which of the following is not true?

The acid ionization constant expression for the ionization of the hydrogen sulfate ion, , in aqueous solution is

In a 1.2 M solution of HClO₄, a strong acid, [H₃O⁺] = , and [OH^-] = .

Identify which of the hydrohalic acids is unlike the others, and why.

For the dissociation of a very weak acid, HA, in water

Ammonia is a weak base and perchloric acid is a strong acid. Which statement is true of a solution of ammonium perchlorate?

Arrange the solutions in order of increasing acidity:

Ammonia is a weak base and acetic acid is a weak acid. Which statement is true of a solution of ammonium acetate?

Which pair of substances represents a conjugate acid-base pair?

Typically, for a weak acid and its conjugate base

In a basic solution at 25^$\circ$C,

A Bronsted-Lowry acid is always

In a neutral polyprotic acid, the value of K_a2 will be ____ the value of K_a1 because ____.

A solution is not neutral. Which one of these statements is true?

Carboxylic acids have the formula

Which condition represents the most acidic solution?

Methylamine, CH₃NH₂, acts as a weak base in water. The products of the reaction are and .

One water molecule can donate a proton to another in a process called ; the equilibrium constant expression for this reaction is .

If the hydrogen ion concentration of a solution is increased by a factor of 4, the pH is

A solution of acetic acid (K_a = 1.8 × 10^-5) has a pH exactly 2 higher than a solution of HCl(aq) of the same concentration. What is that concentration?

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Exam 15: Acids and Bases

In an acidic solution at 25 ∘\circ∘ C, which of the following is not true?

The acid ionization constant expression for the ionization of the hydrogen sulfate ion, , in aqueous solution is

In a 1.2 M solution of HClO4, a strong acid, [H3O+] = ____, and [OH-] = ____.

Identify which of the hydrohalic acids is unlike the others, and why.

For the dissociation of a very weak acid, HA, in water

Ammonia is a weak base and perchloric acid is a strong acid. Which statement is true of a solution of ammonium perchlorate?

Arrange the solutions in order of increasing acidity:

Ammonia is a weak base and acetic acid is a weak acid. Which statement is true of a solution of ammonium acetate?

Which pair of substances represents a conjugate acid-base pair?

Typically, for a weak acid and its conjugate base

In a basic solution at 25 ∘\circ∘ C,

A Bronsted-Lowry acid is always

In a neutral polyprotic acid, the value of Ka2 will be ____ the value of Ka1 because ____.

A solution is not neutral. Which one of these statements is true?

Carboxylic acids have the formula

Which condition represents the most acidic solution?

Methylamine, CH3NH2, acts as a weak base in water. The products of the reaction are ____ and ____.

One water molecule can donate a proton to another in a process called ____; the equilibrium constant expression for this reaction is ____.

If the hydrogen ion concentration of a solution is increased by a factor of 4, the pH is

A solution of acetic acid (Ka = 1.8 × 10-5) has a pH exactly 2 higher than a solution of HCl(aq) of the same concentration. What is that concentration?

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

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In an acidic solution at 25^$\circ$C, which of the following is not true?

In a 1.2 M solution of HClO₄, a strong acid, [H₃O⁺] = , and [OH^-] = .

In a basic solution at 25^$\circ$C,

In a neutral polyprotic acid, the value of K_a2 will be ____ the value of K_a1 because ____.

Methylamine, CH₃NH₂, acts as a weak base in water. The products of the reaction are and .

One water molecule can donate a proton to another in a process called ; the equilibrium constant expression for this reaction is .

A solution of acetic acid (K_a = 1.8 × 10^-5) has a pH exactly 2 higher than a solution of HCl(aq) of the same concentration. What is that concentration?