Question 1

In basic solution, .

Accepted Answer

A)  [H3O+] > [OH- ] 
B)  [H3O+] - ] 
C)  [H3O+] = 0 M 
D)  [OH- ] > 7.00 
E)  [H3O+] = [OH- ] 
A)  [H3O+] > [OH- ] 
B)  [H3O+] - ] 
C)  [H3O+] = 0 M 
D)  [OH- ] > 7.00 
E)  [H3O+] = [OH- ]

Question 2

Using the data in the table, which of the conjugate bases below is the strongest base?

Accepted Answer

A)  CHO2- 
B)  F- 
C)  OAc- 
D)  ClO- 
E)  OAc- and CHO2- 
A)  CHO2- 
B)  F- 
C)  OAc- 
D)  ClO- 
E)  OAc- and CHO2-

Question 3

What is the pH of a sodium acetate solution prepared by adding 0.820 grams of sodium acetate to 100.0 ml of water at 25.0 oC? The Ka at 25.0 oC for acetic acid is 1.8 × 10- 5.

Accepted Answer

Question 4

The molar concentration of hydroxide ion in pure water at 25°C is .

Accepted Answer

A)  0.00 
B)  1.00 
C)  1.0 ×10- 14  
D)  7.00 
E)  1.0 × 10- 7 
A)  0.00 
B)  1.00 
C)  1.0 ×10- 14  
D)  7.00 
E)  1.0 × 10- 7

Question 5

The Ka for formic acid (HCO2H) is 1.8 × 10- 4. What is the pH of a 0.35 M aqueous solution of sodium formate (NaHCO2)?

Accepted Answer

A)  5.4 
B)  4.2 
C)  8.6 
D)  11 
E)  3.3 
A)  5.4 
B)  4.2 
C)  8.6 
D)  11 
E)  3.3

Question 6

The acid- dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10- 10. What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

Accepted Answer

A)  11.11 
B)  3.9 × 10- 11 
C)  1.3 × 10- 3 
D)  7.8 × 10- 12 
E)  2.89 
A)  11.11 
B)  3.9 × 10- 11 
C)  1.3 × 10- 3 
D)  7.8 × 10- 12 
E)  2.89

Question 7

Of the following, which is the strongest acid?

Accepted Answer

A)  HIO2 
B)  HIO 
C)  HIO4 
D)  HIO3 
E)  The acid strength of all of the above is the same. 
A)  HIO2 
B)  HIO 
C)  HIO4 
D)  HIO3 
E)  The acid strength of all of the above is the same.

Question 8

The Ka of hypochlorous acid (HClO) is 3.0 × 10- 8 at 25.0 °C. What is the % ionization of hypochlorous acid in a 0.015- M aqueous solution of HClO at 25.0 °C?

Accepted Answer

A)  1.4 × 10- 3  
B)  0.14 
C)  2.1 × 10- 5  
D)  4.5 × 10- 8  
E)  14 
A)  1.4 × 10- 3  
B)  0.14 
C)  2.1 × 10- 5  
D)  4.5 × 10- 8  
E)  14

Question 9

What is the pH of an aqueous solution at 25.0 °C in which [OH- ] is 0.00250 M?

Accepted Answer

A)  +2.60 
B)  - 2.60 
C)  +11.4 
D)  - 11.4 
E)  - 2.25 
A)  +2.60 
B)  - 2.60 
C)  +11.4 
D)  - 11.4 
E)  - 2.25

Question 10

The acid- dissociation constant for chlorous acid, HClO2, at 25.0 °C is 1.0 × 10- 2. Calculate the concentration of H+ if the initial concentration of acid is 0.10 M.

Accepted Answer

A)  2.7 × 10- 2  
B)  3.2 × 10- 2  
C)  3.7 × 10- 2  
D)  1.0 × 10- 2  
E)  1.0 × 10- 3 
A)  2.7 × 10- 2  
B)  3.2 × 10- 2  
C)  3.7 × 10- 2  
D)  1.0 × 10- 2  
E)  1.0 × 10- 3

Question 11

Calculate the pOH of a solution at 25.0 °C that contains 1.94 × 10- 10 M hydronium ions.

Accepted Answer

A)  9.71 
B)  1.94 
C)  14.0 
D)  7.00 
E)  4.29 
A)  9.71 
B)  1.94 
C)  14.0 
D)  7.00 
E)  4.29

Question 12

The magnitude of Kw indicates that .

Accepted Answer

A)  water autoionizes very quickly 
B)  water autoionizes only to a very small extent 
C)  the autoionization of water is exothermic 
D)  water autoionizes very slowly 
A)  water autoionizes very quickly 
B)  water autoionizes only to a very small extent 
C)  the autoionization of water is exothermic 
D)  water autoionizes very slowly

Question 13

Which one of the following statements regarding Kw is false?

Accepted Answer

A)  Kw changes with temperature. 
B)  Kw is known as the ion product of water. 
C)  The value of Kw is always 1.0 × 10- 14. 
D)  The value of Kw shows that water is a weak acid. 
E)  pKw is 14.00 at 25°C 
A)  Kw changes with temperature. 
B)  Kw is known as the ion product of water. 
C)  The value of Kw is always 1.0 × 10- 14. 
D)  The value of Kw shows that water is a weak acid. 
E)  pKw is 14.00 at 25°C

Question 14

Ka for HF is 7.0 × 10- 4. Kb for the fluoride ion is _ _.

Accepted Answer

A)  7.0 × 10- 4 
B)  2.0 × 10- 8 
C)  1.4 × 10- 11 
D)  1.4 × 103 
E)  7.0 × 10- 18 
A)  7.0 × 10- 4 
B)  2.0 × 10- 8 
C)  1.4 × 10- 11 
D)  1.4 × 103 
E)  7.0 × 10- 18

Question 15

Of the compounds below, a 0.1 M aqueous solution of will have the highest pH.

Accepted Answer

A)  NH4NO3, Kb of NH3 = 1.8 × 10- 5 
B)  NaOAc, Ka of HOAc = 1.8 × 10- 5 
C)  KCN, Ka of HCN = 4.0 × 10- 10 
D)  NaClO, Ka of HClO = 3.2 × 10- 8 
E)  NaHS, Kb of HS- = 1.8 × 10- 7 
A)  NH4NO3, Kb of NH3 = 1.8 × 10- 5 
B)  NaOAc, Ka of HOAc = 1.8 × 10- 5 
C)  KCN, Ka of HCN = 4.0 × 10- 10 
D)  NaClO, Ka of HClO = 3.2 × 10- 8 
E)  NaHS, Kb of HS- = 1.8 × 10- 7

Question 16

Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine) The Kb of methylamine is 4.4 × 10- 4.

Accepted Answer

A)  13 
B)  12 
C)  3.8 
D)  10 
E)  1.9 
A)  13 
B)  12 
C)  3.8 
D)  10 
E)  1.9

Question 17

The concentration of water in pure water is approximately M.

Accepted Answer

A)  0.100 
B)  83 
C)  18 
D)  55 
E)  100 
A)  0.100 
B)  83 
C)  18 
D)  55 
E)  100

Question 18

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.33.

Accepted Answer

A)  5.3 × 10- 14 
B)  2.1 × 10- 9 
C)  8.67 
D)  4.7 × 10- 6 
E)  8.7 × 10- 14 
A)  5.3 × 10- 14 
B)  2.1 × 10- 9 
C)  8.67 
D)  4.7 × 10- 6 
E)  8.7 × 10- 14

Question 19

The Ka of hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10- 4. What is the pH of a 0.35 M aqueous solution of HF?

Accepted Answer

A)  3.6 
B)  3.2 
C)  12 
D)  0.46 
E)  1.8 
A)  3.6 
B)  3.2 
C)  12 
D)  0.46 
E)  1.8

Question 20

The pH of an aqueous solution at 25.0 °C is 10.66. What is the molarity of H+ in this solution?

Accepted Answer

A)  4.6 × 10- 4 
B)  3.3 
C)  2.2 × 10- 11 
D)  1.1 × 10- 13 
E)  4.6 × 1010 
A)  4.6 × 10- 4 
B)  3.3 
C)  2.2 × 10- 11 
D)  1.1 × 10- 13 
E)  4.6 × 1010

Exam 16: Acid-Base Equilibria

In basic solution, .

Using the data in the table, which of the conjugate bases below is the strongest base?

What is the pH of a sodium acetate solution prepared by adding 0.820 grams of sodium acetate to 100.0 ml of water at 25.0 oC? The Ka at 25.0 oC for acetic acid is 1.8 × 10- 5.

The molar concentration of hydroxide ion in pure water at 25°C is .

The Ka for formic acid (HCO2H) is 1.8 × 10- 4. What is the pH of a 0.35 M aqueous solution of sodium formate (NaHCO2)?

The acid- dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10- 10. What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

Of the following, which is the strongest acid?

The Ka of hypochlorous acid (HClO) is 3.0 × 10- 8 at 25.0 °C. What is the % ionization of hypochlorous acid in a 0.015- M aqueous solution of HClO at 25.0 °C?

What is the pH of an aqueous solution at 25.0 °C in which [OH- ] is 0.00250 M?

The acid- dissociation constant for chlorous acid, HClO2, at 25.0 °C is 1.0 × 10- 2. Calculate the concentration of H+ if the initial concentration of acid is 0.10 M.

Calculate the pOH of a solution at 25.0 °C that contains 1.94 × 10- 10 M hydronium ions.

The magnitude of Kw indicates that .

Which one of the following statements regarding Kw is false?

Ka for HF is 7.0 × 10- 4. Kb for the fluoride ion is _ _.

Of the compounds below, a 0.1 M aqueous solution of will have the highest pH.

Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine) The Kb of methylamine is 4.4 × 10- 4.

The concentration of water in pure water is approximately M.

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.33.

The Ka of hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10- 4. What is the pH of a 0.35 M aqueous solution of HF?

The pH of an aqueous solution at 25.0 °C is 10.66. What is the molarity of H+ in this solution?

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What is the pH of a sodium acetate solution prepared by adding 0.820 grams of sodium acetate to 100.0 ml of water at 25.0 ^oC? The K_aat 25.0 ^oC for acetic acid is 1.8 × 10^-⁵.

The K_afor formic acid (HCO₂H) is 1.8 × 10^-⁴. What is the pH of a 0.35 M aqueous solution of sodium formate (NaHCO₂)?

The acid- dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10^-¹⁰. What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

The K_aof hypochlorous acid (HClO) is 3.0 × 10^-⁸at 25.0 °C. What is the % ionization of hypochlorous acid in a 0.015- M aqueous solution of HClO at 25.0 °C?

What is the pH of an aqueous solution at 25.0 °C in which [OH^-] is 0.00250 M?

The acid- dissociation constant for chlorous acid, HClO₂, at 25.0 °C is 1.0 × 10^-². Calculate the concentration of H⁺if the initial concentration of acid is 0.10 M.

Calculate the pOH of a solution at 25.0 °C that contains 1.94 × 10^-¹⁰M hydronium ions.

The magnitude of K_windicates that .

Which one of the following statements regarding K_wis false?

K_afor HF is 7.0 × 10^-⁴. K_bfor the fluoride ion is _ _.

Determine the pH of a 0.35 M aqueous solution of CH₃NH₂(methylamine) The K_bof methylamine is 4.4 × 10^-⁴.

The K_aof hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10^-⁴. What is the pH of a 0.35 M aqueous solution of HF?

The pH of an aqueous solution at 25.0 °C is 10.66. What is the molarity of H⁺in this solution?