Question 1

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

Accepted Answer

A) 1.0 × 10-5 
B) 9.00 
C) 1.0 × 10-9 
D) 5.0 × 10-14 
E) 9.0 × 10-14 
A) 1.0 × 10-5 
B) 9.00 
C) 1.0 × 10-9 
D) 5.0 × 10-14 
E) 9.0 × 10-14

Question 2

Calculate the pH of a 0.0787 M aqueous sodium cyanide solution at 25.0 °C. Kb for CN- is 4.9 × 10-10.

Accepted Answer

A) 9.33 
B) 10.00 
C) 5.21 
D) 1.10 
E) 8.79 
A) 9.33 
B) 10.00 
C) 5.21 
D) 1.10 
E) 8.79

Question 3

Nitric acid is a strong acid. This means that __________.

Accepted Answer

A) aqueous solutions of HNO3 contain equal concentrations of H+(aq)and OH-(aq) 
B) HNO3 does not dissociate at all when it is dissolved in water 
C) HNO3 dissociates completely to H+(aq)and NO3-(aq)when it dissolves in water 
D) HNO3 produces a gaseous product when it is neutralized 
E) HNO3 cannot be neutralized by a weak base 
A) aqueous solutions of HNO3 contain equal concentrations of H+(aq)and OH-(aq) 
B) HNO3 does not dissociate at all when it is dissolved in water 
C) HNO3 dissociates completely to H+(aq)and NO3-(aq)when it dissolves in water 
D) HNO3 produces a gaseous product when it is neutralized 
E) HNO3 cannot be neutralized by a weak base

Question 4

In the reaction
BF3 + F- → BF4-
BF3 acts as a Br∅nsted-Lowry acid.

Accepted Answer

A) True 
 B)False

Question 5

What is the conjugate base of OH-?

Accepted Answer

A) O2 
B) O- 
C) H2O 
D) O2- 
E) H3O+ 
A) O2 
B) O- 
C) H2O 
D) O2- 
E) H3O+

Question 6

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ)is 10.7. What is the Ka for HZ?

Accepted Answer

A) 1.6 × 10-6 
B) 6.0 × 10-9 
C) 8.9 × 10-4 
D) 1.3 × 10-12 
E) 3.3 × 10-8 
A) 1.6 × 10-6 
B) 6.0 × 10-9 
C) 8.9 × 10-4 
D) 1.3 × 10-12 
E) 3.3 × 10-8

Question 7

Of the following, which is the weakest acid?

Accepted Answer

A) HIO 
B) HIO4 
C) HIO2 
D) HIO3 
E) The acid strength of all of the above is the same. 
A) HIO 
B) HIO4 
C) HIO2 
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) 4.5 × 10-8 
B) 14 
C) 2.1 × 10-5 
D) 0.14 
E) 1.4 × 10-3 
A) 4.5 × 10-8 
B) 14 
C) 2.1 × 10-5 
D) 0.14 
E) 1.4 × 10-3

Question 9

A 0.15 M aqueous solution of the weak acid HA at 25.0°C has a pH of 5.35. The value of Ka for HA is __________.

Accepted Answer

A) 3.0 × 10-5 
B) 1.8 × 10-5 
C) 7.1 × 10-9 
D) 1.3 × 10-10 
E) 3.3 × 104 
A) 3.0 × 10-5 
B) 1.8 × 10-5 
C) 7.1 × 10-9 
D) 1.3 × 10-10 
E) 3.3 × 104

Question 10

What is the conjugate acid of CO3-2?

Accepted Answer

A) CO2-2 
B) HCO2-2 
C) H2CO3 
D) HCO3- 
E) none of the above 
A) CO2-2 
B) HCO2-2 
C) H2CO3 
D) HCO3- 
E) none of the above

Question 11

Calculate the concentration (in M)of hydronium ions in a solution at 25.0°C with a pOH of 4.223.

Accepted Answer

A) 5.98 × 10-5 
B) 1.67 × 10-10 
C) 1.67 × 104 
D) 5.99 × 10-19 
E) 1.00 × 10-7 
A) 5.98 × 10-5 
B) 1.67 × 10-10 
C) 1.67 × 104 
D) 5.99 × 10-19 
E) 1.00 × 10-7

Question 12

Which one of the following is a BrØnsted -Lowry base?

Accepted Answer

A) (CH3)3N 
B) CH3COOH 
C) HF 
D) HNO2 
E) none of the above 
A) (CH3)3N 
B) CH3COOH 
C) HF 
D) HNO2 
E) none of the above

Question 13

In basic solution, __________.

Accepted Answer

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

Question 14

A 0.1 M solution of __________ has a pH of 7.0.

Accepted Answer

A) Na2S 
B) KF 
C) NaNO3 
D) NH4Cl 
E) NaF 
A) Na2S 
B) KF 
C) NaNO3 
D) NH4Cl 
E) NaF

Question 15

The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

Accepted Answer

A) 2.1 × 10-4 
B) 4.4 × 10-8 
C) 8.8 × 10-8 
D) 6.6 × 10-4 
E) 2.0 × 10-5 
A) 2.1 × 10-4 
B) 4.4 × 10-8 
C) 8.8 × 10-8 
D) 6.6 × 10-4 
E) 2.0 × 10-5

Question 16

An aqueous solution of __________ will produce a basic solution.

Accepted Answer

A) NH4ClO4 
B) KBr 
C) NaCl 
D) NaHSO4 
E) Na2SO3 
A) NH4ClO4 
B) KBr 
C) NaCl 
D) NaHSO4 
E) Na2SO3

Question 17

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0°C? The Ka at 25.0°C for formic acid is 1.8 × 10-4.

Accepted Answer

Question 18

A 7.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of __________.

Accepted Answer

A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85 
A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85

Question 19

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.010 M solution of HClO is __________.

Accepted Answer

A) 1.7 × 10-5 
B) 0.010 
C) 5.8 × 10-10 
D) 4.76 
E) 2.00 
A) 1.7 × 10-5 
B) 0.010 
C) 5.8 × 10-10 
D) 4.76 
E) 2.00

Question 20

A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M)of the acetic acid solution? The Ka at 25.0 °C for acetic acid is 1.8 × 10-5.

Accepted Answer

Exam 16: Acid-Base Equilibria

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

Calculate the pH of a 0.0787 M aqueous sodium cyanide solution at 25.0 °C. Kb for CN- is 4.9 × 10-10.

Nitric acid is a strong acid. This means that __________.

In the reaction BF3 + F- → BF4- BF3 acts as a Br∅nsted-Lowry acid.

What is the conjugate base of OH-?

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ)is 10.7. What is the Ka for HZ?

Of the following, which is the weakest 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?

A 0.15 M aqueous solution of the weak acid HA at 25.0°C has a pH of 5.35. The value of Ka for HA is __________.

What is the conjugate acid of CO3-2?

Calculate the concentration (in M)of hydronium ions in a solution at 25.0°C with a pOH of 4.223.

Which one of the following is a BrØnsted -Lowry base?

In basic solution, __________.

A 0.1 M solution of __________ has a pH of 7.0.

The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

An aqueous solution of __________ will produce a basic solution.

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0°C? The Ka at 25.0°C for formic acid is 1.8 × 10-4.

A 7.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of __________.

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.010 M solution of HClO is __________.

A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M)of the acetic acid solution? The Ka at 25.0 °C for acetic acid is 1.8 × 10-5.

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Calculate the pH of a 0.0787 M aqueous sodium cyanide solution at 25.0 °C. K_b for CN^- is 4.9 × 10^-10.

In the reaction BF₃ + F^- → BF₄^- BF₃ acts as a Br∅nsted-Lowry acid.

What is the conjugate base of OH^-?

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ)is 10.7. What is the K_a for HZ?

The K_a 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?

A 0.15 M aqueous solution of the weak acid HA at 25.0°C has a pH of 5.35. The value of K_a for HA is __________.

What is the conjugate acid of CO₃^-2?

The pH of a 0.10 M solution of a weak base is 9.82. What is the K_b for this base?

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0°C? The K_a at 25.0°C for formic acid is 1.8 × 10^-4.

A 7.0 × 10^-3 M aqueous solution of Ca(OH)₂ at 25.0°C has a pH of __________.

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10^-8. At equilibrium, the molarity of H₃O⁺ in a 0.010 M solution of HClO is __________.

A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M)of the acetic acid solution? The K_a at 25.0 °C for acetic acid is 1.8 × 10^-5.