Question 1

What is the conjugate acid of CO32- ?

Accepted Answer

A) CO22- 
B) HCO22- 
C) H2CO3 
D) HCO3- 
E) none of the above 
A) CO22- 
B) HCO22- 
C) H2CO3 
D) HCO3- 
E) none of the above

Question 2

A substance that is capable of acting as both an acid and as a base is ________.

Accepted Answer

A) autosomal 
B) conjugated 
C) ambiprotic 
D) saturated 
E) miscible 
A) autosomal 
B) conjugated 
C) ambiprotic 
D) saturated 
E) miscible

Question 3

What is the pH of a 0.020 M aqueous solution of barium hydroxide?

Accepted Answer

A) 12.60 
B) 12.30 
C) 1.70 
D) 10.41 
E) 1.40 
A) 12.60 
B) 12.30 
C) 1.70 
D) 10.41 
E) 1.40

Question 4

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0 °C. The [H+] in a 1.4 × 10-2 M solution of ethylamine is ________ M.

Accepted Answer

A) 3.7 × 4.9 × 10-12 
B) 2.7 × 10-3 
C) 3.3 × 10-12 
D) 3.0 × 10-3 
E) 11.43 
A) 3.7 × 4.9 × 10-12 
B) 2.7 × 10-3 
C) 3.3 × 10-12 
D) 3.0 × 10-3 
E) 11.43

Question 5

Of the following acids, ________ is a strong acid.

Accepted Answer

A) HNO2 
B) H2CO3 
C) HNO3 
D) HClO 
E) HF 
A) HNO2 
B) H2CO3 
C) HNO3 
D) HClO 
E) HF

Question 6

Kb for NH3 is 1.8 × 10-5. What is the pH of a 0.40 M aqueous solution of NH4Cl at 25.0 °C?

Accepted Answer

A) 2.57 
B) 11.43 
C) 9.18 
D) 4.82 
E) 11.23 
A) 2.57 
B) 11.43 
C) 9.18 
D) 4.82 
E) 11.23

Question 7

A Br∅nsted-Lowry base is defined as a substance that ________.

Accepted Answer

A) increases [H+] when placed in H2O 
B) decreases [H+] when placed in H2O 
C) increases [OH-] when placed in H2O 
D) acts as a proton acceptor 
E) acts as a proton donor 
A) increases [H+] when placed in H2O 
B) decreases [H+] when placed in H2O 
C) increases [OH-] when placed in H2O 
D) acts as a proton acceptor 
E) acts as a proton donor

Question 8

Determine the pH of a 0.15 M aqueous solution of KF. For hydrofluoric acid, Ka = 7.0 × 10-4.

Accepted Answer

A) 0.82 
B) 5.83 
C) 8.17 
D) 5.01 
E) 1.17 
A) 0.82 
B) 5.83 
C) 8.17 
D) 5.01 
E) 1.17

Question 9

What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion?

Accepted Answer

A) 8.400 
B) 5.600 
C) 9.000 
D) 3.980 
E) 7.000 
A) 8.400 
B) 5.600 
C) 9.000 
D) 3.980 
E) 7.000

Question 10

A 0.1 M aqueous solution of ________ will have a pH of 7.0 at 25.0 °C. LiF RbBr NaClO4 NH4Cl

Accepted Answer

A) RbBr and NaClO4 
B) LiF and RbBr 
C) NaClO4 only 
D) LiF only 
E) NH4Cl only 
A) RbBr and NaClO4 
B) LiF and RbBr 
C) NaClO4 only 
D) LiF only 
E) NH4Cl only

Question 11

The Ka of hypochlorous acid (HClO)is 3.0 × 10-8 at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

Accepted Answer

A) 3.05 
B) 9.53 
C) 4.47 
D) 6.52 
E) -3.05 
A) 3.05 
B) 9.53 
C) 4.47 
D) 6.52 
E) -3.05

Question 12

Classify the following compounds as weak acids (W)or strong acids (S): hypochlorous acid perchloric acid chloric acid

Accepted Answer

A) W S S 
B) S S S 
C) S W W 
D) W W W 
E) W S W 
A) W S S 
B) S S S 
C) S W W 
D) W W W 
E) W S W

Question 13

Using the data in the table, which of the conjugate acids below is the strongest acid?

Accepted Answer

A) HClO 
B) HCO3- 
C) H2S 
D) NH3CH3+ 
E) H2S and HClO 
A) HClO 
B) HCO3- 
C) H2S 
D) NH3CH3+ 
E) H2S and HClO

Question 14

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

Accepted Answer

A) OAc- 
B) C7H5O2- 
C) NO2- 
D) F- 
E) OAc- and C7H5O2- 
A) OAc- 
B) C7H5O2- 
C) NO2- 
D) F- 
E) OAc- and C7H5O2-

Question 15

Calculate the pOH of a 0.0727 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) 5.22 
D) 1.14 
E) 8.78 
A) 9.33 
B) 10.00 
C) 5.22 
D) 1.14 
E) 8.78

Question 16

Classify the following compounds as weak bases (W)or strong bases (S): ammonia fluoride ion sodium hydroxide

Accepted Answer

A) W W S 
B) S S S 
C) S W W 
D) W S S 
E) W S W 
A) W W S 
B) S S S 
C) S W W 
D) W S S 
E) W S W

Question 17

The hydride ion, H-, is a stronger base than the hydroxide ion, OH-. The product(s)of the reaction of hydride ion with water is/are ________.

Accepted Answer

A) H3O+ (aq) 
B) OH- (aq) + H2 (g) 
C) OH- (aq) + 2H+ (aq) 
D) no reaction occurs 
E) H2O2 (aq) 
A) H3O+ (aq) 
B) OH- (aq) + H2 (g) 
C) OH- (aq) + 2H+ (aq) 
D) no reaction occurs 
E) H2O2 (aq)

Question 18

The conjugate base of H2PO4- is ________.

Accepted Answer

A) H3PO4 
B) HPO42- 
C) PO43- 
D) H3O+ 
E) OH- 
A) H3PO4 
B) HPO42- 
C) PO43- 
D) H3O+ 
E) OH-

Question 19

HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-?

Accepted Answer

A) HA (aq) + H2O (l)   H2A+ (aq) + OH-(aq) 
B) A- (aq) + H3O+ (aq)   HA (aq) + H2O (l) 
C) HA (aq) + OH- (aq)   H2O (l) + H+ (aq) 
D) A- (aq) + H2O (l)   HA (aq) + OH- (aq) 
E) A- (aq) + OH- (aq)   HOA2- (aq) 
A) HA (aq) + H2O (l)   H2A+ (aq) + OH-(aq) 
B) A- (aq) + H3O+ (aq)   HA (aq) + H2O (l) 
C) HA (aq) + OH- (aq)   H2O (l) + H+ (aq) 
D) A- (aq) + H2O (l)   HA (aq) + OH- (aq) 
E) A- (aq) + OH- (aq)   HOA2- (aq)

Question 20

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

Accepted Answer

A) True 
 B)False

Exam 16: Acid-Base Equilibria

What is the conjugate acid of CO32- ?

A substance that is capable of acting as both an acid and as a base is ________.

What is the pH of a 0.020 M aqueous solution of barium hydroxide?

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0 °C. The [H+] in a 1.4 × 10-2 M solution of ethylamine is ________ M.

Of the following acids, ________ is a strong acid.

Kb for NH3 is 1.8 × 10-5. What is the pH of a 0.40 M aqueous solution of NH4Cl at 25.0 °C?

A Br∅nsted-Lowry base is defined as a substance that ________.

Determine the pH of a 0.15 M aqueous solution of KF. For hydrofluoric acid, Ka = 7.0 × 10-4.

What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion?

A 0.1 M aqueous solution of ________ will have a pH of 7.0 at 25.0 °C. LiF RbBr NaClO4 NH4Cl

The Ka of hypochlorous acid (HClO)is 3.0 × 10-8 at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

Classify the following compounds as weak acids (W)or strong acids (S): hypochlorous acid perchloric acid chloric acid

Using the data in the table, which of the conjugate acids below is the strongest acid?

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

Calculate the pOH of a 0.0727 M aqueous sodium cyanide solution at 25.0 °C. Kb for CN- is 4.9 × 10-10.

Classify the following compounds as weak bases (W)or strong bases (S): ammonia fluoride ion sodium hydroxide

The hydride ion, H-, is a stronger base than the hydroxide ion, OH-. The product(s)of the reaction of hydride ion with water is/are ________.

The conjugate base of H2PO4- is ________.

HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-?

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

Introduction: Matter and Measurement

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Filters

What is the conjugate acid of CO₃²^-?

The base-dissociation constant of ethylamine (C₂H₅NH₂)is 6.4 × 10^-⁴ at 25.0 °C. The [H⁺] in a 1.4 × 10^-² M solution of ethylamine is ________ M.

K_b for NH₃ is 1.8 × 10^-⁵. What is the pH of a 0.40 M aqueous solution of NH₄Cl at 25.0 °C?

Determine the pH of a 0.15 M aqueous solution of KF. For hydrofluoric acid, K_a = 7.0 × 10^-4.

What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10^-9 M hydronium ion?

A 0.1 M aqueous solution of ________ will have a pH of 7.0 at 25.0 °C. LiF RbBr NaClO₄ NH₄Cl

The K_a of hypochlorous acid (HClO)is 3.0 × 10^-⁸ at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

Calculate the pOH of a 0.0727 M aqueous sodium cyanide solution at 25.0 °C. K_b for CN^- is 4.9 × 10^-¹⁰.

The hydride ion, H^-, is a stronger base than the hydroxide ion, OH^-. The product(s)of the reaction of hydride ion with water is/are ________.

The conjugate base of H₂PO₄^- is ________.

HA is a weak acid. Which equilibrium corresponds to the equilibrium constant K_b for A^-?

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