Question 1

Of the following, which is the strongest acid?

Accepted Answer

A)  HClO 
B)  HClO2  
C)  HClO3  
D)  HIO 
E)  HClO4 
A)  HClO 
B)  HClO2  
C)  HClO3  
D)  HIO 
E)  HClO4 E

Question 2

A solution of ammonia is 2.0% dissociated at 25.0 oC. What was the original concentration ( in M) of the ammonia solution? The Kb at 25.0 oC for ammonia is 1.8 × 10- 5.

Accepted Answer

0.045

Question 3

A 0.1 M solution of has a pH of 7.0.

Accepted Answer

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

Question 4

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

Accepted Answer

A)  5.60 
B)  8.40 
C)  7.00 
D)  3.98 
E)  9.00 
A)  5.60 
B)  8.40 
C)  7.00 
D)  3.98 
E)  9.00

Question 5

Which solution below has the highest concentration of hydroxide ions?

Accepted Answer

A)  pH = 7.93 
B)  pH = 3.21 
C)  pH = 7.00 
D)  pH = 12.6 
E)  pH = 9.82 
A)  pH = 7.93 
B)  pH = 3.21 
C)  pH = 7.00 
D)  pH = 12.6 
E)  pH = 9.82

Question 6

What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.282?

Accepted Answer

A)  5.22 × 10- 5 
B)  1.91 × 10- 10 
C)  9.72 
D)  4.28 
E)  1.66 × 104 
A)  5.22 × 10- 5 
B)  1.91 × 10- 10 
C)  9.72 
D)  4.28 
E)  1.66 × 104

Question 7

A BrØnsted- Lowry acid is defined as a substance that .

Accepted Answer

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

Question 8

An acid containing the COOH group is called a carbo- oxy acid.

Accepted Answer

A) True 
 B)False

Question 9

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

Accepted Answer

A)  (CH3)3NH+ 
B)  HNO2 
C)  CH3COOH 
D)  HF 
E)  all of the above 
A)  (CH3)3NH+ 
B)  HNO2 
C)  CH3COOH 
D)  HF 
E)  all of the above

Question 10

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

Accepted Answer

A)  5.8 
B)  6.6 
C)  12 
D)  8.2 
E)  2.3 
A)  5.8 
B)  6.6 
C)  12 
D)  8.2 
E)  2.3

Question 11

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

Question 12

Of the following substances, an aqueous solution of will form basic solutions. NH4Cl Cu(NO3)2 K2CO3 NaF

Accepted Answer

A)  NH4Cl only 
B)  NH4Cl , Cu(NO3)2 
C)  NaF, K2CO3 
D)  NaF only 
E)  K2CO3, NH4Cl 
A)  NH4Cl only 
B)  NH4Cl , Cu(NO3)2 
C)  NaF, K2CO3 
D)  NaF only 
E)  K2CO3, NH4Cl

Question 13

Which of the following ions will act as a weak base in water?

Accepted Answer

A)  OH- 
B)  NO3- 
C)  ClO- 
D)  Cl- 
E)  None of the above will act as a weak base in water. 
A)  OH- 
B)  NO3- 
C)  ClO- 
D)  Cl- 
E)  None of the above will act as a weak base in water.

Question 14

The Ka of hypochlorous acid (HClO) is 3.00 × 10- 8. What is the pH at 25.0 °C of an aqueous solution that is 0.0200 M in HClO?

Accepted Answer

A)  +2.45 
B)  - 2.45 
C)  - 9.22 
D)  +9.22 
E)  +4.61 
A)  +2.45 
B)  - 2.45 
C)  - 9.22 
D)  +9.22 
E)  +4.61

Question 15

The Ka of hydrazoic acid (HN3) is 1.9 × 10- 5 at 25.0 °C. What is the pH of a 0.35 M aqueous solution of HN3?

Accepted Answer

A)  5.2 
B)  2.4 
C)  11 
D)  - 2.4 
E)  2.6 
A)  5.2 
B)  2.4 
C)  11 
D)  - 2.4 
E)  2.6

Question 16

What is the concentration (in M) of hydronium ions in a solution at 25.0 °C with pH = 4.282?

Accepted Answer

A)  1.66 × 104 
B)  9.71 
C)  1.92 × 10- 10 
D)  5.22 × 10- 5 
E)  4.28 
A)  1.66 × 104 
B)  9.71 
C)  1.92 × 10- 10 
D)  5.22 × 10- 5 
E)  4.28

Question 17

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

Accepted Answer

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

Question 18

When the proton in the COOH group in an amino acid is transferred to the NH2 group of that same amino acid molecule, a zwitterion is formed.

Accepted Answer

A) True 
 B)False

Question 19

The acid- dissociation constants of sulfurous acid (H2SO3) are Ka1 = 1.7 × 10- 2 and
Ka2 = 6.4 × 10- 8 at 25.0 °C. Calculate the pH of a 0.163 M aqueous solution of sulfurous acid.

Accepted Answer

A)  1.4 
B)  7.2 
C)  1.8 
D)  1.3 
E)  4.5 
A)  1.4 
B)  7.2 
C)  1.8 
D)  1.3 
E)  4.5

Question 20

A BrØnsted- Lowry base is defined as a substance that .

Accepted Answer

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

Exam 16: Acid-Base Equilibria

Of the following, which is the strongest acid?

A solution of ammonia is 2.0% dissociated at 25.0 oC. What was the original concentration ( in M) of the ammonia solution? The Kb at 25.0 oC for ammonia is 1.8 × 10- 5.

A 0.1 M solution of has a pH of 7.0.

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

Which solution below has the highest concentration of hydroxide ions?

What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.282?

A BrØnsted- Lowry acid is defined as a substance that .

An acid containing the COOH group is called a carbo- oxy acid.

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

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

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 _.

Of the following substances, an aqueous solution of will form basic solutions. NH4Cl Cu(NO3)2 K2CO3 NaF

Which of the following ions will act as a weak base in water?

The Ka of hypochlorous acid (HClO) is 3.00 × 10- 8. What is the pH at 25.0 °C of an aqueous solution that is 0.0200 M in HClO?

The Ka of hydrazoic acid (HN3) is 1.9 × 10- 5 at 25.0 °C. What is the pH of a 0.35 M aqueous solution of HN3?

What is the concentration (in M) of hydronium ions in a solution at 25.0 °C with pH = 4.282?

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

When the proton in the COOH group in an amino acid is transferred to the NH2 group of that same amino acid molecule, a zwitterion is formed.

The acid- dissociation constants of sulfurous acid (H2SO3) are Ka1 = 1.7 × 10- 2 and Ka2 = 6.4 × 10- 8 at 25.0 °C. Calculate the pH of a 0.163 M aqueous solution of sulfurous acid.

A BrØnsted- Lowry base is defined as a substance that .

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A solution of ammonia is 2.0% dissociated at 25.0 ^oC. What was the original concentration ( in M) of the ammonia solution? The K_bat 25.0 ^oC for ammonia is 1.8 × 10^-⁵.

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

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

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 _.

Of the following substances, an aqueous solution of will form basic solutions. NH₄Cl Cu(NO₃)₂K₂CO₃NaF

The K_aof hypochlorous acid (HClO) is 3.00 × 10^-⁸. What is the pH at 25.0 °C of an aqueous solution that is 0.0200 M in HClO?

The K_aof hydrazoic acid (HN₃) is 1.9 × 10^-⁵at 25.0 °C. What is the pH of a 0.35 M aqueous solution of HN₃?

When the proton in the COOH group in an amino acid is transferred to the NH₂group of that same amino acid molecule, a zwitterion is formed.

The acid- dissociation constants of sulfurous acid (H₂SO₃) are K_a1= 1.7 × 10^-²and K_a2= 6.4 × 10^-⁸at 25.0 °C. Calculate the pH of a 0.163 M aqueous solution of sulfurous acid.