Question 1

Identify the diprotic acid.

Accepted Answer

A) HNO3 
B) HCl 
C) CH3COOH 
D) H2SO4 
E) HClO4 
A) HNO3 
B) HCl 
C) CH3COOH 
D) H2SO4 
E) HClO4

Question 2

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 mol L-1 in hydronium ion.

Accepted Answer

A) 2.86 × 10-3 mol L-1 
B) 2.86 × 10-10 mol L-1 
C) 2.86 × 10-11 mol L-1 
D) 3.50 × 10-11 mol L-1 
A) 2.86 × 10-3 mol L-1 
B) 2.86 × 10-10 mol L-1 
C) 2.86 × 10-11 mol L-1 
D) 3.50 × 10-11 mol L-1

Question 3

Calculate the pH of a solution that contains 7.8 × 10-6 mol L-1 OH⁻ at 25 °C.

Accepted Answer

A) 1.28 
B) 5.11 
C) 12.72 
D) 8.89 
E) 9.64 
A) 1.28 
B) 5.11 
C) 12.72 
D) 8.89 
E) 9.64

Question 4

What is the pH of a 0.30 mol L-1 pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is below:

Accepted Answer

A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38 
A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38

Question 5

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 6

Find the percent ionization of a 0.337 mol L-1 HF solution. The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 1.1% 
B) 1.2 × 10-2% 
C) 3.2% 
D) 3.5 × 10-2% 
E) 4.7% 
A) 1.1% 
B) 1.2 × 10-2% 
C) 3.2% 
D) 3.5 × 10-2% 
E) 4.7%

Question 7

Which of the following is a weak base?

Accepted Answer

A) NH(CH3)2 
B) N2 
C) NaOH 
D) CH2CH2 
E) Ca(OH)2 
A) NH(CH3)2 
B) N2 
C) NaOH 
D) CH2CH2 
E) Ca(OH)2

Question 8

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 mol L-1 OH⁻ at 25 °C. Also identify the solution as acidic, basic, or neutral.

Accepted Answer

A) 1.8 × 10-10 mol L-1, basic 
B) 1.8 × 10-10 mol L-1, acidic 
C) 5.5 × 10-10 mol L-1, neutral 
D) 9.2 × 10-1 mol L-1, acidic 
E) 9.2 × 10-1 mol L-1, basic 
A) 1.8 × 10-10 mol L-1, basic 
B) 1.8 × 10-10 mol L-1, acidic 
C) 5.5 × 10-10 mol L-1, neutral 
D) 9.2 × 10-1 mol L-1, acidic 
E) 9.2 × 10-1 mol L-1, basic

Question 9

Calculate the pH of a 0.080 mol L-1 carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 1.10 
B) 3.73 
C) 6.37 
D) 10.25 
A) 1.10 
B) 3.73 
C) 6.37 
D) 10.25

Question 10

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L-1 in acid at 25 ∘C? The acid is followed by its Ka value.

Accepted Answer

A) HF, 3.5 × 10-4 
B) HCN, 4.9 × 10-10 
C) HNO2, 4.6 × 10-4 
D) HCHO2, 1.8 × 10-4 
E) HClO2, 1.1 × 10-2 
A) HF, 3.5 × 10-4 
B) HCN, 4.9 × 10-10 
C) HNO2, 4.6 × 10-4 
D) HCHO2, 1.8 × 10-4 
E) HClO2, 1.1 × 10-2

Question 11

Which Bronsted-Lowry acid is not considered to be a strong acid in water?

Accepted Answer

A) HBr 
B) HI  
C) H IO4 
D) HNO3 
A) HBr 
B) HI  
C) H IO4 
D) HNO3

Question 12

Determine the concentration of CO32- ions in a 0.18 mol L-1 H2CO3 solution. Carbonic acid is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 2.8 × 10-4 mol L-1 
B) 3.2 × 10-6 mol L-1 
C) 5.6 × 10-11 mol L-1 
D) 4.3 × 10-7 mol L-1 
E) 6.9 × 10-8 mol L-1 
A) 2.8 × 10-4 mol L-1 
B) 3.2 × 10-6 mol L-1 
C) 5.6 × 10-11 mol L-1 
D) 4.3 × 10-7 mol L-1 
E) 6.9 × 10-8 mol L-1

Question 13

What is the hydronium ion concentration of a 0.150 mol L-1 hypochlorous acid solution with Ka = 3.5 × 10-8? The equation for the dissociation of hypochlorous acid is below:

Accepted Answer

A) 1.9 × 10-4 mol L-1 
B) 7.2 × 10-4 mol L-1 
C) 2.8 × 10-5 mol L-1 
D) 7.2 × 10-5 mol L-1 
A) 1.9 × 10-4 mol L-1 
B) 7.2 × 10-4 mol L-1 
C) 2.8 × 10-5 mol L-1 
D) 7.2 × 10-5 mol L-1

Question 14

List the compound that is formed from the reaction of carbon dioxide with water.

Accepted Answer

The answer of List the compound that is formed from...

Question 15

Determine the [OH-] concentration of a 0.741 mol L-1 KOH solution at 25 °C.

Accepted Answer

A) 1.34 × 10-13 mol L-1 
B) 1.34 × 10-14 mol L-1 
C) 0.741 mol L-1 
D) 7.41 mol L-1 
E) 7.41 × 10-13 mol L-1 
A) 1.34 × 10-13 mol L-1 
B) 1.34 × 10-14 mol L-1 
C) 0.741 mol L-1 
D) 7.41 mol L-1 
E) 7.41 × 10-13 mol L-1

Question 16

Identify the weakest acid.

Accepted Answer

A) HF 
B) HCl 
C) HBr 
D) HI 
E) NaH 
A) HF 
B) HCl 
C) HBr 
D) HI 
E) NaH

Question 17

Determine the [OH⁻] concentration in a 0.235 mol L-1 NaOH solution.

Accepted Answer

A) 4.25 × 10-14 mol L-1 
B) 0.470 mol L-1 
C) 2.13 × 10-14 mol L-1 
D) 0.198 mol L-1 
E) 0.235 mol L-1 
A) 4.25 × 10-14 mol L-1 
B) 0.470 mol L-1 
C) 2.13 × 10-14 mol L-1 
D) 0.198 mol L-1 
E) 0.235 mol L-1

Question 18

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

Accepted Answer

No. Polyprotic acids ionize in stages. A

Question 19

Identify the weak diprotic acid.

Accepted Answer

A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4 
A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4

Question 20

Which of the following bases is the weakest? The base is followed by its Kb value.

Accepted Answer

A) HOCH2CH2NH2, 3.2 × 10-5 
B) NH3, 1.76 × 10-5 
C) C5H5N, 1.7 × 10-9 
D) (CH3CH2)3N, 5.2 × 10-4 
E) CH3CH2NH2, 5.6 × 10-4 
A) HOCH2CH2NH2, 3.2 × 10-5 
B) NH3, 1.76 × 10-5 
C) C5H5N, 1.7 × 10-9 
D) (CH3CH2)3N, 5.2 × 10-4 
E) CH3CH2NH2, 5.6 × 10-4

Exam 15: Acids and Bases

Identify the diprotic acid.

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 mol L-1 in hydronium ion.

Calculate the pH of a solution that contains 7.8 × 10-6 mol L-1 OH⁻ at 25 °C.

What is the pH of a 0.30 mol L-1 pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is below:

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

Find the percent ionization of a 0.337 mol L-1 HF solution. The Ka for HF is 3.5 × 10-4.

Which of the following is a weak base?

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 mol L-1 OH⁻ at 25 °C. Also identify the solution as acidic, basic, or neutral.

Calculate the pH of a 0.080 mol L-1 carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L-1 in acid at 25 ∘C? The acid is followed by its Ka value.

Which Bronsted-Lowry acid is not considered to be a strong acid in water?

Determine the concentration of CO32- ions in a 0.18 mol L-1 H2CO3 solution. Carbonic acid is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

What is the hydronium ion concentration of a 0.150 mol L-1 hypochlorous acid solution with Ka = 3.5 × 10-8? The equation for the dissociation of hypochlorous acid is below:

List the compound that is formed from the reaction of carbon dioxide with water.

Determine the [OH-] concentration of a 0.741 mol L-1 KOH solution at 25 °C.

Identify the weakest acid.

Determine the [OH⁻] concentration in a 0.235 mol L-1 NaOH solution.

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

Identify the weak diprotic acid.

Which of the following bases is the weakest? The base is followed by its Kb value.

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Filters

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-4 mol L^-1 in hydronium ion.

Calculate the pH of a solution that contains 7.8 × 10^-6 mol L^-1 OH⁻ at 25 °C.

What is the pH of a 0.30 mol L^-1 pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is below:

Find the percent ionization of a 0.337 mol L^-1 HF solution. The K_a for HF is 3.5 × 10^-4.

Calculate the concentration of H₃O⁺ in a solution that contains 5.5 × 10^-5 mol L^-1 OH⁻ at 25 °C. Also identify the solution as acidic, basic, or neutral.

Calculate the pH of a 0.080 mol L^-1 carbonic acid solution, H₂CO₃₍_aq_),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L^-1in acid at 25 ^∘C? The acid is followed by its K_a value.

Determine the concentration of CO₃^2- ions in a 0.18 mol L^-1 H₂CO₃ solution. Carbonic acid is a diprotic acid with K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the hydronium ion concentration of a 0.150 mol L^-1 hypochlorous acid solution with K_a = 3.5 × 10^-8?The equation for the dissociation of hypochlorous acid is below:

Determine the [OH^-] concentration of a 0.741 mol L^-1 KOH solution at 25 °C.

Determine the [OH⁻] concentration in a 0.235 mol L^-1 NaOH solution.

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

Which of the following bases is the weakest? The base is followed by its K_b value.