Question 1

Calculate the concentration of malonate ion (C3H2O42-) in a 0.200 M solution of malonic acid (C3H4O4). [For malonic acid, Ka1 = 1.4 * 10-3, Ka2 = 2.0 * 10-6.]

Accepted Answer

A)  2.8 * 10-4 M 
B)  0.016 M 
C)  1.8 * 10-4 M 
D)  1.4 * 10-3 M 
E)  2.0 * 10-6 M 
A)  2.8 * 10-4 M 
B)  0.016 M 
C)  1.8 * 10-4 M 
D)  1.4 * 10-3 M 
E)  2.0 * 10-6 M E

Question 2

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 105 m3 of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident

Accepted Answer

A)  5.44 
B)  8.56 
C)  8.44 
D)  5.56 
E)  2.44 
A)  5.44 
B)  8.56 
C)  8.44 
D)  5.56 
E)  2.44 A

Question 3

The pH of a 0.095 M solution of an unknown monoprotic acid is 5.42. Calculate the Ka of the acid.

Accepted Answer

A)  3.8 x 10-6 
B)  3.6 x 10-7 
C)  1.5 x 10-10 
D)  2.6 x 10-9 
E)  2.8 x 10-8 
A)  3.8 x 10-6 
B)  3.6 x 10-7 
C)  1.5 x 10-10 
D)  2.6 x 10-9 
E)  2.8 x 10-8 C

Question 4

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C8H10N4O2). What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, Kb = 4.1 * 10-4.)

Accepted Answer

A)  2.76 
B)  7.67 
C)  10.96 
D)  6.33 
E)  11.24 
A)  2.76 
B)  7.67 
C)  10.96 
D)  6.33 
E)  11.24

Question 5

Write the chemical formula for the acid formed when Cl2O5 is dissolved in water.

Accepted Answer

A)  HClO 
B)  HClO2 
C)  HClO3 
D)  HClO4 
E)  None of the above 
A)  HClO 
B)  HClO2 
C)  HClO3 
D)  HClO4 
E)  None of the above

Question 6

The oxides SO2 and N2O5 will form the following acids in water, respectively.

Accepted Answer

A)  H2SO4(aq) and HNO3(aq) 
B)  H2SO3(aq) and HNO3(aq) 
C)  H2SO4(aq) and HNO2(aq) 
D)  H2SO3(aq) and HNO2(aq) 
E)  H2S(aq) and HNO3(aq) 
A)  H2SO4(aq) and HNO3(aq) 
B)  H2SO3(aq) and HNO3(aq) 
C)  H2SO4(aq) and HNO2(aq) 
D)  H2SO3(aq) and HNO2(aq) 
E)  H2S(aq) and HNO3(aq)

Question 7

Which of the following is not a conjugate acid-base pair

Accepted Answer

A)  H2O and OH- 
B)  H2O and H3O+ 
C)  H3O+ and OH- 
D)  HO2- and H2O2 
E)  O22- and HO2- 
A)  H2O and OH- 
B)  H2O and H3O+ 
C)  H3O+ and OH- 
D)  HO2- and H2O2 
E)  O22- and HO2-

Question 8

A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH solution. What is the pH of the mixture

Accepted Answer

A)  13.40 
B)  13.12 
C)  11.68 
D)  12.84 
E)  13.04 
A)  13.40 
B)  13.12 
C)  11.68 
D)  12.84 
E)  13.04

Question 9

Which one of the following equations represents the ionization of a weak monoprotic acid in water

Accepted Answer

A)  HCN(aq) + H2O(l) $\leftrightharpoons$ H3O+(aq) + CN-(aq) 
B)  HCN(aq) + OH-(aq) $\leftrightharpoons$ H2O(l) + CN+(aq) 
C)  CN- (aq) + H2O(aq) $\leftrightharpoons$ HCN(aq) + OH-(aq) 
D)  HCN(aq) + OH- (aq) $\leftrightharpoons$ H2O(l) + CN-(aq) 
E)  HCN(aq) + NH3(aq) $\leftrightharpoons$ NH$_4$CN(aq) 
A)  HCN(aq) + H2O(l) $\leftrightharpoons$ H3O+(aq) + CN-(aq) 
B)  HCN(aq) + OH-(aq) $\leftrightharpoons$ H2O(l) + CN+(aq) 
C)  CN- (aq) + H2O(aq) $\leftrightharpoons$ HCN(aq) + OH-(aq) 
D)  HCN(aq) + OH- (aq) $\leftrightharpoons$ H2O(l) + CN-(aq) 
E)  HCN(aq) + NH3(aq) $\leftrightharpoons$ NH$_4$CN(aq)

Question 10

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.0 and 10.0 mL of a strong acid solution with pH = 6.0

Accepted Answer

A)  2.0 
B)  2.3 
C)  4.0 
D)  6.0 
E)  8.0 
A)  2.0 
B)  2.3 
C)  4.0 
D)  6.0 
E)  8.0

Question 11

Which of the following yields an acidic solution when dissolved in water
I. NO2
II. NH4Cl
III. NaCl
IV. HNO2

Accepted Answer

A)  I and IV 
B)  II and III 
C)  I, II, and IV 
D)  I and III 
E)  I, II, III, and IV 
A)  I and IV 
B)  II and III 
C)  I, II, and IV 
D)  I and III 
E)  I, II, III, and IV

Question 12

In the reaction HSO4-(aq) + OH-(aq) $\leftrightharpoons$ SO42-(aq) + H2O(l), the conjugate acid-base pairs are 
$~~~~~~~~~\text { pair } 1 \quad~~~~~~~~~~~~~~~~~ \text { pair } 2$
A. $ \mathrm{HSO}_{4}^{-} $and $ \mathrm{SO}_{4}{ }^{2-} ; \quad\mathrm{H}_{2} \mathrm{O} $ and $ \mathrm{OH}^{-} $
B. $ \mathrm{HSO}_{4}^{-} $and $ \mathrm{H}_{3} \mathrm{O}^{-} ; \quad\mathrm{SO}_{4}{ }^{2-} $ and $ \mathrm{OH}^{-} $.
C. $ \mathrm{HSO}_{4}^{-} $and $ \mathrm{OH}^{-} ; \quad \mathrm{SO}_{4}^{2-} $ and $ \mathrm{H}_{2} \mathrm{O} $.
D. $ \mathrm{HSO}_{4}{ }^{-} $and $ \mathrm{H}_{2} \mathrm{O}; \quad\mathrm{OH}^{-} $and $ \mathrm{SO}_{4}{ }^{2-} $
E. $ \mathrm{HSO}_{4}^{-} $and $ \mathrm{OH}^{-} ; \quad \mathrm{SO}_{4}{ }^{2-} $ and $ \mathrm{H}_{3} \mathrm{O}^{+} $

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 13

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

Accepted Answer

A)  4.0 * 10-3 M 
B)  4.0 * 10-9 M 
C)  4.0 * 10-10 M 
D)  2.5 * 10-5 M 
E)  2.5 * 10-4 M 
A)  4.0 * 10-3 M 
B)  4.0 * 10-9 M 
C)  4.0 * 10-10 M 
D)  2.5 * 10-5 M 
E)  2.5 * 10-4 M

Question 14

Which of the following yields a basic solution when dissolved in water
I. NH3
II. Na2O
III. LiOH
IV. P4O10

Accepted Answer

A)  I and II 
B)  I and IV 
C)  II and III 
D)  I, II, and III 
E)  I, II, III, and IV 
A)  I and II 
B)  I and IV 
C)  II and III 
D)  I, II, and III 
E)  I, II, III, and IV

Question 15

What is the pH of a 0.11 M solution of $C_6H_5O\underline{H}$ (Ka = 1.3 x 10-10)

Accepted Answer

A)  0.96 
B)  10.84 
C)  5.42 
D)  9.89 
E)  4.11 
A)  0.96 
B)  10.84 
C)  5.42 
D)  9.89 
E)  4.11

Question 16

H3PO4 is a stronger acid than H3AsO4.

Accepted Answer

A) True 
 B)False

Question 17

In the reaction Ag+(aq) + Cl-(aq)$\rarr$ AgCl(s), Ag+ acts as a Lewis acid.

Accepted Answer

A) True 
 B)False

Question 18

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [Ka(HClO) = 4.0 * 10-8]

Accepted Answer

A)  20. g 
B)  0.032 g 
C)  4.1 g 
D)  2.4 g 
E)  9.1 g 
A)  20. g 
B)  0.032 g 
C)  4.1 g 
D)  2.4 g 
E)  9.1 g

Question 19

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 * 10-8 and Ka2 = 1 * 10-19. Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Accepted Answer

A)  0.10 M 
B)  7.5 * 10-5 M 
C)  5.7 * 10-9 M 
D)  1 * 10-19 M 
E)  1 * 10-20 M 
A)  0.10 M 
B)  7.5 * 10-5 M 
C)  5.7 * 10-9 M 
D)  1 * 10-19 M 
E)  1 * 10-20 M

Question 20

Calculate the pOH for a solution with [H3O+] = 3.1 x 10-9 M.

Accepted Answer

A)  3.10 
B)  10.90 
C)  8.51 
D)  5.49 
E)  3.2 x 10-6 
A)  3.10 
B)  10.90 
C)  8.51 
D)  5.49 
E)  3.2 x 10-6

Exam 15: Acids and Bases

Calculate the concentration of malonate ion (C3H2O42-) in a 0.200 M solution of malonic acid (C3H4O4). [For malonic acid, Ka1 = 1.4 * 10-3, Ka2 = 2.0 * 10-6.]

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 105 m3 of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident

The pH of a 0.095 M solution of an unknown monoprotic acid is 5.42. Calculate the Ka of the acid.

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C8H10N4O2). What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, Kb = 4.1 * 10-4.)

Write the chemical formula for the acid formed when Cl2O5 is dissolved in water.

The oxides SO2 and N2O5 will form the following acids in water, respectively.

Which of the following is not a conjugate acid-base pair

A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH solution. What is the pH of the mixture

Which one of the following equations represents the ionization of a weak monoprotic acid in water

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.0 and 10.0 mL of a strong acid solution with pH = 6.0

Which of the following yields an acidic solution when dissolved in water I. NO2 II. NH4Cl III. NaCl IV. HNO2

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

Which of the following yields a basic solution when dissolved in water I. NH3 II. Na2O III. LiOH IV. P4O10

What is the pH of a 0.11 M solution of C6H5OH‾C_6H_5O\underline{H}C6​H5​OH​ (Ka = 1.3 x 10-10)

H3PO4 is a stronger acid than H3AsO4.

In the reaction Ag+(aq) + Cl-(aq) →\rarr→ AgCl(s), Ag+ acts as a Lewis acid.

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [Ka(HClO) = 4.0 * 10-8]

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 * 10-8 and Ka2 = 1 * 10-19. Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Calculate the pOH for a solution with [H3O+] = 3.1 x 10-9 M.

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Calculate the concentration of malonate ion (C₃H₂O₄^2-) in a 0.200 M solution of malonic acid (C₃H₄O₄). [For malonic acid, K_a1 = 1.4 * 10^-3, K_a2 = 2.0 * 10^-6.]

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 10⁵ m³ of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident

The pH of a 0.095 M solution of an unknown monoprotic acid is 5.42. Calculate the K_a of the acid.

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C₈H₁₀N₄O₂). What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, K_b = 4.1 * 10^-4.)

Write the chemical formula for the acid formed when Cl₂O₅ is dissolved in water.

The oxides SO₂ and N₂O₅ will form the following acids in water, respectively.

Which of the following yields an acidic solution when dissolved in water I. NO₂ II. NH₄Cl III. NaCl IV. HNO₂

Which of the following yields a basic solution when dissolved in water I. NH₃ II. Na₂O III. LiOH IV. P₄O₁₀

What is the pH of a 0.11 M solution of $C_6H_5O\underline{H}$ (K_a = 1.3 x 10^-10)

H₃PO₄ is a stronger acid than H₃AsO₄.

In the reaction Ag⁺(aq) + Cl^-(aq) $\rarr$ AgCl(s), Ag⁺ acts as a Lewis acid.

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [K_a(HClO) = 4.0 * 10^-8]

Hydrosulfuric acid is a diprotic acid, for which K_a1 = 5.7 * 10^-8 and K_a2 = 1 * 10^-19. Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Calculate the pOH for a solution with [H₃O⁺] = 3.1 x 10^-9 M.