Question 1

Al(OH)3 is an amphoteric hydroxide. The balanced ionic equation to show its reaction with KOH is: Al(OH)3 + KOH $\rarr$ K[Al(OH)4]

Accepted Answer

A) True 
 B)False

Question 2

Which of these species will act as a Lewis acid

Accepted Answer

A)  NH3 
B)  NH4+ 
C)  H2O 
D)  BF3 
E)  F- 
A)  NH3 
B)  NH4+ 
C)  H2O 
D)  BF3 
E)  F-

Question 3

Which one of these salts will form a neutral solution on dissolving in water

Accepted Answer

A)  NaCl 
B)  KNO2 
C)  NaCN 
D)  NH4NO3 
E)  FeCl3 
A)  NaCl 
B)  KNO2 
C)  NaCN 
D)  NH4NO3 
E)  FeCl3

Question 4

Calculate the pH of 2.6 *10-2 M KOH.

Accepted Answer

A)  12.41 
B)  15.59 
C)  2.06 
D)  7.00 
E)  1.59 
A)  12.41 
B)  15.59 
C)  2.06 
D)  7.00 
E)  1.59

Question 5

Calculate the pOH of a solution containing 0.25 g of HCl in 800. mL of solution.

Accepted Answer

A)  11.93 
B)  10.93 
C)  9.93 
D)  8.93 
E)  None of the above 
A)  11.93 
B)  10.93 
C)  9.93 
D)  8.93 
E)  None of the above

Question 6

Calculate the H+ ion concentration in a solution with a pH of 3.85.

Accepted Answer

A)  1.0 * 10-4 M 
B)  1.4 * 10-4 M 
C)  1.8 * 10-4 M 
D)  2.2 * 10-4 M 
E)  None of the above 
A)  1.0 * 10-4 M 
B)  1.4 * 10-4 M 
C)  1.8 * 10-4 M 
D)  2.2 * 10-4 M 
E)  None of the above

Question 7

Calculate the pH of a 0.021 M NaCN solution. [Ka(HCN) = 4.9 * 10-10]

Accepted Answer

A)  1.68 
B)  3.18 
C)  5.49 
D)  7.00 
E)  10.82 
A)  1.68 
B)  3.18 
C)  5.49 
D)  7.00 
E)  10.82

Question 8

The pOH of a solution is 9.60. Calculate the hydrogen ion concentration in this solution.

Accepted Answer

A)  2.5 * 10-10 M 
B)  6.0 * 10-9 M 
C)  4.0 * 10-5 M 
D)  2.4 * 10-4 M 
E)  1.0 * 10-14 M 
A)  2.5 * 10-10 M 
B)  6.0 * 10-9 M 
C)  4.0 * 10-5 M 
D)  2.4 * 10-4 M 
E)  1.0 * 10-14 M

Question 9

The salt hydrolysis reaction for NH4NO3 that represents the acidic or basic nature of the solution is:

Accepted Answer

A)  NH4+(aq) + H2O(l) $\leftrightharpoons$ NH3(aq) + H2(g) + OH-(aq) 
B)  NO3-(aq) + H2O(l) $\leftrightharpoons$ HNO3(aq) + OH-(aq) 
C)  NH4+(aq) + H2O(l) $\leftrightharpoons$ H3O+(aq) + NH3(aq) 
D)  NH4+(aq) + NO3-(aq) $\leftrightharpoons$ NH4NO3(aq) 
E)  NO3-(aq) + 3H2O(l) $\leftrightharpoons$ HNO$_3$(aq) + 2H$_3$O$^+$(aq) 
A)  NH4+(aq) + H2O(l) $\leftrightharpoons$ NH3(aq) + H2(g) + OH-(aq) 
B)  NO3-(aq) + H2O(l) $\leftrightharpoons$ HNO3(aq) + OH-(aq) 
C)  NH4+(aq) + H2O(l) $\leftrightharpoons$ H3O+(aq) + NH3(aq) 
D)  NH4+(aq) + NO3-(aq) $\leftrightharpoons$ NH4NO3(aq) 
E)  NO3-(aq) + 3H2O(l) $\leftrightharpoons$ HNO$_3$(aq) + 2H$_3$O$^+$(aq)

Question 10

The hydrolysis of NH4NO2 will result in which of the following types of solutions given: (Ka(NH4+) = 5.6 x 10-10, Kb(NO2-) = 2.2 x 10-11)

Accepted Answer

A)  acidic, pH  7 
C)  neutral, pH = 7 
A)  acidic, pH  7 
C)  neutral, pH = 7

Question 11

The pH of a sample of river water is 6.0. A sample of effluent from a food processing plant has a pH of 4.0. What is the ratio of hydronium ion concentration in the effluent to the hydronium ion concentration in the river

Accepted Answer

A)  1/3 times as acidic 
B)  1.5 times more acidic 
C)  10 times more acidic 
D)  100 times more acidic 
E)  None of the above 
A)  1/3 times as acidic 
B)  1.5 times more acidic 
C)  10 times more acidic 
D)  100 times more acidic 
E)  None of the above

Question 12

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

Accepted Answer

A)  1.0 * 10-14 M 
B)  5.6 * 10-5 M 
C)  4.0 * 10-25 M 
D)  2.5 * 10-4 M 
E)  5.6 * 10-4 M 
A)  1.0 * 10-14 M 
B)  5.6 * 10-5 M 
C)  4.0 * 10-25 M 
D)  2.5 * 10-4 M 
E)  5.6 * 10-4 M

Question 13

A 8.0 M solution of formic acid (HCOOH) is 0.47% ionized. What is the Ka of formic acid

Accepted Answer

A)  1.57 * 10-4 
B)  1.77 * 10-4 
C)  1.97 * 10-4 
D)  2.17 * 10-4 
E)  None of the above 
A)  1.57 * 10-4 
B)  1.77 * 10-4 
C)  1.97 * 10-4 
D)  2.17 * 10-4 
E)  None of the above

Question 14

Calculate the H+ ion concentration in a 8.8 * 10-4 M Ca(OH)2 solution.

Accepted Answer

A)  8.8 * 10-4 M 
B)  1.8 * 10-3 M 
C)  2.2 * 10-11 M 
D)  1.1 * 10-11 M 
E)  5.7 * 10-12 M 
A)  8.8 * 10-4 M 
B)  1.8 * 10-3 M 
C)  2.2 * 10-11 M 
D)  1.1 * 10-11 M 
E)  5.7 * 10-12 M

Question 15

The conjugate acid-base pairs in the reaction HSO4- + HF $\leftrightharpoons$ H2SO4 + F- are HF-F-; H2SO4-HSO4-

Accepted Answer

A) True 
 B)False

Question 16

Calculate the concentration of oxalate ion (C2O42-) in a 0.175 M solution of oxalic acid (C2H2O4). [For oxalic acid, Ka1 = 6.5 * 10-2, Ka2 = 6.1 * 10-5.]

Accepted Answer

A)  0.11 M 
B)  6.1 * 10-5 M 
C)  4.0 * 10-6 M 
D)  0.0791 M 
E)  0.175 M 
A)  0.11 M 
B)  6.1 * 10-5 M 
C)  4.0 * 10-6 M 
D)  0.0791 M 
E)  0.175 M

Question 17

A 0.10 M NH3 solution is 1.3% ionized. Calculate the H+ ion concentration.NH3 + H2O $\leftrightharpoons$ NH4+ + OH-

Accepted Answer

A)  1.3 * 10-3 M 
B)  7.7 * 10-2 M 
C)  7.7 * 10-12 M 
D)  0.13 M 
E)  0.10 M 
A)  1.3 * 10-3 M 
B)  7.7 * 10-2 M 
C)  7.7 * 10-12 M 
D)  0.13 M 
E)  0.10 M

Question 18

The equilibrium expression for the ionization of a weak monoprotic acid, HA, in water is:

Accepted Answer

A)  Ka = [HA]/[OH-][H3O+] 
B)  Ka = [OH-][H3O+]/[HA] 
C)  Ka = [H3O+][HA]/[A-] 
D)  Ka = [H3O+][A-]/[HA] 
E)  Ka = [HA]/[H3O+][A-] 
A)  Ka = [HA]/[OH-][H3O+] 
B)  Ka = [OH-][H3O+]/[HA] 
C)  Ka = [H3O+][HA]/[A-] 
D)  Ka = [H3O+][A-]/[HA] 
E)  Ka = [HA]/[H3O+][A-]

Exam 15: Acids and Bases

Al(OH)3 is an amphoteric hydroxide. The balanced ionic equation to show its reaction with KOH is: Al(OH)3 + KOH →\rarr→ K[Al(OH)4]

Which of these species will act as a Lewis acid

Which one of these salts will form a neutral solution on dissolving in water

Calculate the pH of 2.6 *10-2 M KOH.

Calculate the pOH of a solution containing 0.25 g of HCl in 800. mL of solution.

Calculate the H+ ion concentration in a solution with a pH of 3.85.

Calculate the pH of a 0.021 M NaCN solution. [Ka(HCN) = 4.9 * 10-10]

The pOH of a solution is 9.60. Calculate the hydrogen ion concentration in this solution.

The salt hydrolysis reaction for NH4NO3 that represents the acidic or basic nature of the solution is:

The hydrolysis of NH4NO2 will result in which of the following types of solutions given: (Ka(NH4+) = 5.6 x 10-10, Kb(NO2-) = 2.2 x 10-11)

The pH of a sample of river water is 6.0. A sample of effluent from a food processing plant has a pH of 4.0. What is the ratio of hydronium ion concentration in the effluent to the hydronium ion concentration in the river

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

A 8.0 M solution of formic acid (HCOOH) is 0.47% ionized. What is the Ka of formic acid

Calculate the H+ ion concentration in a 8.8 * 10-4 M Ca(OH)2 solution.

The conjugate acid-base pairs in the reaction HSO4- + HF ⇋\leftrightharpoons⇋ H2SO4 + F- are HF-F-; H2SO4-HSO4-

Calculate the concentration of oxalate ion (C2O42-) in a 0.175 M solution of oxalic acid (C2H2O4). [For oxalic acid, Ka1 = 6.5 * 10-2, Ka2 = 6.1 * 10-5.]

A 0.10 M NH3 solution is 1.3% ionized. Calculate the H+ ion concentration.NH3 + H2O ⇋\leftrightharpoons⇋ NH4+ + OH-

The equilibrium expression for the ionization of a weak monoprotic acid, HA, in water is:

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Al(OH)₃ is an amphoteric hydroxide. The balanced ionic equation to show its reaction with KOH is: Al(OH)₃ + KOH $\rarr$ K[Al(OH)₄]

Calculate the pH of 2.6 *10^-2 M KOH.

Calculate the H⁺ ion concentration in a solution with a pH of 3.85.

Calculate the pH of a 0.021 M NaCN solution. [K_a(HCN) = 4.9 * 10^-10]

The salt hydrolysis reaction for NH₄NO₃ that represents the acidic or basic nature of the solution is:

The hydrolysis of NH₄NO₂ will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(NO₂^-) = 2.2 x 10^-11)

A 8.0 M solution of formic acid (HCOOH) is 0.47% ionized. What is the K_a of formic acid

Calculate the H⁺ ion concentration in a 8.8 * 10^-4 M Ca(OH)₂ solution.

The conjugate acid-base pairs in the reaction HSO₄^- + HF $\leftrightharpoons$ H₂SO₄ + F^- are HF-F^-; H₂SO₄-HSO₄^-

Calculate the concentration of oxalate ion (C₂O₄^2-) in a 0.175 M solution of oxalic acid (C₂H₂O₄). [For oxalic acid, K_a1 = 6.5 * 10^-2, K_a2 = 6.1 * 10^-5.]

A 0.10 M NH₃ solution is 1.3% ionized. Calculate the H⁺ ion concentration.NH₃ + H₂O $\leftrightharpoons$ NH₄⁺ + OH^-