Question 1

Which of the following compounds is more soluble in a 0.10 M NH3(aq) solution than in pure neutral water

Accepted Answer

A)  CaF2 
B)  MgCO3 
C)  AgI 
D)  SrSO4 
E)  Ba(NO3)2 
A)  CaF2 
B)  MgCO3 
C)  AgI 
D)  SrSO4 
E)  Ba(NO3)2

Question 2

A solution is prepared by mixing 500. mL of 0.10 M NaOCl and 500. mL of 0.20 M HOCl. What is the pH of this solution 
[Ka(HOCl) = 3.2 * 10-8]

Accepted Answer

A)  4.10 
B)  7.00 
C)  7.19 
D)  7.49 
E)  7.80 
A)  4.10 
B)  7.00 
C)  7.19 
D)  7.49 
E)  7.80

Question 3

Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s) + 2CN-(aq) $\leftrightharpoons$ Ag(CN)2-(aq) + Cl-(aq)
For AgCl, Ksp = 1.6 * 10-10; for Ag(CN)2-, Kf = 1.0 * 1021.

Accepted Answer

A)  1.2 * 1011 
B)  1.4 * 1011 
C)  1.6 * 1011 
D)  1.8 * 1011 
E)  None of the above 
A)  1.2 * 1011 
B)  1.4 * 1011 
C)  1.6 * 1011 
D)  1.8 * 1011 
E)  None of the above

Question 4

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq) required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H+ in the lake

Accepted Answer

A)  1.8 * 10-4 M 
B)  2.0 * 10-4 M 
C)  2.2 * 10-4 M 
D)  2.4 * 10-4 M 
E)  None of the above 
A)  1.8 * 10-4 M 
B)  2.0 * 10-4 M 
C)  2.2 * 10-4 M 
D)  2.4 * 10-4 M 
E)  None of the above

Question 5

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution [Ka(C6H5COOH) = 6.5 * 10-5]

Accepted Answer

A)  3.3% 
B)  12% 
C)  1.3% 
D)  0.52% 
E)  0.065% 
A)  3.3% 
B)  12% 
C)  1.3% 
D)  0.52% 
E)  0.065%

Question 6

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Accepted Answer

A) True 
 B)False

Question 7

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Accepted Answer

A) True 
 B)False

Question 8

25.0 mL of a 0.100 M solution of NH3 is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is:

Accepted Answer

A)  Basic and before the equivalence point 
B)  Basic and after the equivalence point 
C)  Acidic and before the equivalence point 
D)  Acidic and after the equivalence point 
E)  Neutral and at the equivalence point 
A)  Basic and before the equivalence point 
B)  Basic and after the equivalence point 
C)  Acidic and before the equivalence point 
D)  Acidic and after the equivalence point 
E)  Neutral and at the equivalence point

Question 9

In which one of the following solutions will acetic acid have the greatest percent ionization

Accepted Answer

A)  0.1 M CH3COOH 
B)  0.1 M CH3COOH dissolved in 1.0 M HCl 
C)  0.1 M CH3COOH plus 0.1 M CH3COONa 
D)  0.1 M CH3COOH plus 0.2 M CH3COONa 
A)  0.1 M CH3COOH 
B)  0.1 M CH3COOH dissolved in 1.0 M HCl 
C)  0.1 M CH3COOH plus 0.1 M CH3COONa 
D)  0.1 M CH3COOH plus 0.2 M CH3COONa

Question 10

5.0 mL of 12 M NH3 is added to 500. mL of 0.050 M AgNO3. What concentration of silver ion will exist after equilibrium is established [Kf for Ag(NH3)2+ is 1.5 * 107.]

Accepted Answer

A)  8.2 * 10-6 M 
B)  8.4 * 10-6 M 
C)  8.6 * 10-6 M 
D)  8.8 * 10-6 M 
E)  None of the above 
A)  8.2 * 10-6 M 
B)  8.4 * 10-6 M 
C)  8.6 * 10-6 M 
D)  8.8 * 10-6 M 
E)  None of the above

Question 11

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20 [Ka(C6H5COOH) = 6.5 *10-5]

Accepted Answer

A)  10.1 
B)  10.3 
C)  10.5 
D)  10.7 
E)  None of the Above 
A)  10.1 
B)  10.3 
C)  10.5 
D)  10.7 
E)  None of the Above

Question 12

Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp = 8.1 *10-12).

Accepted Answer

A)  5.0 * 10-5 M 
B)  2.5 * 10-4 M 
C)  1.3 * 10-4 M 
D)  2.0 * 10-4 M 
E)  8.1 * 10-4 M 
A)  5.0 * 10-5 M 
B)  2.5 * 10-4 M 
C)  1.3 * 10-4 M 
D)  2.0 * 10-4 M 
E)  8.1 * 10-4 M

Question 13

A precipitate of AgCl will form when 0.050 mol NaCl(s) and 0.050 mol AgNO3(s) are dissolved in 500. mL of 3.0 M NH3. [Kf for Ag(NH3)2+ is 1.5 * 107; Ksp(AgCl) = 1.6 * 10-10]

Accepted Answer

A) True 
 B)False

Question 14

Calculate the pH of a solution that is 0.20M NH3(aq) and 0.35 M NH4Cl(aq).(Kb(NH3) = 1.8 x 10-5)

Accepted Answer

A)  9.01 
B)  9.21 
C)  9.41 
D)  9.61 
E)  None of the Above 
A)  9.01 
B)  9.21 
C)  9.41 
D)  9.61 
E)  None of the Above

Question 15

Calculate the molar solubility of lead (II) fluoride. (Ksp (PbF2 = 4.1 x 10-8))

Accepted Answer

A)  1.6 x 10-3 M 
B)  1.8 x 10-3 M 
C)  2.0 x 10-3 M 
D)  2.2 x 10-3 M 
E)  None of the above 
A)  1.6 x 10-3 M 
B)  1.8 x 10-3 M 
C)  2.0 x 10-3 M 
D)  2.2 x 10-3 M 
E)  None of the above

Question 16

The Ksp for silver(I) phosphate is 1.8 * 10-18. Calculate the molar solubility of silver(I) phosphate.

Accepted Answer

A)  1.6 * 10-5 M 
B)  2.1 * 10-5 M 
C)  3.7 * 10-5 M 
D)  7.2 * 10-1 M 
E)  1.8 * 10-1 M 
A)  1.6 * 10-5 M 
B)  2.1 * 10-5 M 
C)  3.7 * 10-5 M 
D)  7.2 * 10-1 M 
E)  1.8 * 10-1 M

Question 17

What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M HCOOH? to obtain a solution with a pH of 4.50 [Ka(HCOOH) = 1.7 * 10-4]

Accepted Answer

A)  540 mL 
B)  420 mL 
C)  80. mL 
D)  340 mL 
E)  500. mL 
A)  540 mL 
B)  420 mL 
C)  80. mL 
D)  340 mL 
E)  500. mL

Question 18

In which one of the following solutions will acetic acid have the greatest percent ionization

Accepted Answer

A)  0.1 M CH3COOH 
B)  0.1 M CH3COOH dissolved in 0.1 M HCl 
C)  0.1 M CH3COOH dissolved in 0.2 M HCl 
D)  0.1 M CH3COOH plus 0.1 M CH3COONa 
E)  0.1 M CH3COOH plus 0.2 M CH3COONa 
A)  0.1 M CH3COOH 
B)  0.1 M CH3COOH dissolved in 0.1 M HCl 
C)  0.1 M CH3COOH dissolved in 0.2 M HCl 
D)  0.1 M CH3COOH plus 0.1 M CH3COONa 
E)  0.1 M CH3COOH plus 0.2 M CH3COONa

Question 19

Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.7 * 10-6) solution.

Accepted Answer

A)  7.6 * 10-3 M 
B)  1.5 * 10-2 M 
C)  3.4 * 10-5 M 
D)  1.7 * 10-6 M 
E)  3.4 * 10-6 M 
A)  7.6 * 10-3 M 
B)  1.5 * 10-2 M 
C)  3.4 * 10-5 M 
D)  1.7 * 10-6 M 
E)  3.4 * 10-6 M

Question 20

340. mL of a 0.150 M solution of NH3(aq) is titrated with 0.100 M HCl. Calculate the pH of the solution after 350. mL of HCl has been added. (Ka(NH4+) = 5.6 x 10-10)

Accepted Answer

A)  8.71 
B)  8.91 
C)  9.11 
D)  9.31 
E)  None of the above 
A)  8.71 
B)  8.91 
C)  9.11 
D)  9.31 
E)  None of the above

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Which of the following compounds is more soluble in a 0.10 M NH3(aq) solution than in pure neutral water

A solution is prepared by mixing 500. mL of 0.10 M NaOCl and 500. mL of 0.20 M HOCl. What is the pH of this solution [Ka(HOCl) = 3.2 * 10-8]

Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s) + 2CN-(aq) ⇋\leftrightharpoons⇋ Ag(CN)2-(aq) + Cl-(aq) For AgCl, Ksp = 1.6 * 10-10; for Ag(CN)2-, Kf = 1.0 * 1021.

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq) required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H+ in the lake

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution [Ka(C6H5COOH) = 6.5 * 10-5]

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

25.0 mL of a 0.100 M solution of NH3 is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is:

In which one of the following solutions will acetic acid have the greatest percent ionization

5.0 mL of 12 M NH3 is added to 500. mL of 0.050 M AgNO3. What concentration of silver ion will exist after equilibrium is established [Kf for Ag(NH3)2+ is 1.5 * 107.]

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20 [Ka(C6H5COOH) = 6.5 *10-5]

Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp = 8.1 *10-12).

A precipitate of AgCl will form when 0.050 mol NaCl(s) and 0.050 mol AgNO3(s) are dissolved in 500. mL of 3.0 M NH3. [Kf for Ag(NH3)2+ is 1.5 * 107; Ksp(AgCl) = 1.6 * 10-10]

Calculate the pH of a solution that is 0.20M NH3(aq) and 0.35 M NH4Cl(aq).(Kb(NH3) = 1.8 x 10-5)

Calculate the molar solubility of lead (II) fluoride. (Ksp (PbF2 = 4.1 x 10-8))

The Ksp for silver(I) phosphate is 1.8 * 10-18. Calculate the molar solubility of silver(I) phosphate.

What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M HCOOH? to obtain a solution with a pH of 4.50 [Ka(HCOOH) = 1.7 * 10-4]

In which one of the following solutions will acetic acid have the greatest percent ionization

Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.7 * 10-6) solution.

340. mL of a 0.150 M solution of NH3(aq) is titrated with 0.100 M HCl. Calculate the pH of the solution after 350. mL of HCl has been added. (Ka(NH4+) = 5.6 x 10-10)

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Which of the following compounds is more soluble in a 0.10 M NH₃(aq) solution than in pure neutral water

A solution is prepared by mixing 500. mL of 0.10 M NaOCl and 500. mL of 0.20 M HOCl. What is the pH of this solution [K_a(HOCl) = 3.2 * 10^-8]

Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s) + 2CN^-(aq) $\leftrightharpoons$ Ag(CN)₂^-(aq) + Cl^-(aq) For AgCl, K_sp = 1.6 * 10^-10; for Ag(CN)₂^-, K_f = 1.0 * 10²¹.

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq) required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H⁺ in the lake

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution [K_a(C₆H₅COOH) = 6.5 * 10^-5]

The pH of a solution that is 0.20 M CH₃COOH and 0.20 M CH₃COONa should be higher than the pH of a 0.20 M CH₃COOH solution.

25.0 mL of a 0.100 M solution of NH₃ is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is:

5.0 mL of 12 M NH₃ is added to 500. mL of 0.050 M AgNO₃. What concentration of silver ion will exist after equilibrium is established [K_f for Ag(NH₃)₂⁺ is 1.5 * 10⁷.]

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20 [K_a(C₆H₅COOH) = 6.5 *10^-5]

Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (K_sp = 8.1 *10^-12).

A precipitate of AgCl will form when 0.050 mol NaCl(s) and 0.050 mol AgNO₃(s) are dissolved in 500. mL of 3.0 M NH₃. [K_f for Ag(NH₃)₂⁺ is 1.5 * 10⁷; K_sp(AgCl) = 1.6 * 10^-10]

Calculate the pH of a solution that is 0.20M NH₃(aq) and 0.35 M NH₄Cl(aq).(K_b(NH₃) = 1.8 x 10^-5)

Calculate the molar solubility of lead (II) fluoride. (K_sp (PbF₂ = 4.1 x 10^-8))

The K_sp for silver(I) phosphate is 1.8 * 10^-18. Calculate the molar solubility of silver(I) phosphate.

What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M HCOOH? to obtain a solution with a pH of 4.50 [K_a(HCOOH) = 1.7 * 10^-4]

Calculate the concentration of fluoride ions in a saturated barium fluoride (K_sp = 1.7 * 10^-6) solution.

340. mL of a 0.150 M solution of NH₃(aq) is titrated with 0.100 M HCl. Calculate the pH of the solution after 350. mL of HCl has been added. (K_a(NH₄⁺) = 5.6 x 10^-10)