Question 1

Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. Ksp = 1.0 × 10−11

Accepted Answer

A)  1.4 × 10 −4  M
B)  8.2 × 10 −5  M
C)  5.4 × 10 −5  M
D)  3.2 × 10 −6  M
E)  2.5 × 10 −12  MF) D) and E)
G) A) and E)

Question 2

At the equivalence point in an acid-base titration

Accepted Answer

A)  the [H 3O +] equals the K a of the acid.
B)  the [H 3O +] equals the K a of the indicator.
C)  the amounts of acid and base which have been combined are in their stoichiometric ratio.
D)  the pH is 7.0.
E)  the pH has reached a maximum.F) A) and D)
G) A) and E)

Question 3

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? For NaH2PO4, Ka = 6.2 × 10−8

Accepted Answer

A)  6.51
B)  6.91
C)  7.51
D)  7.90
E)  8.13F) C) and D)
G) A) and D)

Question 4

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For AgCl, Ksp = 1.8 × 10−10.

Accepted Answer

A)  1.8 × 10 −10 mol Ag +
B)  9.0 × 10 −10 mol Ag +
C)  9.0 × 10 −9 mol Ag +
D)  6.7 × 10 −8 mol Ag +
E)  1.3 × 10 −5 mol Ag +F) All of the above
G) A) and C)

Question 5

When 20.0 mL of 0.15 M hydrochloric acid is mixed with 20.0 mL of 0.10 M sodium hydroxide, the pH of the resulting solution is

Accepted Answer

A)  0.00.
B)  12.40.
C)  1.60.
D)  0.82.
E)  7.00.F) B) and D)
G) All of the above

Question 6

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 × 10−18

Accepted Answer

A)  4.0 × 10 −5  M
B)  1.8 × 10 −5  M
C)  4.0 × 10 −6  M
D)  1.5 × 10 −5  M
E)  −5  MF) None of the above
G) All of the above

Question 7

Which, if any, of the following aqueous mixtures would be a buffer system?

Accepted Answer

A)  CH 3COOH, NaH 2PO 4
B)  H 2CO 3, HCO 3 −
C)  H 2PO 4 − , HCO 3 −
D)  HSO 4 − , HSO 3 −
E)  None of these choices are correct.F) B) and D)
G) A) and B)

Question 8

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L−1)  with a strong base of the same concentration? −1)  with a strong base of the same concentration?   A) A B) B C) C D) D E) E" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  A
B)  B
C)  C
D)  D
E)  EF) None of the above
G) A) and E)

Question 9

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the highest pH?

Accepted Answer

A)  [H 2PO 4 −] = 0.50 M, [HPO 4 2−] = 0.50 M
B)  [H 2PO 4 −] = 1.0 M, [HPO 4 2−] = 1.0 M
C)  [H2PO4−] = 1.0 M, [HPO42−] = 0.50 M
D)  [H2PO4−] = 0.50 M, [HPO42−] = 1.0 M
E)  [H 2PO 4 −] = 0.75 M, [HPO 4 2−] = 1.0 MF) B) and D)
G) B) and C)

Question 10

Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 × 10−3

Accepted Answer

A)  4.2 × 10 −2  M
B)  5.9 × 10 −2  M
C)  7.7 × 10 −2  M
D)  3.5 × 10 −5  M
E)  3.5 × 10 −6  MF) C) and D)
G) A) and E)

Question 11

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Accepted Answer

A)  HOC 6H 4OCOOH, K a = 1.0 × 10 −3
B)  C 6H 4(COOH) 2, K a = 2.9 × 10 −4
C)  CH 3COOH, K a = 1.8 × 10 −5
D)  C 5H 5O 5COOH, K a = 4.0 × 10 −6
E)  HBrO, K a = 2.3 × 10 −9F) A) and E)
G) A) and D)

Question 12

Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 × 10−12

Accepted Answer

A)  1.4 × 10−4 M
B)  3.4 × 10 −5  M
C)  1.1 × 10 −5  M
D)  1.6 × 10 −6  M
E)  −6  MF) A) and B)
G) A) and E)

Question 13

The solubility of silver chloride __________ when dilute nitric acid is added to it.

Accepted Answer

A)  increases
B)  decreases
C)  does not change
D)  first increases, then decreases
E)  first decreases, then increasesF) D) and E)
G) A) and E)

Question 14

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. a for HClO? A) 1.1 × 10 −7 B) 3.5 × 10 −8 C) 1.2 × 10 −8 D) 4.9 × 10 −11 E) None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > What is the Ka for HClO?

Accepted Answer

A)  1.1 × 10 −7
B)  3.5 × 10 −8
C)  1.2 × 10 −8
D)  4.9 × 10 −11
E)  None of these choices are correct.F) A) and C)
G) D) and E)

Question 15

The equivalence point in a titration is defined as the point when the indicator changes color.

Accepted Answer

A) True 
 B)False

Question 16

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 × 10−4.

Accepted Answer

A)  1.3 g
B)  0.69 g
C)  6.9 g
D)  23 g
E)  1.5 gF) A) and B)
G) A) and C)

Question 17

Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

Accepted Answer

A)  0.10 mol L −1 HCl and 0.05 mol L −1 NaOH
B)  0.10 mol L −1 HCl and 0.15 mol L −1 NH 3
C)  0.10 mol L −1 HCl and 0.05 mol L −1 NH 3
D)  0.10 mol L −1 HCl and 0.20 mol L −1 CH 3COOH
E)  0.10 mol L −1 HCl and 0.20 mol L −1 NaClF) D) and E)
G) A) and D)

Question 18

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Accepted Answer

A)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
B)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
C)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
D)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
E)  None of these choices are correct.F) C) and E)
G) A) and E)

Question 19

Citric acid has an acid dissociation constant of 8.4 × 10−4. It would be most effective for preparation of a buffer with a pH of

Accepted Answer

A)  2.
B)  3.
C)  4.
D)  5.
E)  6.F) A) and B)
G) B) and C)

Question 20

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Accepted Answer

A)  BaF 2
B)  CuCl
C)  CuBr
D)  AgI
E)  None of these choices are correct.F) A) and C)
G) B) and D)

Exam 19: Ionic Equilibria in Aqueous Systems

The solubility of silver chloride __________ when dilute nitric acid is added to it.

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Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

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Which of the following acids should be used to prepare a buffer with a pH of 4.5?

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What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 × 10−4.

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Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L−1) with a strong base of the same concentration?

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Citric acid has an acid dissociation constant of 8.4 × 10−4. It would be most effective for preparation of a buffer with a pH of

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Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 × 10−3

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Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For AgCl, Ksp = 1.8 × 10−10.

Correct AnswerverifiedShow Answer

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the highest pH?

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A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. What is the Ka for HClO?

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A change in pH will significantly affect the solubility of which, if any, of the following compounds?

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What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? For NaH2PO4, Ka = 6.2 × 10−8

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Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 × 10−18

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Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. Ksp = 1.0 × 10−11

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When 20.0 mL of 0.15 M hydrochloric acid is mixed with 20.0 mL of 0.10 M sodium hydroxide, the pH of the resulting solution is

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Which, if any, of the following aqueous mixtures would be a buffer system?

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The equivalence point in a titration is defined as the point when the indicator changes color.

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At the equivalence point in an acid-base titration

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Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 × 10−12

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Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

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Correct Answer
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Correct Answer
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Correct Answer
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What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, K_a = 7.2 × 10⁻⁴.

Correct Answer
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Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L⁻¹) with a strong base of the same concentration?

Correct Answer
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Citric acid has an acid dissociation constant of 8.4 × 10⁻⁴. It would be most effective for preparation of a buffer with a pH of

Correct Answer
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Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂solution. K_sp = 5.9 × 10⁻³

Correct Answer
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Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. For AgCl, K_sp = 1.8 × 10⁻¹⁰.

Correct Answer
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Correct Answer
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A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. What is the K_a for HClO?

Correct Answer
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Correct Answer
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What is the pH of a buffer that consists of 0.20 M NaH₂PO₄and 0.40 M Na₂HPO₄? For NaH₂PO₄, K_a = 6.2 × 10⁻⁸

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Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 × 10⁻¹⁸

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Calculate the solubility of silver oxalate, Ag₂C₂O₄, in pure water. K_sp = 1.0 × 10⁻¹¹

Correct Answer
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Correct Answer
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Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 × 10⁻¹²

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Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

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