Deck 19: Ionic Equilibria in Aqueous Systems

Question 1

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

A) The pH will be greater than the pK_a of hypochlorous acid.
B) The pH will be less than the pK_a of hypochlorous acid.
C) The pH will be equal to the pK_a of hypochlorous acid.
D) The pH will equal the pK_b of sodium hypochlorite.
E) The pH will be none of the above.

Answer 1

The pH will be less than the pK_a of hypochlorous acid.

Question 2

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

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 NH₃
C) 0.10 mol L^-1 HCl and 0.05 mol L^-1 NH₃
D) 0.10 mol L^-1 HCl and 0.20 mol L^-1 CH₃COOH
E) 0.10 mol L^-1 HCl and 0.20 mol L^-1 NaCl

Answer 2

0.10 mol L^-1 HCl and 0.15 mol L^-1 NH₃

Question 3

Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L^-1 aqueous NH₃, will produce a buffer solution?

A) 0.10 mol L^-1 HCl
B) 0.20 mol L^-1 HCl
C) 0.10 mol L^-1 CH₃COOH
D) 0.050 mol L^-1 NaOH
E) 0.20 mol L^-1 NH₄Cl

Answer 3

0.20 mol L^-1 NH₄Cl

Question 4

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H₂PO₄^-] = [HPO₄^2-] = 0.35 M?

A) The pH will increase slightly.
B) The pH will increase significantly.
C) The pH will decrease slightly.
D) The pH will decrease significantly.
E) Since it is a buffer solution, the pH will not be affected.

Question 5

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH₃COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

A) 3.0 M CH₃COONa
B) 2.5 M CH₃COONa
C) 2.0 M CH₃COONa
D) 1.5 M CH₃COONa
E) 0.30 M CH₃COONa

Question 6

mL of aqueous CH₃COOH and 25. mL of aqueous CH₃COONa

Question 7

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

A) CH₃COOH, NaH₂PO₄
B) H₂CO₃, HCO₃^-
C) H₂PO₄^-, HCO₃^-
D) HSO₄^-, HSO₃^-
E) None of the above will be a buffer solution.

Question 8

A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH₃COOH). What is the pH of the buffer?

A) The pH will be pK_a - 0.30, where pK_a is that of acetic acid.
B) The pH will be greater than the pK_a for acetic acid.
C) The pH will be less than the value in answer a.
D) The pH will be equal to the pK_a for acetic acid.
E) More information is needed to solve the problem.

Question 9

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

A) 0.9 M CO₃^2- and 0.1 M HCO₃^-
B) 0.1 M CO₃^2- and 0.9 M HCO₃^-
C) 0.5 M CO₃^2- and 0.5 M HCO₃^-
D) 0.1 M CO₃^2- and 0.1 M HCO₃^-
E) They all have the same buffer capacity.

Question 10

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

A) 1 L of 0.9 M CO₃^2- and 0.1 M HCO₃^-
B) 1 L of 0.1 M CO₃^2- and 0.9 M HCO₃^-
C) 1 L of 0.5 M CO₃^2- and 0.5 M HCO₃^-
D) 1 L of 0.1 M CO₃^2- and 0.1 M HCO₃^-
E) They can all neutralize the same amount of hydrochloric acid.

Question 11

Which of the following has the highest buffer capacity?

A) 0.10 M H₂PO₄^-/0.10 M HPO₄^2-
B) 0.50 M H₂PO₄^-/0.10 M HPO₄^2-
C) 0.10 M H₂PO₄^-/0.50 M HPO₄^2-
D) 0.50 M H₂PO₄^-/0.50 M HPO₄^2-
E) They all have the same buffer capacity.

Question 12

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

A) It is a buffer, pH > pK_a of propanoic acid.
B) It is a buffer, pH < pK_a of propanoic acid.
C) It is a buffer, pH = pK_a of propanoic acid.
D) It is a buffer, pH = pK_b of sodium propanoate.
E) Since sodium hydroxide is a strong base, this is not a buffer.

Question 13

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

A) dissolving a small amount of solid sodium acetate
B) adding a small amount of dilute hydrochloric acid
C) adding a small amount of dilute sodium hydroxide
D) dissolving a small amount of solid sodium chloride
E) diluting the buffer solution with water

Question 14

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO^-] = 0.5 M?

A) The pH will increase slightly.
B) The pH will increase significantly.
C) The pH will decrease slightly.
D) The pH will decrease significantly.
E) Since it is a buffer solution, the pH will not be affected.

Question 15

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

A) [CH₃COOH] = 0.25 M, [CH₃COO^-] = 0.25 M
B) [CH₃COOH] = 0.75 M, [CH₃COO^-] = 0.75 M
C) [CH₃COOH] = 0.75 M, [CH₃COO^-] = 0.25 M
D) [CH₃COOH] = 0.25 M, [CH₃COO^-] = 0.75 M
E) [CH₃COOH] = 1.00 M, [CH₃COO^-] = 1.00 M

Question 16

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

A) HCl, NaCl
B) HNO₃, NaNO₃
C) H₃PO₄, H₂PO₄^-
D) H₂SO₄, CH₃COOH
E) NH₃, NaOH

Question 17

A solution is prepared by adding 100 mL of 0.2 M hydrochloric acid to 100 mL of 0.4 M sodium formate. Is this a buffer solution, and if so, what is its pH?

A) It is a buffer, pH > pK_a of formic acid.
B) It is a buffer, pH < pK_a of formic acid.
C) It is a buffer, pH = pK_a of formic acid.
D) It is a buffer, pH = pK_b of sodium formate.
E) Since hydrochloric acid is a strong acid, this is not a buffer.

Question 18

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

A) HOC₆H₄OCOOH, K_a = 1.0 × 10^-3
B) C₆H₄(COOH)₂, K_a = 2.9 × 10^-4
C) CH₃COOH, K_a = 1.8 × 10^-5
D) C₅H₅O₅COOH, K_a = 4.0 × 10^-6
E) HBrO, K_a = 2.3 × 10^-9

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

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

Question 20

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

A) [H₂PO₄^-] = 0.50 M, [HPO₄^2-] = 0.50 M
B) [H₂PO₄^-] = 1.0 M, [HPO₄^2-] = 1.0 M
C) [H₂PO₄^-] = 1.0 M, [HPO₄^2-] = 0.50 M
D) [H₂PO₄^-] = 0.50 M, [HPO₄^2-] = 1.0 M
E) [H₂PO₄^-] = 0.75 M, [HPO₄^2-] = 1.0 M

Question 21

A phosphate buffer (H₂PO₄^-/HPO₄^2-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

A) dissolving a small amount of Na₂HPO₄
B) dissolving a small amount of NaH₂PO₄
C) adding a small amount of dilute hydrochloric acid
D) adding a small amount of dilute phosphoric acid
E) making the buffer more concentrated by removing some water

Question 22

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units? If necessary, assume the total volume remains unchanged at 400 mL.

A) 0.025 mol HCl
B) 0.063 mol HCl
C) 0.082 mol HCl
D) 0.50 mol HCl
E) 1.0 mol HCl

Question 23

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈ (ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 × 10^-4

A) 2.0 × 10^-3 M
B) 1.1 × 10^-3 M
C) 6.3 × 10^-9 M
D) 2.1 × 10^-10 M
E) 5.0 × 10^-11 M

Question 24

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? K_a = 1.8 × 10^-5

A) 4.49
B) 4.64
C) 4.85
D) 5.00
E) 5.52

Question 25

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10^-8

A) 7.8 × 10^-9 M
B) 1.8 × 10^-8 M
C) 6.7 × 10^-8 M
D) 1.6 × 10^-7 M
E) none of the above

Question 26

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10^-4

A) 1.1 × 10^-4 M
B) 2.6 × 10^-4 M
C) 4.3 × 10^-4 M
D) 6.7 × 10^-5 M
E) none of the above

Question 27

You need to use KH₂PO₄ and K₂HPO₄ to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H₃PO₄), K_a2 = 6.2 × 10^-8.

A) [base]/[acid] = 1.75
B) [base]/[acid] = 1.27
C) [base]/[acid] = 1.24
D) [base]/[acid] = 0.79
E) [base]/[acid] = 0.57

Question 28

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 NH₄Cl? K_b = 1.8 × 10^-5

A) 1.1 × 10^-5 M
B) 3.0 × 10^-6 M
C) 3.3 × 10^-9 M
D) 9.3 × 10^-10 M
E) none of the above

Question 29

The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H₂CO₃) and the bicarbonate (hydrogen carbonate, HCO₃^-) ion. What is the ratio of [bicarbonate]/[carbonic acid] at this pH? For carbonic acid, K_a1 = 4.2 × 10^-7.

A) [bicarbonate]/[carbonic acid] = 0.11
B) [bicarbonate]/[carbonic acid] = 0.38
C) [bicarbonate]/[carbonic acid] = 2.65
D) [bicarbonate]/[carbonic acid] = 9.4
E) None of the above ratios is correct.

Question 30

Two buffer solutions are prepared using acetic acid and sodium acetate. Solution A contains 20.0 g of acetic acid (CH₃COOH) and 5.0 g of sodium acetate CH₃COONa). Solution B contains 10.0 g of acetic acid and 25.0 g of sodium acetate. What is the difference between the pH values of these two solutions? For acetic acid, K_a = 1.8 × 10^-5.

A) 0.0
B) 1.0
C) 2.0
D) 2.3
E) 4.6

Question 31

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

A) 6.51
B) 6.91
C) 7.51
D) 7.90
E) 8.13

Question 32

A solution is prepared by dissolving 20.0 g of K₂HPO₄ and 25.0 g of KH₂PO₄ in enough water to produce 1.0 L of solution. What is the pH of this buffer? For phosphoric acid (H₃PO₄), K_a2 = 6.2 × 10^-8.

A) 7.70
B) 7.42
C) 7.21
D) 7.00
E) 6.72

Question 33

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

A) 3.67
B) 3.78
C) 3.81
D) 3.85
E) 3.95

Question 34

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH. What is the pH of this buffer? K_a = 1.8 × 10^-5

A) 4.57
B) 4.52
C) 4.87
D) 4.92
E) 4.97

Question 35

What is the pK_a for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

A) < 4.00
B) 4.63
C) 4.87
D) 5.02
E) > 5.50

Question 36

What is the pH of a solution that consists of 0.50 M H₂C₆H₆O₆ (ascorbic acid) and 0.75 M NaHC₆H₆O₆ (sodium ascorbate)? For ascorbic acid, K_a = 6.8 × 10^-5

A) 3.76
B) 3.99
C) 4.34
D) 4.57
E) 5.66

Question 37

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10^{- 4}.

A) [base]/[acid] = 0.14
B) [base]/[acid] = 0.42
C) [base]/[acid] = 2.36
D) [base]/[acid] = 7.20
E) None of the above ratios is correct.

Question 38

An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

A) 4.77
B) 4.71
C) 4.68
D) 4.62
E) none of the above

Question 39

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.

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

Question 40

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? K_a = 1.7 × 10^-4

A) 2.87
B) 3.72
C) 3.82
D) 3.95
E) 4.66

Question 41

If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, K_a = 6.8 × 10^-4.

A) 7.13
B) 2.54
C) 1.57
D) 3.17
E) 4.86

Question 42

A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? K_b = 1.8 × 10^-5

A) 10.26
B) 9.30
C) 9.21
D) 8.30
E) 8.21

Question 43

At the equivalence point in an acid-base titration

A) the [H₃O⁺] equals the K_a of the acid.
B) the [H₃O⁺] 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.

Question 44

A 20.0-mL sample of 0.30 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

A) 2.95
B) 3.13
C) 10.87
D) 11.05
E) 13.14

Question 45

When a strong acid is titrated with a strong base, the pH at the equivalence point

A) is greater than 7.0.
B) is equal to 7.0.
C) is less than 7.0, but is not 3.5.
D) is equal to the pK_a of the acid.
E) is equal to 3.5.

Question 46

When a strong acid is titrated with a weak base, the pH at the equivalence point

A) is greater than 7.0.
B) is equal to 7.0.
C) is less than 7.0.
D) is equal to the pK_a of the acid.
E) is equal to the pK_b of the base.

Question 47

A 20.0-mL sample of 0.25 M HNO₃ is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

A) 2.00
B) 1.60
C) 1.05
D) 1.00
E) none of the above

Question 48

Which of the following indicators would be the best to use when 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.05 M NaOH?

A) bromphenol blue, pH range: 3.0-4.5
B) bromcresol green, pH range: 3.8-5.4
C) alizarin, pH range: 5.7-7.2
D) phenol red, pH range: 6.9-8.2
E) phenolphthalein, pH range: 8.0-10.1

Question 49

When a weak acid is titrated with a weak base, the pH at the equivalence point

A) is greater than 7.0.
B) is equal to 7.0.
C) is less than 7.0.
D) is determined by the sizes of K_a and K_b.
E) is no longer affected by addition of base.

Question 50

A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? K_a = 1.77 × 10^-4

A) 4.00
B) 3.88
C) 3.63
D) 3.51
E) 3.47

Question 51

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

A) 1.26
B) 1.67
C) 12.33
D) 12.74
E) 13.03

Question 52

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? K_a = 1.3 × 10^-5

A) 5.75
B) 4.94
C) 4.83
D) 4.02
E) 3.95

Question 53

The indicator propyl red has K_a = 3.3 × 10^-6. What would be the approximate pH range over which it would change color?

A) 3.5-5.5
B) 4.5-6.5
C) 5.5-7.5
D) 6.5-8.5
E) none of the above

Question 54

When a weak acid is titrated with a strong base, the pH at the equivalence point

A) is greater than 7.0.
B) is equal to 7.0.
C) is less than 7.0.
D) is equal to the pK_a of the acid.
E) is equal to 14.0 - pK_b , where pK_b is that of the base.

Question 55

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?

A) 1.1 × 10^-7
B) 3.5 × 10^-8
C) 1.2 × 10^-8
D) 4.9 × 10^-11
E) none of the above

Question 56

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

A) 0.00.
B) 12.40.
C) 1.60.
D) 0.82.
E) 7.00.

Question 57

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak base (0.10 mol L^-1) with HCl of the same concentration?

A)

B)

C)

D)

E)

Question 58

A 25.0-mL sample of 0.10 M C₂H₃NH₂ (ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? K_b = 6.5 × 10^-4

A) 11.08
B) 10.88
C) 10.74
D) 10.55
E) 10.49

Question 59

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

A) 0.85
B) 0.75
C) 0.66
D) 0.49
E) 3.8

Question 60

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

A)

B)

C)

D)

E)

Question 61

A diprotic acid H₂A has K_a1 = 1 × 10^-4 and K_a2 = 1 × 10^-8. The corresponding base A^2- is titrated with aqueous HCl, both solutions being 0.1 mol L^-1. Which one of the following diagrams best represents the titration curve which will be seen?

A)

B)

C)

D)

E)

Question 62

Calculate the solubility of barium carbonate, BaCO₃, in pure water. K_sp = 2.0 × 10^-9

A) 1.3 × 10^-3 M
B) 3.2 × 10^-5 M
C) 2.2 × 10^-5 M
D) 4.5 × 10^-5 M
E) 4.0 × 10^-18 M

Question 63

A saturated solution of calcium hydroxide, Ca(OH)₂, is in contact with excess solid Ca(OH)₂. Which of the following statements correctly describes what will happen when aqueous HCl (a strong acid) is added to this mixture, and system returns to equilibrium? (For Ca(OH)₂, K_sp = 6.5 × 10^-6))

A) The solubility of Ca(OH)₂ will be unchanged.
B) The OH^- concentration will decrease and the Ca²⁺ concentration will increase.
C) The OH^- concentration will increase and the Ca²⁺ concentration will decrease.
D) The concentrations of both Ca²⁺ and OH^- will increase.
E) The solubility of Ca(OH)₂ will decrease.

Question 64

Write the ion product expression for magnesium fluoride, MgF₂.

A)
B)
C)
D)
E)

Question 65

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

A) BaF₂
B) CuCl
C) CuBr
D) AgI
E) None of the solubilities will be significantly affected.

Question 66

Which of the following substances has the greatest solubility in water?

A) MgCO₃, K_sp = 3.5 × 10^-8
B) NiCO₃, K_sp = 1.3 × 10^-7
C) AgIO₃, K_sp = 3.1 × 10^-8
D) CuBr, K_sp = 5.0 × 10^-9
E) AgCN, K_sp = 2.2 × 10^-16

Question 67

Write the ion product expression for silver sulfide, Ag₂S.

A)
B)
C)
D)
E)

Question 68

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

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 M

Question 69

What volume of 0.200 M KOH must be added to 17.5 mL of 0.135 M H₃PO₄ to reach the third equivalence point?

A) 3.94 mL
B) 11.8 mL
C) 17.5 mL
D) 23.6 mL
E) 35.4 mL

Question 70

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

A) 4.0 × 10^-5 M
B) 1.8 × 10^-5 M
C) 4.0 × 10^-6 M
D) 1.5 × 10^-6 M
E) < 1.0 × 10^-6 M

Question 71

The solubility of calcium chromate is 1.56 × 10^-3 g/100 mL of solution. What is the K_sp for CaCrO₄?

A) 2.4 × 10^-4
B) 1.5 × 10^-5
C) 7.6 × 10^-6
D) 1.0 × 10^-8
E) < 1.0 × 10^-8

Question 72

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

A)
B)
C)
D)
E) None of the above is the correct ion product expression.

Question 73

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

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

Question 74

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

A) 4.9 × 10^-2
B) 1.7 × 10^-5
C) 8.5 × 10^-6
D) 4.2 × 10^-6
E) < 1.0 × 10^-6

Question 75

What volume of 0.500 M H₂SO₄ is needed to react completely with 20.0 mL of 0.400 M LiOH?

A) 4.00 mL
B) 8.00 mL
C) 12.5 mL
D) 16.0 mL
E) 32.0 mL

Question 76

When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

A) H₂S
B) H₂C₂O₄
C) H₂C₄H₄O₆
D) H₂Se
E) H₂Te

Question 77

Which of the following substances has the greatest solubility in water?

A) PbI₂, K_sp = 7.9 × 10^-9
B) BaF₂, K_sp = 1.5 × 10^-6
C) Ca(OH)₂, K_sp = 6.5 × 10^-6
D) Zn(IO₃)₂, K_sp = 3.9 × 10^-6
E) Ag₂SO₄, K_sp = 1.5 × 10^-5

Question 78

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

A) 37.0 g/mol
B) 81.0 g/mol
C) 128 g/mol
D) 20.3 g/mol
E) 211 g/mol

Question 79

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

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

Question 80

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄)₂?

A) 6.5 × 10^-12
B) 6.0 × 10^-14
C) 5.2 × 10^-24
D) 4.8 × 10^-26
E) 1.0 × 10^-26