Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl2, 95.21 g/mol, Ksp = 740). How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

A) 9.0 kg B) 12 kg C) 57 kg D) 5.4 kg E) 7.2 kg A) 9.0 kg B) 12 kg C) 57 kg D) 5.4 kg E) 7.2 kg D

When [H+] = 4.0 F1F1F1S1F1F1F10 10-9 M in water at 25°C, then __________

A) pH = 9.40. B) pH = 7.00. C) pH = -8.40. D) pH = 8.40. E) pH = -9.40 A) pH = 9.40. B) pH = 7.00. C) pH = -8.40. D) pH = 8.40. E) pH = -9.40

Exam 17: Equilibrium in the Aqueous Phase

Magnesium sulfate can be obtained at a drugstore as Epsom salts. The monohydrate is found as the mineral kieserite. What would be the pH of a 500 mL aqueous solution containing 1.62 g kieserite? The value for sulfuric acid is 1.2  10^-².

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(Multiple Choice)

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Question 1

Correct Answer:

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Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl₂, 95.21 g/mol, K_sp = 740). How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

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(Multiple Choice)

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Question 2

Correct Answer:

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Research with biochemical systems commonly requires buffers because __________

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Question 3

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If 500 mL of a solution containing 1.00 g of barium nitrate (199.33 g/mol) is combined with 500 mL of a solution containing 1.00 g of sodium sulfate (142.03 g/mol), will there be a precipitate? Barium sulfate has a K_sp value of 9.1  10^-¹¹.

(Multiple Choice)

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Question 4

When [H⁺] = 4.0  10^-⁹ M in water at 25°C, then __________

(Multiple Choice)

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Question 5

Which one of the following salts forms aqueous solutions with pH = 7?

(Multiple Choice)

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Question 6

To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a buffer solution by dissolving sodium dihydrogen phosphate (K_a = 6.2  10^-⁸) and sodium hydrogen phosphate (K_a= 3.6  10^-¹³) together in an aqueous solution. What mole ratio of Na₂HPO₄/NaH₂PO₄ did she need to use?

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Question 7

Which combination of solutions is the best choice for making a buffer solution?

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Question 8

Which one, A-D, is not related to the water autoionization constant, K_w? If all are related, respond E.

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Question 9

A solution of hydrochloric acid (HCl, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the hydrochloric acid?

(Multiple Choice)

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Question 10

Which of the following groups, A-D, consist of salts that all form basic solutions in water? (Ac = acetate) If none or all satisfy this criterion, respond E.

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Question 11

A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl. It was found that the solution contained 0.125 moles of quinine. What was the pH of the solution after 50.00 mL of the HCl solution were added? Quinine is monobasic with pK_b = 5.10.

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Question 12

Which of these is a strong acid that ionizes to make a weak acid?

(Multiple Choice)

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Question 13

Aqueous solutions of __________ are basic.

(Multiple Choice)

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Question 14

Which of the following is a strong acid?

(Multiple Choice)

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Question 15

Ammonia (NH₃) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

(Multiple Choice)

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Question 16

What is the actual concentration of the molecular form of HF in a 1.0 M HF solution given that K_a of HF is 6.8  10^-⁴?

(Multiple Choice)

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Question 17

What is the pH of a 0.500 M solution of trimethylamine (pK_b = 4.13)?

(Multiple Choice)

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Question 18

A substance that can act as both an acid and base is __________

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Question 19

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

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Question 20

Showing 1 - 20 of 156

Exam 17: Equilibrium in the Aqueous Phase

Magnesium sulfate can be obtained at a drugstore as Epsom salts. The monohydrate is found as the mineral kieserite. What would be the pH of a 500 mL aqueous solution containing 1.62 g kieserite? The value for sulfuric acid is 1.2  10-2.

Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl2, 95.21 g/mol, Ksp = 740). How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

Research with biochemical systems commonly requires buffers because __________

If 500 mL of a solution containing 1.00 g of barium nitrate (199.33 g/mol) is combined with 500 mL of a solution containing 1.00 g of sodium sulfate (142.03 g/mol), will there be a precipitate? Barium sulfate has a Ksp value of 9.1  10-11.

When [H+] = 4.0  10-9 M in water at 25°C, then __________

Which one of the following salts forms aqueous solutions with pH = 7?

Which combination of solutions is the best choice for making a buffer solution?

Which one, A-D, is not related to the water autoionization constant, Kw? If all are related, respond E.

A solution of hydrochloric acid (HCl, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the hydrochloric acid?

Which of the following groups, A-D, consist of salts that all form basic solutions in water? (Ac = acetate) If none or all satisfy this criterion, respond E.

A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl. It was found that the solution contained 0.125 moles of quinine. What was the pH of the solution after 50.00 mL of the HCl solution were added? Quinine is monobasic with pKb = 5.10.

Which of these is a strong acid that ionizes to make a weak acid?

Aqueous solutions of __________ are basic.

Which of the following is a strong acid?

Ammonia (NH3) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

What is the actual concentration of the molecular form of HF in a 1.0 M HF solution given that Ka of HF is 6.8  10-4?

What is the pH of a 0.500 M solution of trimethylamine (pKb = 4.13)?

A substance that can act as both an acid and base is __________

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

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Magnesium sulfate can be obtained at a drugstore as Epsom salts. The monohydrate is found as the mineral kieserite. What would be the pH of a 500 mL aqueous solution containing 1.62 g kieserite? The value for sulfuric acid is 1.2  10^-².

Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl₂, 95.21 g/mol, K_sp = 740). How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

If 500 mL of a solution containing 1.00 g of barium nitrate (199.33 g/mol) is combined with 500 mL of a solution containing 1.00 g of sodium sulfate (142.03 g/mol), will there be a precipitate? Barium sulfate has a K_sp value of 9.1  10^-¹¹.

When [H⁺] = 4.0  10^-⁹ M in water at 25°C, then __________

Which one, A-D, is not related to the water autoionization constant, K_w? If all are related, respond E.

A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl. It was found that the solution contained 0.125 moles of quinine. What was the pH of the solution after 50.00 mL of the HCl solution were added? Quinine is monobasic with pK_b = 5.10.

Ammonia (NH₃) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

What is the actual concentration of the molecular form of HF in a 1.0 M HF solution given that K_a of HF is 6.8  10^-⁴?

What is the pH of a 0.500 M solution of trimethylamine (pK_b = 4.13)?