Barium sulfate (BaSO4) is a slightly soluble salt, with Ksp = 1.1 × 10-10. What mass of Ba2+ ions will be present in 1.0 L of a saturated solution of barium sulfate?

A) -7 g B) 1.0 × 10-5 g C) 0.0014 g D) 0.0024 g E) > 0.05 g A) -7 g B) 1.0 × 10-5 g C) 0.0014 g D) 0.0024 g E) > 0.05 g C

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO3)2. Which of the following statements is correct? Ksp = 6.44 × 10-3 for CdF2.

A) Cadmium fluoride precipitates until the solution is saturated. B) The solution is unsaturated and no precipitate forms. C) The solubility of cadmium fluoride is increased by the presence of additional fluoride ions. D) One must know Ksp for cadmium nitrate to make meaningful predictions on this system. E) The presence of NaF will raise the solubility of Cd(NO3)2. A) Cadmium fluoride precipitates until the solution is saturated. B) The solution is unsaturated and no precipitate forms. C) The solubility of cadmium fluoride is increased by the presence of additional fluoride ions. D) One must know Ksp for cadmium nitrate to make meaningful predictions on this system. E) The presence of NaF will raise the solubility of Cd(NO3)2. A

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

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

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 NH4Cl? Kb = 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 these choices are correct. 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 these choices are correct.

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

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 M 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 M

Exam 19: Ionic Equilibria in Aqueous Systems

Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 × 10^-10. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

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

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(True/False)

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Question 2

Correct Answer:

Verified

False

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃)₂. Which of the following statements is correct? K_sp = 6.44 × 10^-3 for CdF₂.

Free

(Multiple Choice)

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Question 3

Correct Answer:

Verified

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?

(Multiple Choice)

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Question 4

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

(Multiple Choice)

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Question 5

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

(Multiple Choice)

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Question 6

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

(Multiple Choice)

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Question 7

Which of the following has the highest buffer capacity?

(Multiple Choice)

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Question 8

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?

(Multiple Choice)

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Question 9

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

(Multiple Choice)

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Question 10

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?

(Multiple Choice)

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Question 11

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.

(Multiple Choice)

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Question 12

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

(Multiple Choice)

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Question 13

The salts X(NO₃)₂ and Y(NO₃)₂ (where X⁺ and Y⁺ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the K_sp values listed below, decide which aqueous reagent, if any, will definitely precipitate X⁺ before precipitating Y+ from solution. Given K_sp values: XCl₂, 1 × 10^-5 YCl₂, 1 × 10^-10 X(OH)₂, 1 × 10^-10 Y(OH)₂, 1 × 10^-5

(Multiple Choice)

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Question 14

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

(True/False)

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Question 15

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

(Multiple Choice)

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Question 16

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?

(Multiple Choice)

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Question 17

Which one of the following pairs of 0.100 mol L^-1 solutions, when mixed, will produce a buffer solution?

(Multiple Choice)

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Question 18

The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest? Hg(CN)₄^2- K_f = 9.3 × 10³⁸ Be(OH)₄^2- K_f = 4.0 × 10¹⁸ Zn(OH)₄^2- K_f = 3.0 × 10¹⁵ Cu(NH₃)₄²⁺ K_f = 5.6 × 10¹¹ CdI₄^2- K_f = 1.0 × 10⁶

(Multiple Choice)

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Question 19

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

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Question 20

Showing 1 - 20 of 114

Exam 19: Ionic Equilibria in Aqueous Systems

Barium sulfate (BaSO4) is a slightly soluble salt, with Ksp = 1.1 × 10-10. What mass of Ba2+ ions will be present in 1.0 L of a saturated solution of barium sulfate?

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

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO3)2. Which of the following statements is correct? Ksp = 6.44 × 10-3 for CdF2.

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?

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

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

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

Which of the following has the highest buffer capacity?

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?

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

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?

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.

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

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

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

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?

Which one of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution?

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

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Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 × 10^-10. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃)₂. Which of the following statements is correct? K_sp = 6.44 × 10^-3 for CdF₂.

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

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

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

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.

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

Which one of the following pairs of 0.100 mol L^-1 solutions, when mixed, will produce a buffer solution?