Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. Ksp = 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 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

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 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 −5 M E) −5 M 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 M

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

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

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

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 M 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 M

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

Exam 19: Ionic Equilibria in Aqueous Systems

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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?

(Multiple Choice)

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Question 61

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?

(Multiple Choice)

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Question 62

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

(Multiple Choice)

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Question 63

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

(Multiple Choice)

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Question 64

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

(Multiple Choice)

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Question 65

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

(Multiple Choice)

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Question 66

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

(Multiple Choice)

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Question 67

At the equivalence point in an acid-base titration

(Multiple Choice)

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Question 68

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

(Multiple Choice)

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Question 69

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 70

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

(Multiple Choice)

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Question 71

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

(Multiple Choice)

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Question 72

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

(True/False)

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Question 73

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.

(Multiple Choice)

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Question 74

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

(Multiple Choice)

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Question 75

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

(Multiple Choice)

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Question 76

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

(Multiple Choice)

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Question 77

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

(Multiple Choice)

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Question 78

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

(Multiple Choice)

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Question 79

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 80

Showing 61 - 80 of 114

Exam 19: Ionic Equilibria in Aqueous Systems

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?

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?

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

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

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

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

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

At the equivalence point in an acid-base titration

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

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

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

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

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

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.

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

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

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

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

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.

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

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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?

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?

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

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

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

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

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 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.

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

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

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.