What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10-5 for calcium sulfate.

A) 1.2 × 10-2 mol B) 4.9 × 10-3 mol C) 3.5 × 10-3 mol D) 1.2 × 10-5 mol E) 4.8 × 10-8 mol A) 1.2 × 10-2 mol B) 4.9 × 10-3 mol C) 3.5 × 10-3 mol D) 1.2 × 10-5 mol E) 4.8 × 10-8 mol

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, Ka = 6.8 × 10-5

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

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8 (ethylene diamine) and 0.35 C2N2H9Cl? Kb = 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 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

Exam 19: Ionic Equilibria in Aqueous Systems

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10^-5 for calcium sulfate.

(Multiple Choice)

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Question 81

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

(Multiple Choice)

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Question 82

Hydrofluoric acid (HF) has a K_a value of 7.2 × 10^-4. a. 0.250 mol of F^- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L^-1 aqueous HF. Calculate the resulting pH. b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L^-1 NaOH. Calculate the resulting pH.

(Essay)

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Question 83

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

(True/False)

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Question 84

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

(Multiple Choice)

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Question 85

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?

(Multiple Choice)

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Question 86

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

(True/False)

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Question 87

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO₃)₂with 50.0 mL of 0.50 M Co(NO₃)₂. Sodium hydroxide is added to the mixture. Which hydroxide precipitates first and what concentration of hydroxide ions present in solution will accomplish the separation? K_sp = 2.2 × 10^-20 for Cu(OH)₂, K_sp = 1.3 × 10^-15for Co(OH)₂

(Multiple Choice)

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Question 88

Write the ion product expression for magnesium fluoride, MgF₂.

(Multiple Choice)

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Question 89

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 90

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

(Multiple Choice)

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Question 91

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

(Multiple Choice)

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Question 92

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

(Multiple Choice)

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Question 93

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?

(Multiple Choice)

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Question 94

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 95

Calculate the solubility of copper(II) carbonate, CuCO₃, in 1.00 mol L^-1 NH₃. K_sp = 3.0 × 10^-12 for CuCO₃, K_f = 5.6 × 10¹¹ for Cu(NH₃)₄²⁺

(Short Answer)

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Question 96

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

(Multiple Choice)

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Question 97

Use the following information to calculate the solubility product constant, K_sp, for CuCl. A saturated solution of CuCl in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid CuClresidue recovered in the beaker was found to weigh 0.041g.

(Multiple Choice)

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Question 98

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}.

(Multiple Choice)

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Question 99

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?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 119

Exam 19: Ionic Equilibria in Aqueous Systems

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10-5 for calcium sulfate.

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, Ka = 6.8 × 10-5

Hydrofluoric acid (HF) has a Ka value of 7.2 × 10-4. a. 0.250 mol of F- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L-1 aqueous HF. Calculate the resulting pH. b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L-1 NaOH. Calculate the resulting pH.

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

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

A popular buffer solution consists of carbonate (CO32-) 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?

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

Write the ion product expression for magnesium fluoride, MgF2.

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?

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? Ka = 1.7 × 10-4

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? Ka = 1.3 × 10-5

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?

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

Calculate the solubility of copper(II) carbonate, CuCO3, in 1.00 mol L-1 NH3. Ksp = 3.0 × 10-12 for CuCO3, Kf = 5.6 × 1011 for Cu(NH3)42+

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

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, Ka = 7.2 × 10- 4.

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?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The 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: Bonding, Structure, and Reactivity

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 the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10^-5 for calcium sulfate.

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

Hydrofluoric acid (HF) has a K_a value of 7.2 × 10^-4. a. 0.250 mol of F^- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L^-1 aqueous HF. Calculate the resulting pH. b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L^-1 NaOH. Calculate the resulting pH.

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 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?

Write the ion product expression for magnesium fluoride, MgF₂.

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 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 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 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?

Calculate the solubility of copper(II) carbonate, CuCO₃, in 1.00 mol L^-1 NH₃. K_sp = 3.0 × 10^-12 for CuCO₃, K_f = 5.6 × 10¹¹ for Cu(NH₃)₄²⁺

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}.

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?