(a) Interpretation: The value of K a for the given weak acid based on the equilibrium concentrations and pH values is to be calculated. Concept introduction: pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H + and OH − ions at a particular temperature. The dissociation constant of a weak acid is denoted by K a . It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

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Answer 1

Question

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

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8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?

Answer 2

Question

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

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Answer 3

Question

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

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Answer 4

Question

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

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Answer 5

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 6

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 7

Chapter 9, Problem 9.129E

Interpretation Introduction

(a)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 10

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 11

Interpretation Introduction

(c)

Interpretation:

The value of Ka for the given weak acid based on the equilibrium concentrations and pH values is to be calculated.

Concept introduction:

pH of a solution is the value of negative logarithm of the concentration of hydrogen ions in a solution. Ionic product of water is obtained by taking the product of the concentrations of H+ and OH− ions at a particular temperature. The dissociation constant of a weak acid is denoted by Ka. It is equal to the ratio of concentration of products to the concentration of reactants in the dissociation reaction of the weak acid.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 9 - Write the dissociation equations for the following...Ch. 9 - Write the dissociation equations for the following...Ch. 9 - Each of the following produces a basic solution...Ch. 9 - Prob. 9.4E Ch. 9 - Identify each Brnsted acid and base in the...Ch. 9 - Prob. 9.6E Ch. 9 - Prob. 9.7E Ch. 9 - Prob. 9.8E Ch. 9 - Prob. 9.9E Ch. 9 - Write equations to represent the Brnsted acid...

Solution Summary: The author explains the value of K_a for the given weak acid based on the equilibrium concentrations and pH values.

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