(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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A small artisanal cheesemaker is testing the acidity of their milk before it coagulates. During fermentation, bacteria produce lactic acid (K₁ = 1.4 x 104), a weak acid that helps to curdle the milk and develop flavor. The cheesemaker has measured that the developing mixture contains lactic acid at an initial concentration of 0.025 M. Your task is to calculate the pH of this mixture and determine whether it meets the required acidity for proper cheese development. To achieve the best flavor, texture and reduce/control microbial growth, the pH range needs to be between pH 4.6 and 5.0. Assumptions: Lactic acid is a monoprotic acid H H :0:0: H-C-C H :0: O-H Figure 1: Lewis Structure for Lactic Acid For simplicity, you can use the generic formula HA to represent the acid You can assume lactic acid dissociation is in water as milk is mostly water. Temperature is 25°C 1. Write the K, expression for the dissociation of lactic acid in the space provided. Do not forget to include state symbols.…

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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