   # Using the K a values in Table 13-2, calculate the percent dissociation in a 0.20- M solution of each of the following acids. a. nitric acid (HNO 3 ) b. nitrous acid (HNO 2 ) c. phenol (HOC 6 H 5 ) d. How is percent dissociation of an acid related to the K a value for the acid (assuming equal initial concentrations of acids)? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 74E
Textbook Problem
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## Using the Ka values in Table 13-2, calculate the percent dissociation in a 0.20-M solution of each of the following acids.a. nitric acid (HNO3)b. nitrous acid (HNO2)c. phenol (HOC6H5)d. How is percent dissociation of an acid related to the Ka value for the acid (assuming equal initial concentrations of acids)?

(a)

Interpretation Introduction

Interpretation: The percent dissociation of the acid in each of the given solutions is to be calculated.

Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

The percent dissociation of an acid is calculated by the formula,

Percentdissociation=Equilibriumconcentrationof[H+]Initialconcentrationoftheacid×100

To determine: The percent dissociation for a 0.20M solution of nitric acid (HNO3) .

### Explanation of Solution

Explanation

HNO3 is a strong acid. A strong acid completely dissociates in water.

Therefore, the [H+] is equal to the initial concentration of the acid.

Therefore, the [H+] is 0.20M_ .

The equilibrium concentration of [H+] is 0.20M .

The initial concentration of HNO3 is 0.20M

(b)

Interpretation Introduction

Interpretation: The percent dissociation of the acid in each of the given solutions is to be calculated.

Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

The percent dissociation of an acid is calculated by the formula,

Percentdissociation=Equilibriumconcentrationof[H+]Initialconcentrationoftheacid×100

To determine: The percent dissociation for a 0.20M solution of nitrous acid (HNO2) .

(c)

Interpretation Introduction

Interpretation: The percent dissociation of the acid in each of the given solutions is to be calculated.

Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

The percent dissociation of an acid is calculated by the formula,

Percentdissociation=Equilibriumconcentrationof[H+]Initialconcentrationoftheacid×100

To determine: The percent dissociation for a 0.20M solution of phenol (C6H5OH) .

(d)

Interpretation Introduction

Interpretation: The percent dissociation of the acid in each of the given solutions is to be calculated.

Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

The percent dissociation of an acid is calculated by the formula,

Percentdissociation=Equilibriumconcentrationof[H+]Initialconcentrationoftheacid×100

To determine: The relation of percent dissociation of an acid and the Ka value for the acid.

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