   # What are the major species present in 0.250 M solutions of each of the following acids? Calculate the pH of each of these solutions. a. HNO 2 b. CH 3 CO 2 H(HC 2 H 3 O 2 ) ### 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 63E
Textbook Problem
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## What are the major species present in 0.250 M solutions of each of the following acids? Calculate the pH of each of these solutions.a. HNO2b. CH3CO2H(HC2H3O2)

(a)

Interpretation Introduction

Interpretation: The major species present in 0.250M solutions of the given acids and the pH value of these solutions is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

### Explanation of Solution

Explanation

To determine: The major species present in 0.250M solution of HNO2 and the pH of this solution.

The major species present in 0.250M solution of HNO2 are HNO2 and H2O .

HNO2 is a weak acid. Hence, it does not completely dissociate in water.

The major species present in the given solution of HNO2 are HNO2 and H2O .

The equilibrium constant expression for the stated dissociation reaction is,

Ka=[H+][NO2][HNO2]

HNO2 is a comparatively stronger acid than H2O .

The dominant equilibrium reaction for the given case is,

HNO2(aq)H+(aq)+NO2(aq)

At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

Where,

• Ka is the acid dissociation constant.

The equilibrium constant expression for the given reaction is,

Ka=[H+][NO2][HNO2] (1)

The [H+] is 1×10-2M_ .

The change in concentration of HNO2 is assumed to be x .

The ICE table for the stated reaction is,

HNO2(aq)H+(aq)+NO2(aq)Inititialconcentration0.25000Changex+x+xEquilibriumconcentration0.250xxx

The equilibrium concentration of [HNO2] is (0.250x)M .

The equilibrium concentration of [H+] is xM

(b)

Interpretation Introduction

Interpretation: The major species present in 0.250M solutions of the given acids and the pH value of these solutions is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

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