   # Calculate the pH of a solution that is 1.00 M HNO 2 and 1.00 M NaNO 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 14, Problem 31E
Textbook Problem
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## Calculate the pH of a solution that is 1.00 M HNO2 and 1.00 M NaNO2.

Interpretation Introduction

Interpretation:

The concentration of HNO2 and NaNO2 is given. The pH value of a solution of HNO2 and NaNO2 is to be calculated.

Concept introduction:

A solution that contains the mixture of a weak acid and its conjugate base is known as buffer solution.

The pH value is the measure of H+ ions. The pH is calculated by the formula,

pH=log10[H+]

### Explanation of Solution

Explanation

Given

The concentration of HNO2 and NaNO2 is 1.00M .

The value of Ka of HNO2 is 4.0×104 .

The major species in the solution are HNO2,Na+,NO2 and H2O .

The dominant equilibrium dissociation reaction is,

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

The equilibrium ratio for the given reaction is,

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

Substitute the given value of Ka in the above equation.

Ka=[NO2][H+][HNO2]4.0×104=[NO2][H+][HNO2] (1)

The concentrations are as follows,

Initialconcentration(mol/L)Equilibriumconcentration(mol/L)[HNO2]0=1.00[HNO2]0=1.00x[NO2]0=1.00dissociatestoreachequilibriumxmol/LofHNO2[NO2]0=1.00+x[H+]00[H+]0=x

Make the ICE table for the dissociation reaction of HNO2 .

HNO2(aq)H+(aq)NO2(aq)Initial(M):1

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