   # Calculate the volume of 1.50 × 10 −2 M NaOH that must be added to 500.0 mL of 0.200 M HCl to give a solution that has pH = 2.15. ### 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 91AE
Textbook Problem
1 views

## Calculate the volume of 1.50 × 10−2 M NaOH that must be added to 500.0 mL of 0.200 M HCl to give a solution that has pH = 2.15.

Interpretation Introduction

Interpretation:

The volume of 1.50×102M NaOH that must be added to 500.0mL of 0.200M HCl to give a solution that has a pH of 2.15 is to be calculated.

Concept introduction:

The pH of a solution is calculated by the formula,

pH=log[H+]

According to the dilution law, N1V1=N2V2

### Explanation of Solution

Explanation

To find the [H+]

The volume of 1.50×102M NaOH required is assumed to be VmL .

The given volume of HCl is 500.0mL .

The given pH value is 2.15 .

The pH of a solution is calculated by the formula,

pH=log[H+]

Rearrange the above expression to calculate the value of [H+] .

[H+]=10pH

Substitute the value of pH in the above expression.

[H+]=102.15=7.08×10-3M_

To find the required volume of 1.50×102M NaOH

On the basis of the dilution law,

N1V1=N2V2

Where,

• N1 is the normality of NaOH .
• N2 is the normality of HCl .
• V1 is the volume of NaOH .
• V2 is the volume of HCl .

As NaOH is a monoacidic base, (1×Molarity)=Normality

As HCl is a monobasic acid, (1×Molarity)=Normality

Therefore,

The normality of NaOH (N1)=1

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