   # Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.200 M acetic acid to form a pH = 5.00 buffer solution. ### 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 41E
Textbook Problem
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## Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.200 M acetic acid to form a pH = 5.00 buffer solution.

Interpretation Introduction

Interpretation:

The concentration and volume of acetic acid and the required pH of solution is given. The mass of sodium acetate that must be added to make a buffer solution with acetic acid is to be calculated.

Concept introduction:

The pH value is the measure of H+ ions. The relation between pH and pKa is given by the Henderson-Hassel Bach equation. According to this equation,

pH=pKa+log[Base][Acid]

### Explanation of Solution

Explanation

To find the concentration of sodium acetate

The concentration of acetic acid is 0.200M .

The value of Ka for acetic acid is 1.8×105 .

The pH value of acetic acid is 5.00 .

The pH is calculated using the Henderson-Hassel Bach equation,

pH=pKa+log[CH3COONa][CH3COOH]

Where,

• pH is the measure of H+ ions.
• pKa is the measure of acidic strength.
• [CH3COONa] is the concentration of CH3COONa .
• [CH3COOH] is the concentration of CH3COOH .

The formula of pKa is,

pKa=logKa

Where,

• Ka is acid equilibrium constant.

Substitute the value of pKa in the Henderson-Hassel Bach equation.

pH=logKa+log[CH3COONa][CH3COOH]

Substitute the given value of Ka , [CH3COOH] and pH in the above equation.

pH=logKa+log[CH3COONa][CH3COOH]5=log(1.8×105)+log[CH3COONa]0.2005=4.74+log[CH3COONa]0.200

Simplify the above equation

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