   # If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? (a) 100. mL (b) 50. mL (c) 36 mL (d) 18 mL ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 17.2, Problem 2RC
Textbook Problem
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## If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? (a) 100. mL (b) 50. mL (c) 36 mL (d) 18 mL

Interpretation Introduction

Interpretation:

The value of pH for the solution containing 100mL of acetic acid and 0.10M of sodium acetate were dissolved in 0.10M of water is to be calculated by using Henderson-Hasselbalch equation

Concept introduction:

The Henderson-Hasselbalch equation relates pH of a buffer with pKa of acid, concentration of conjugate base and concentration of acid. The expression is written as,

pH=pKa+log[conjugatebase][acid] (1)

This equation shows that pH of buffer solution is controlled by two major factors. First, Strength of the acid which can be expressed on terms of pKa and second, the relative concentration of acid and its conjugate base at equilibrium.

### Explanation of Solution

The pH value calculation for the given solution of accetic acid/sodium accetate is given below.

The acid dissociation constant expression is given as;

Given the data Volume ofCH3COOHsoultion=100mL(or)=0.100LMolarofCH3COOHsoultion=0.10nCOOH=0.01molpH=4AceticacidpKavalues=4.74LetusconsidertheHenderson-Hasselbalch equationpH=pKa+log[CH3COONa+](eq)[CH3COOH](eq)4=4.74+log[CH3COONa+](eq)[CH3COOH](eq)44

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