   # 8-66 Calculate the pH of an aqueous solution containing the following: (a) 0.80 M lactic acid and 0.40 M lactate ion (b) 0.30 M and 1.50 M NH 4 + ### Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759

#### Solutions

Chapter
Section ### Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759
Chapter 8, Problem 8.66P
Textbook Problem
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## 8-66 Calculate the pH of an aqueous solution containing the following: (a) 0.80 M lactic acid and 0.40 M lactate ion (b) 0.30 M and 1.50 M NH4+

Interpretation Introduction

(a)

Interpretation:

The pH of an aqueous solution containing 0.80 m lactic acid and 0.40 m lactate ion should be calculated.

Concept Introduction:

The pH of buffer can be calculated using the Henderson-Hasselbalch equation as follows:

pH=pKa+log[A][HA]

Here, pH is negative log of hydrogen ion, pKa is negative log of acid dissociation constant, [A] is concentration of conjugate base and [HA] is concentration of acid.

### Explanation of Solution

Given Information:

The concentration of lactic acid lactate ion is 0.80 m and 0.40 m respectively.

Calculation:

For the given buffer, the Henderson-Hasselbalch equation is as follows:

pH=pKa+log[lactate ion][lactic acid]

The pKa value of lactic acid is 3

Interpretation Introduction

(b)

Interpretation:

The pH of an aqueous solution containing 0.30 m NH3 and 1.50 m NH4+ should be calculated.

Concept Introduction:

The pH of buffer can be calculated using the Henderson-Hasselbalch equation as follows:

pH=pKa+log[A][HA]

Here, pH is negative log of hydrogen ion, pKa is negative log of acid dissociation constant, [A] is concentration of conjugate base and [HA] is concentration of acid.

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