Biochemistry: Concepts and Connections (2nd Edition)
Biochemistry: Concepts and Connections (2nd Edition)
2nd Edition
ISBN: 9780134641621
Author: Dean R. Appling, Spencer J. Anthony-Cahill, Christopher K. Mathews
Publisher: PEARSON
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Chapter 2, Problem 5P
Interpretation Introduction

(a) Interpretation:

The pH of a 1 M NH4Cl solution should be calculated.

Concept Introduction:

For a weak acid or a weak base, the dissociation reaction is in equilibrium and the equilibrium constant is known as acid or base dissociation constant. For such a solution, concentration of each species is calculated using ICE table.

The pH of solution is calculated as follows:

    pH=log[H+]

Here, [H+] is concentration of hydrogen ions in the solution.

Interpretation Introduction

(b) Interpretation:

The pH of solution resulting from addition of 10 mL of a 1 M NaOH to 40 mL of 1 M NH4Cl.

Concept Introduction:

For a buffer solution, pH is calculated using Henderson-Hasselbalch equation as follows:

    pH=pKa+log[Conjugate base][acid]

Here, pH is log[H+] of solution and pKa is -log(Ka) of weak acid.

Interpretation Introduction

(c) Interpretation:

The pH of the solution that results from the addition of 30 mL of 1 M NaOH to 40 mL of 1 M NH4Cl.

Concept Introduction:

For a buffer solution, pH is calculated using Henderson-Hasselbalch equation as follows:

    pH=pKa+log[Conjugate base][acid]

Here, pH is log[H+] of solution and pKa is -log(Ka) of weak acid.

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