Chapter 2, Problem 18P

Summary Introduction

To determine: The $\text{pH}$ of a solution containing $0.12\text{ mol}/\text{L}$ of ${\text{NH}}_{\text{4}}\text{Cl}$ and $0.03\text{ mol}/\text{L}$ of $\text{NaOH}$( ${\text{pK}}_{\text{a}}$ of ${\text{NH}}_4^{+}/{\text{NH}}_{\text{3}}$ is $9.25$) is to be determined.

Introduction:

The Henderson-Hasselbalch equation depicts the measurement of acidity as $\text{pH}$ (potential of hydrogen) in biochemical reactions. The isoelectric point and $\text{pH}$ of buffers are calculated by this reaction. The $\text{pH}$ is used to calculate the ${\text{pK}}_{\text{a}}$ of molecules. The “ionized and unionized” concentrations of chemicals are estimated with the help of this equation. The ${\text{pK}}_{\text{a}}$ is used to calculate the $\text{pH}$ of molecules.