Chapter 10, Problem 10.74AP

Interpretation Introduction

Interpretation:

The components of buffer systems and the working of buffer system should be discussed.

Concept Introduction:

$\text{pH}$: $\text{pH}$ is the logarithm of the reciprocal of the concentration of ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ in a solution. The pH of a solution is a measure of concentration of hydrogen ion in a solution. Lower $\text{pH}$ due to more hydrogen ions and higher $\text{pH}$ due to less concentration of hydrogen ions.

$\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation.

Buffer solutions: Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base. Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

$K_a$: Acid dissociation constant ${\text{K}}_{\text{a}}$ represents how strong the acid is in a solution.

$p{K}_a=-\log \left[K_a\right]$ It is negative logarithm of acid dissociation constant ${\text{K}}_{\text{a}}$.