Chapter 9, Problem 9.115E

Interpretation Introduction

Interpretation:

The pH of the given buffer is to be calculated.

Concept Introduction:

The buffer is a solution that resists any change in pH on addition of little amounts of ${\text{H}}^{+}$ and ${\text{OH}}^{-}$. An acidic buffer is made up of a weak acid and its salt. A basic buffer is made up of a weak base and its salt. The pH of the acidic buffer is given as,

$\text{pH}={\text{pK}}_{\text{a}}+\log \frac{\left[{\text{B}}^{-}\right]}{\left[\text{HB}\right]}$

Where,

• $\left[{\text{B}}^{-}\right]$ represents the concentration of ${\text{B}}^{-}$ the ion.

• $\left[\text{HB}\right]$ represents the concentration of $\text{HB}$ acid.

• ${\text{pK}}_{\text{a}}$ represents the negative logarithm of the acid dissociation constant.