Chapter 17, Problem 17.3QP

Interpretation Introduction

Interpretation:

From the given buffer systems the one with better buffer capacity should be identified.

Concept Introduction:

Buffer:

A buffer is a chemical solution that contains a weak acid/base mixed with its conjugate base/acid (as in the form of salts). It can resist $\text{pH}$ change when a small amount of a strong acid/base is added to it. The acidic buffer solution is made up of less than $\text{pH 7}$ and the alkali buffer solution is made up of more than $\text{pH 7}$.

Henderson-Hasselbalch equation is a mathematical expression which can be used to calculate the $\text{pH}$ of buffer solutions.

  ${\text{pH = pK}}_{\text{a}}\text{+ log}\frac{{\text{[A}}^{-}\text{]}}{\text{[HA]}}$

Here,

The power of ${\text{H}}^{\text{+}}$ in a buffer solution is $\text{pH}$.

The power of acid dissociation constant of a weak acid is ${\text{pK}}_{\text{a}}$.

The concentration of a weak monoprotic acid is $\text{[HA]}$.

The concentration of its conjugate base is ${\text{[A}}^{\text{-}}\text{]}$.