Chapter 16, Problem 16.76QP

Interpretation Introduction

Interpretation:

From the relationship ${\text{K}}_{\text{w}}{\text{=K}}_{\text{a}}\times {\text{K}}_{\text{b}}$ , what can you deduce about the relative strengths of a weak acid and its conjugate base has to be explained.

Concept Information:

When a Bronsted acid donates a proton, what remains of the acid is known as a conjugate base; when a Bronsted base accepts a proton, the newly formed protonated species is known as a conjugate acid.  This can be given by the below equation as shown in Figure 1.

Figure 1

The relationship between the acid ionization constant and base ionization constant is:

${\text{K}}_{\text{w}}{\text{=K}}_{\text{a}}\times {\text{K}}_{\text{b}}$

Where,

${\text{K}}_{\text{w}}$ is autoionization of water. ( ${\text{K}}_{\text{w}}{\text{=[H}}^{\text{+}}{\text{][OH}}^{\text{-}}\text{]}$)