Chapter 14.7, Problem 14.20E

Interpretation Introduction

Interpretation:

$K_b$ value should be calculated for the phenolate ion. Base having strength closest to the phenolate ion has to be identified and explained.

Concept Introduction:

The relation between acidic and basic constants $K_{a}and{K}_b$ with $K_w$ (equilibrium constant for water) is,

    $\begin{array}{l}{K}_a=\frac{1}{K_b}\times K_w\\ \\ K_w=K_b\times K_a\end{array}$

$K_b$ value of the phenolate ion is $7.7\times {10}^{-5}$

Carbonate ion has strength closest to the phenolate ion because the $K_b$ value of carbonate is nearest to the $K_b$ value of phenolate ion.