Chapter 6, Problem 6C.1BST

Interpretation Introduction

Interpretation:

Chemical formula for the conjugate base of ${\text{HIO}}_{\text{3}}$ has to be written and also the value of $\text{p}{K}_b$ has to be calculated.

Concept Introduction:

Generally acid donates proton to form conjugate base.  As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid.  Base accepts protons to form conjugate acid.  As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

Sum of acidity constant and basicity constant is equal to $14.00$.  $K_a$ is the acidity constant of acid while $K_b$ is the basicity constant of base.  The equation can be given as shown below;

    $\text{p}{K}_a+\text{p}{K}_b=\text{p}{K}_w$