Chapter 16.10, Problem 19PPC

Interpretation Introduction

Interpretation:

Among the given graphs, the graph that best represents the relationship between pH of a acidic salt solution and the ${\text{K}}_{\text{b}}$  of the base from which the salt is derived has to be explained

Concept Information:

Base  ionization constant $K_b$

The equilibrium expression for the ionization of weak base $\text{B}$ will be,

${\text{B}}_{(aq)}+{\text{H}}_{\text{2}}{\text{O}}_{(l)}\rightleftarrows {\text{HB}}^{\text{+}}{}_{(aq)}+{\text{OH}}^{\text{-}}{}_{(aq)}$

${\text{K}}_b=\frac{[{\text{HB}}^{\text{+}}][{\text{OH}}^{\text{-}}]}{[\text{B}]}$

Where $K_b$ is base ionization constant, $[{\text{OH}}^{-}\text{]}$ is concentration of hydroxide ion, $[{\text{HB}}^{\text{+}}\text{]}$ is concentration of conjugate acid, $[\text{B]}$ is concentration of the base

pH and pOH:

$\begin{array}{l}\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}\\ \text{pOH}\text{=}{\text{-log[OH}}^{-}\text{]}\end{array}$

The pOH scale is the reverse of pH scale

To Explain: The diagram that best represents the relationship between pH of a acidic salt solution and $K_b$ of the base