Chapter 9, Problem 9.15P

Interpretation Introduction

Interpretation:

The $\text{pH}$ of $\text{0}\text{.010}\text{M}$ and fraction of dissociation of Chromium in $\text{Cr}{\left(\text{OH}\right)}^{\text{2+}}$ has to be calculated.

Concept Introduction:

Consider a weak-acid equilibrium reaction,

$\text{HA}\stackrel{{\text{K}}_{\text{a}}}{\rightleftharpoons }{\text{H}}^{\text{+}}{\text{+A}}^{\text{-}}$

The acid dissociation constant ${\text{K}}_{\text{a}}$ can be given as,

${\text{K}}_{\text{a}}\text{=}\frac{\left[{\text{H}}^{\text{+}}\right]\left[{\text{A}}^{\text{-}}\right]}{\left[\text{HA}\right]}$

A weak acid is one that doesn’t undergo completion.

The $\text{pH}$ of solution can be calculated as,

$\begin{array}{l}{\text{pH=-logA}}_{{\text{H}}^{\text{+}}}\\ \\ \text{pH=-log}{\left[{\text{H}}^{\text{+}}\right]}_{{\text{γH}}^{\text{+}}}\end{array}$

With the above equation, the negative logarithm of activity of Hydrogen ion can be measured.

Fraction of dissociation:

The fraction of acid that represents ${\text{A}}^{\text{-}}$ is called as fraction of dissociation. It is represented by the symbol $\text{α}$.

Generally, fraction of dissociation of weak acid is calculated as,

$\begin{array}{l}\text{α=}\frac{\left[{\text{A}}^{\text{-}}\right]}{\left[{\text{A}}^{\text{-}}\right]\text{+}\left[\text{HA}\right]}\\ \\ \text{α=}\frac{\text{x}}{\text{x+}\left(\text{F-x}\right)}\\ \\ \text{α=}\frac{\text{x}}{\text{F}}\end{array}$