Chapter 14, Problem 14.45P

Interpretation Introduction

Interpretation:

${\text{K}}_{\text{sp}}$ value for the reaction has to be calculated.

Base dissociation constant:

The value of ${\text{E}}^{\text{o}}$ can be calculated as,

${\text{E}}^{\text{o}}\text{=}\frac{{\text{-ΔG}}^{\text{o}}}{\text{nF}}$

Where

${\text{E}}^{\text{o}}$ = The standard reduction potential

n = number of electrons

The equilibrium constant for the reaction can be calculated as,

Finding $\text{K}$ from ${\text{E}}^{\text{o}}$

$\text{K}\text{=}\frac{{\text{10}}^{{\text{nE}}^{\text{o}}}}{\text{0}\text{.05916}}\text{at}{\text{25}}^{\text{o}}\text{C}$

Where $\text{K}$ is equilibrium constant

Solubility product: ${\text{K}}_{\text{sp}}$ It is defined as the product formed from mathematical product of its concentration of dissolved ion raised up to the power of their stoichiometric coefficient.

$\begin{array}{l}{\text{M}}_{\text{y}}{\text{X}}_{\text{z(s)}}\underset{}{\rightleftharpoons }{\text{yM}}_{{}_{\text{(aq)}}}^{\text{Z+}}\text{+}{\text{zX}}_{\text{(aq)}}^{\text{y-}}\\ {\text{K}}_{\text{sp}}\text{=}{\left[{\text{M}}_{{}_{}}^{\text{Z+}}\right]}^{\text{y}}{\left[{\text{X}}_{{}_{}}^{\text{y-}}\right]}^{\text{z}}\end{array}$