Chapter 5, Problem 5.50P

Interpretation Introduction

Interpretation:

The mercury $\left(I\right)$ iodide salt solubility in water has to be calculated.

Concept Introduction:

Solubility: It defines the maximum quantity of the solute that can be dissolved in the given volume of the solvent.

Dissociation: The separation of the ionic compound into its constituent anion and cation is called as dissociation; generally, dissociation takes place in an aqueous condition.

The solubility product (${\text{K}}_{\text{sp}}$): Solubility product is defined as the concentration of the dissolved ion’s rise to the power of its stoichiometric coefficients in an equilibrium condition.

Ionic product ($\text{Q}$): It is the solubility product of a concentration of ions in a solution of dissolving ionic solid.

Consider a general reaction:

${\text{M}}_{\text{n}}{\text{X}}_{\text{m}}\text{(s)}\stackrel{}{\rightleftharpoons }\text{n}{\text{M}}^{\text{m+}}\text{(aq)+m}{\text{X}}^{\text{n-}}\text{(aq)}$

The solubility product is expressed as follows:

${\text{K}}_{\text{sp}}\text{=}{\left[{\text{M}}^{\text{m+}}\right]}^{\text{n}}{\left[{\text{X}}^{\text{n-}}\right]}^{\text{m}}$

Here,

Solubility product = ${\text{K}}_{\text{sp}}$,

$\begin{array}{l}\text{Molar solubility of M ion =}\left[{\text{M}}^{\text{m+}}\right],\\ \\ \text{Molar solubility of X ion =}\left[{\text{X}}^{\text{n-}}\right],\end{array}$

$\text{n}\text{and}\text{m}\text{are}\text{powers}\text{of ions}$.

Free energy change${\text{ΔG}}^0$: change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant $\text{K}$

  ${\text{ΔG}}^{\text{0}}\text{=}-\text{RT}\left(\text{ln}\text{K}\right)\text{=}{\text{ΔH}}^{\text{0}}-{\text{TΔS}}^{\text{0}}$

  Where $\text{T}$ is the temperature