Chapter 15.13, Problem 15.29P

(a)

Interpretation Introduction

Interpretation:

The possibility of precipitate formation should be explained, when mixing of $\text{3}\text{.0}\times {\text{10}}^{\text{-3}}{\text{M BaCl}}_{\text{2}}\text{ with 2}\text{.0}\times {\text{10}}^{\text{-3}}{\text{ M Na}}_{\text{2}}{\text{CO}}_{\text{3}}$.

Concept Introduction:

Solubility product constant:

The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.

The equilibrium constant of more soluble ionic compound is given by ${\text{K}}_{\text{sp}}$ and it is expressed by product of multiplication of number of each ion present in the compound rise to the power of number respective ion present in the compound to give a maximum solubility of the compound.

$\begin{array}{l}{\text{M}}_{\text{m}}{\text{X}}_{\text{x}}{}_{\text{(s)}}\stackrel{}{\rightleftharpoons }{\text{ mM}}^{\text{n+}}{}_{\text{(aq)}}{\text{ + xX}}^{\text{y-}}{}_{\text{(aq)}}\\ \\ {\text{K}}_{\text{sp}}{\text{ = [M}}^{\text{n+}}{\text{]}}^{\text{m}}{\text{×[X}}^{\text{y-}}{\text{]}}^{\text{x}}\end{array}$

Ion product:

The multiplication of concentrations power of number of ion each ions in the formula to give the ion product.

$\begin{array}{l}{\text{M}}_{\text{m}}{\text{X}}_{\text{x}}{}_{\text{(s)}}\stackrel{}{\rightleftharpoons }{\text{ mM}}^{\text{n+}}{}_{\text{(aq)}}{\text{ + xX}}^{\text{y-}}{}_{\text{(aq)}}\\ \\ {\text{IP = [M}}^{\text{n+}}{\text{]}}_{\text{t}}{}^{\text{m}}{\text{×[X}}^{\text{y-}}{\text{]}}^{\text{x}}\end{array}$

Precipitation occurs that solution is supersaturated if $\text{IP}\text{>}{\text{K}}_{\text{sp}}$

Precipitation will not occurs that solution is saturated and in equilibrium if $\text{IP}\text{>}{\text{K}}_{\text{sp}}$

Precipitation will not occurs that solution is unsaturated if $\text{IP}<{\text{K}}_{\text{sp}}$

(b)

Interpretation Introduction

Interpretation:

The possibility of precipitate formation should be explained, when mixing of $\text{1}\text{.0}\times {\text{10}}^{\text{-5}}{\text{M Ba(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{ with 4}\text{.0}\times {\text{10}}^{\text{-5}}\text{ M}{\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$.

Concept Introduction:

Solubility product constant:

The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.

The equilibrium constant of more soluble ionic compound is given by ${\text{K}}_{\text{sp}}$ and it is expressed by product of multiplication of number of each ion present in the compound rise to the power of number respective ion present in the compound to give a maximum solubility of the compound.

$\begin{array}{l}{\text{M}}_{\text{m}}{\text{X}}_{\text{x}}{}_{\text{(s)}}\stackrel{}{\rightleftharpoons }{\text{ mM}}^{\text{n+}}{}_{\text{(aq)}}{\text{ + xX}}^{\text{y-}}{}_{\text{(aq)}}\\ \\ {\text{K}}_{\text{sp}}{\text{ = [M}}^{\text{n+}}{\text{]}}^{\text{m}}{\text{×[X}}^{\text{y-}}{\text{]}}^{\text{x}}\end{array}$

Ion product:

The multiplication of concentrations power of number of ion each ions in the formula to give the ion product.

$\begin{array}{l}{\text{M}}_{\text{m}}{\text{X}}_{\text{x}}{}_{\text{(s)}}\stackrel{}{\rightleftharpoons }{\text{ mM}}^{\text{n+}}{}_{\text{(aq)}}{\text{ + xX}}^{\text{y-}}{}_{\text{(aq)}}\\ \\ {\text{IP = [M}}^{\text{n+}}{\text{]}}_{\text{t}}{}^{\text{m}}{\text{×[X}}^{\text{y-}}{\text{]}}^{\text{x}}\end{array}$

Precipitation occurs that solution is supersaturated if $\text{IP}\text{>}{\text{K}}_{\text{sp}}$

Precipitation will not occurs that solution is saturated and in equilibrium if $\text{IP}\text{>}{\text{K}}_{\text{sp}}$

Precipitation will not occurs that solution is unsaturated if $\text{IP}<{\text{K}}_{\text{sp}}$