Chapter 15, Problem 15.95SP

(a)

Interpretation Introduction

Interpretation:

The ${\text{K}}_{\text{sp}}$ Value for $\text{1}\text{.0 }\times {\text{10}}^{\text{-6}}\text{ M}$ ${\text{CdCO}}_{\text{3}}$ solution should be calculated.

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 number of each ion present in the compound raised to the power of coefficients of respective ion present in the compound to give a maximum solubility of the compound.

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

Molar solubility:

Molar solubility (X) can be given as solubility in moles per litre.

$\text{X =}\frac{\text{Solubility}\text{in}\text{gram}}{\text{1L}}\text{×}\frac{\text{1}\text{mol}}{\text{Molarmass}\text{(g)}}$

(b)

Interpretation Introduction

Interpretation:

The ${\text{K}}_{\text{sp}}$ Value for $\text{1}\text{.06}\times {\text{10}}^{\text{-2}}\text{ M}$${\text{Ca(OH)}}_{\text{2}}$ solution should be calculated.

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 number of each ion present in the compound raised to the power of coefficients of respective ion present in the compound to give a maximum solubility of the compound.

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

Molar solubility:

Molar solubility (X) can be given as solubility in moles per litre.

$\text{X =}\frac{\text{Solubility}\text{in}\text{gram}}{\text{1L}}\text{×}\frac{\text{1}\text{mol}}{\text{Molarmass}\text{(g)}}$

(c)

Interpretation Introduction

Interpretation:

The ${\text{K}}_{\text{sp}}$ Value for $\text{4}\text{.34 g/L}$${\text{PbBr}}_{\text{2}}$ solution should be calculated.

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 number of each ion present in the compound raised to the power of coefficients of respective ion present in the compound to give a maximum solubility of the compound.

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

Molar solubility:

Molar solubility (X) can be given as solubility in moles per litre.

$\text{X =}\frac{\text{Solubility}\text{in}\text{gram}}{\text{1L}}\text{×}\frac{\text{1}\text{mol}}{\text{Molarmass}\text{(g)}}$

(d)

Interpretation Introduction

Interpretation:

The ${\text{K}}_{\text{sp}}$ Value for $\text{2}\text{.8 }\times {\text{10}}^{\text{-3}}\text{g/L}$ ${\text{BaCrO}}_{\text{4}}$ solution should be calculated.

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 number of each ion present in the compound raised to the power of coefficients of respective ion present in the compound to give a maximum solubility of the compound.

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

Molar solubility:

Molar solubility (X) can be given as solubility in moles per litre.

$\text{X =}\frac{\text{Solubility}\text{in}\text{gram}}{\text{1L}}\text{×}\frac{\text{1}\text{mol}}{\text{Molarmass}\text{(g)}}$