Chapter 15, Problem 15.104SP

(a)

Interpretation Introduction

Interpretation:

The change in solubility of ${\text{Zn(OH)}}_2$ by the addition of $\text{HCl}$ should be explained. Also a balanced net ionic equation for the dissolution reaction has to be written.

Le Chatelier's principle:

Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it reset to counteract the effect of disturbance.

The concentrations of reactant and product are equal in equilibrium chemical reaction.  The effect of concentration, temperature and external pressure makes a change in equilibrium.  To counteract this, the chemical reaction is shifted to reactant or product side to attain equilibrium.

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

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

Molar solubility:

Molar solubility (S) is given as solubility in moles per litre.

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

(b)

Interpretation Introduction

Interpretation:

The change in solubility of ${\text{Zn(OH)}}_2$ by the addition of $\text{KOH}$ should be explained. Also a balanced net ionic equation for the dissolution reaction has to be written.

Concept Introduction:

Le Chatelier's principle:

Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it reset to counteract the effect of disturbance.

The concentrations of reactant and product are equal in equilibrium chemical reaction.  The effect of concentration, temperature and external pressure makes a change in equilibrium.  To counteract this, the chemical reaction is shifted to reactant or product side to attain equilibrium.

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

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

Molar solubility:

Molar solubility (S) is given as solubility in moles per litre.

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

(c)

Interpretation Introduction

Interpretation:

The change in solubility of ${\text{Zn(OH)}}_2$ by the addition of $\text{NaCN}$ should be explained. Also a balanced net ionic equation for the dissolution reaction has to be written.

Concept Introduction:

Le Chatelier's principle:

Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it reset to counteract the effect of disturbance.

The concentrations of reactant and product are equal in equilibrium chemical reaction.  The effect of concentration, temperature and external pressure makes a change in equilibrium.  To counteract this, the chemical reaction is shifted to reactant or product side to attain equilibrium.

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

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

Molar solubility:

Molar solubility (S) is given as solubility in moles per litre.

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