Chapter 11, Problem 46A

(a)

Interpretation Introduction

Interpretation:

To balance the net ionic equation.

Concept Introduction:

An ionic equation is a chemical equation in which ions are represented in an aqueous solution. If all the ions are represented then, it is known as a complete ionic equation but when spectator ions are removed then, it is known as a net ionic equation.

Answer to Problem 46A

The balanced net ionic equation is: ${\text{H}}^{+}\text{(}aq{\text{) + OH}}^{-}(aq)\to {\text{ H}}_{2}O(l)$ .

Explanation of Solution

To balance the ionic equation, some steps need to be followed and those are:

Step $1$ : Write the reactants.

Step $2$ : Identify the possible pairing of anions and cations to give insoluble products.

Step $3$: Remove the spectator ions.

The ionic equation given is:

  $\text{HCl(}aq{\text{) + Ca(OH)}}_2(aq)\to$

Step $1$ : ${\text{H}}^{+}\text{(}aq{\text{) +Cl}}^{-}\text{(}aq{\text{) + Ca}}^{2+}{\text{(aq) + 2OH}}^{-}(aq)\to$

Step $2$ :

  ${\text{2H}}^{+}\text{(}aq{\text{) +2Cl}}^{-}\text{(}aq{\text{) + Ca}}^{2+}{\text{(aq) + 2OH}}^{-}(aq)\to {\text{ Ca}}^{2+}\text{(}aq{\text{) +2Cl}}^{-}\text{(}aq{\text{)+ 2H}}^{+}(aq)+2O{H}^{-}(aq)$

Step $3$ : ${\text{H}}^{+}\text{(}aq{\text{) + OH}}^{-}(aq)\to {\text{ H}}_{2}O(l)$

(b)

Interpretation Introduction

Interpretation:

To balance the net ionic equation.

Concept Introduction:

An ionic equation is a chemical equation in which ions are represented in an aqueous solution. If all the ions are represented then, it is known as a complete ionic equation but when spectator ions are removed then, it is known as the net ionic equation.

Answer to Problem 46A

The balanced net ionic equation is: ${\text{Ag}}^{+}\text{(}aq{\text{) + Cl}}^{-}(aq)\to \text{ AgCl(}s\text{)}$ .

Explanation of Solution

To balance the ionic equation, some steps need to be followed and those are:

Step $1$ : Write the reactants.

Step $2$ : Identify the possible pairing of anions and cations to give insoluble products.

Step $3$: Remove the spectator ions.

The ionic equation given is:

  ${\text{3AgNO}}_3\text{(}aq{\text{) + AlCl}}_3(aq)$ $\to$

Step $1$ : ${\text{3Ag}}^{+}\text{(}aq{\text{) +NO}}_3{}^{-}\text{(}aq{\text{) + Al}}^{3+}{\text{(aq) + 3Cl}}^{-}(aq)\to$

Step $2$ :

  ${\text{3Ag}}^{+}\text{(}aq{\text{) +3NO}}_3{}^{-}\text{(}aq{\text{) + Al}}^{3+}{\text{(aq) + 3Cl}}^{-}(aq)\to {\text{ 3Ag}}^{+}\text{(}aq{\text{) +3Cl}}^{-}\text{(}aq{\text{)+ Al}}^{3+}(aq)+3{\text{NO}}_3{}^{-}(aq)$

Step $3$ : ${\text{Ag}}^{+}\text{(}aq{\text{) + Cl}}^{-}(aq)\to \text{ AgCl(}s\text{)}$