Chapter 4, Problem 4.22QE

(a)

Interpretation Introduction

Interpretation:

The net ionic equation has to be written if reaction occurs when solutions of potassium bromide and silver nitrate are mixed.

Explanation of Solution

Given: solutions of potassium bromide $\text{KBr}$ and silver nitrate ${\text{AgNO}}_{\text{3}}$ are mixed.

The general molecular equation is as follows,

    $\text{Overall equation: KBr}\left(aq\right){\text{+ AgNO}}_{\text{3}}\left(aq\right)\to {\text{ KNO}}_{\text{3}}\left(aq\right)\text{+ AgBr}\left(s\right)$

Ionic equation is an equation in which ions are explicitly shown.

  $\begin{array}{l}\underset{\_}{\text{Complete ionic equation: }}\\ \\ {\text{K}}^{\text{+}}\left(aq\right){\text{+ Br}}^{\text{-}}\left(aq\right){\text{+ Ag}}^{\text{+}}\left(aq\right){\text{+ NO}}_{\text{3}}{}^{\text{-}}\left(aq\right)\to \text{AgBr}\left(s\right){\text{ + K}}^{\text{+}}\left(aq\right)+{\text{NO}}_{\text{3}}{}^{\text{-}}\left(aq\right)\end{array}$

Net ionic equation is the chemical equation for a reaction which lists only those species participating in the reaction.

The net ionic equation is determined as follows,

  $\begin{array}{l}\underset{\_}{\text{Net ionic equation:}}\\ \\ {\text{Br}}^{\text{-}}\left(aq\right){\text{+ Ag}}^{\text{+}}\left(aq\right)\to \text{AgBr}\left(s\right)\end{array}$

To write the net ionic equation, steps mentioned below must be followed.

The balanced molecular equation is first determined.

The ionic equation showing the strong electrolytes completely dissociated into cations and anions.

The spectator ions ${\text{K}}^{\text{+}}\left(aq\right)+{\text{NO}}_{\text{3}}{}^{\text{-}}\left(aq\right)$ on both sides of the ionic equation get cancelled.

Finally, the charges and number of atoms are checked that they are balanced in the net ionic equation.

(b)

Interpretation Introduction

Interpretation:

The net ionic equation has to be written if reaction occurs when solutions of nitric acid and calcium metal are mixed.

Explanation of Solution

Given: solutions of nitric acid, ${\text{HNO}}_{\text{3}}$ and calcium metal, $\text{Ca}$ are mixed.

No reaction occurs since formed $\text{Ca}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}$ is soluble and again forms the reactants.

(c)

Interpretation Introduction

Interpretation:

The net ionic equation has to be written if reaction occurs on mixing lithium hydroxide and iron $\left(\text{III}\right)$ chloride solutions.

Explanation of Solution

Given: solutions of lithium hydroxide $\text{LiOH}$ and iron $\left(\text{III}\right)$ chloride ${\text{FeCl}}_{\text{3}}$ are mixed.

The general molecular equation is as follows,

    $\text{Overall equation: 3LiOH}\left(aq\right){\text{+ FeCl}}_{\text{3}}\left(aq\right)\to \text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\text{+ 3LiCl}\left(aq\right)$

Ionic equation is an equation in which ions are explicitly shown.

  $\begin{array}{l}\underset{\_}{\text{Complete ionic equation: }}\\ \\ {\text{3Li}}^{\text{+}}\left(aq\right){\text{+ 3OH}}^{\text{-}}\left(aq\right){\text{+ Fe}}^{\text{3+}}\left(aq\right){\text{+ 3Cl}}^{\text{-}}\left(aq\right)\to \text{Fe}{\left(\text{OH}\right)}_3\left(s\right){\text{ + 3Li}}^{\text{+}}\left(aq\right)+{\text{ 3Cl}}^{\text{-}}\left(aq\right)\end{array}$

Net ionic equation is the chemical equation for a reaction which lists only those species participating in the reaction.

The net ionic equation is determined as follows,

  $\begin{array}{l}\underset{\_}{\text{Net ionic equation:}}\\ \\ {\text{3OH}}^{\text{-}}\left(aq\right){\text{+ Fe}}^{\text{3+}}\left(aq\right)\to \text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\end{array}$

To write the net ionic equation, steps mentioned below must be followed.

The balanced molecular equation is first determined.

The ionic equation showing the strong electrolytes completely dissociated into cations and anions.

The spectator ions ${\text{3Li}}^{\text{+}}\left(aq\right)+{\text{ 3Cl}}^{\text{-}}\left(aq\right)$ on both sides of the ionic equation get cancelled.

Finally, the charges and number of atoms are checked that they are balanced in the net ionic equation.