Chapter 4, Problem 58E

(a)

Interpretation Introduction

Interpretation: The molecular equation, complete ionic equation and net ionic equation representing the reaction of aqueous ammonia and nitric acid are to be stated.

Concept introduction: The chemical equation in which molecules of reactants and products are present is termed as molecular equation. The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the chemical equation which contains ions only is termed as complete ionic equation. The equation obtained by the elimination of spectator ions from the complete ionic equation is known as net ionic equation.

Answer to Problem 58E

The molecular equation is shown below.

  ${\text{NH}}_3\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NH}}_4{\text{NO}}_3\left(aq\right)$

The complete ionic equation is shown below.

  ${\text{NH}}_3\left(aq\right)+{\text{H}}^{+}\left(aq\right)+{\text{NO}}_3{}^{-}\left(aq\right)\to {\text{NH}}_4{}^{+}\left(aq\right)+{\text{NO}}_3{}^{-}\left(aq\right)$

The net ionic equation is ${\text{NH}}_3\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)\to {\text{NH}}_4{}^{+}\left(\text{aq}\right)$ .

Explanation of Solution

The molecular equation representing the reaction between aqueous ammonia and nitric acid is shown below.

  ${\text{NH}}_3\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NH}}_4{\text{NO}}_3\left(aq\right)$

The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the complete ionic equation representing the reaction between aqueous ammonia and nitric acid is shown below.

  ${\text{NH}}_3\left(aq\right)+{\text{H}}^{+}\left(aq\right)+{\text{NO}}_3{}^{-}\left(aq\right)\to {\text{NH}}_4{}^{+}\left(aq\right)+{\text{NO}}_3{}^{-}\left(aq\right)$

The net ionic equation is obtained by eliminating the spectator ions present on left and right side of the complete ionic equation. Therefore, the net ionic equation representing the formation of precipitate is shown below.

  ${\text{NH}}_3\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)\to {\text{NH}}_4{}^{+}\left(\text{aq}\right)$

(b)

Interpretation Introduction

Interpretation: The molecular equation, complete ionic equation and net ionic equation representing the reaction of aqueous barium hydroxide and hydrochloric acid are to be stated.

Concept introduction: The chemical equation in which molecules of reactants and products are present is termed as molecular equation. The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the chemical equation which contains ions only is termed as complete ionic equation. The equation obtained by the elimination of spectator ions from the complete ionic equation is known as net ionic equation.

Answer to Problem 58E

The molecular equation is shown below.

  $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\left(aq\right)+2\text{HCl}\left(aq\right)\to {\text{BaCl}}_{\text{2}}\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)$

The complete ionic equation is shown below.

  $\begin{array}{l}{\text{Ba}}^{2+}\left(aq\right)+2{\text{OH}}^{-}\left(aq\right)+2{\text{H}}^{+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)\to \\ {\text{Ba}}^{2+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)\end{array}$

The net ionic equation is ${\text{OH}}^{-}\left(aq\right)+{\text{H}}^{+}\left(aq\right)\to {\text{H}}_2\text{O}\left(l\right)$ .

Explanation of Solution

The molecular equation representing the reaction between barium hydroxide and hydrochloric acid is shown below.

  $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\left(aq\right)+2\text{HCl}\left(aq\right)\to {\text{BaCl}}_{\text{2}}\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)$

The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the complete ionic equation representing the reaction between barium hydroxide and hydrochloric acid is shown below.

  $\begin{array}{l}{\text{Ba}}^{2+}\left(aq\right)+2{\text{OH}}^{-}\left(aq\right)+2{\text{H}}^{+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)\to \\ {\text{Ba}}^{2+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)\end{array}$

The net ionic equation is obtained by eliminating the spectator ions present on left and right side of the complete ionic equation. Therefore, the net ionic equation representing the formation of precipitate is shown below.

  ${\text{OH}}^{-}\left(aq\right)+{\text{H}}^{+}\left(aq\right)\to {\text{H}}_2\text{O}\left(l\right)$

(c)

Interpretation Introduction

Interpretation: The molecular equation, complete ionic equation and net ionic equation representing the reaction of perchloric acid and solid iron $\left(\text{III}\right)$ hydroxide are to be stated.

Concept introduction: The chemical equation in which molecules of reactants and products are present is termed as molecular equation. The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the chemical equation which contains ions only is termed as complete ionic equation. The equation obtained by the elimination of spectator ions from the complete ionic equation is known as net ionic equation.

Answer to Problem 58E

The molecular equation is shown below.

  ${\text{3HClO}}_{\text{4}}\left(aq\right)+\text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\to \text{Fe}{\left({\text{ClO}}_{\text{4}}\right)}_{\text{3}}\left(aq\right)+3{\text{H}}_2\text{O}\left(l\right)$

The complete ionic equation is shown below.

  $\begin{array}{l}{\text{3H}}^{+}\left(aq\right)+3{\text{ClO}}_{\text{4}}{}^{-}\left(aq\right)+\text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\to \\ {\text{Fe}}^{3+}\left(aq\right)+3{\text{ClO}}_{\text{4}}{}^{-}\left(aq\right)+3{\text{H}}_2\text{O}\left(l\right)\end{array}$

The net ionic equation is ${\text{3H}}^{+}\left(aq\right)+\text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\to {\text{Fe}}^{3+}\left(aq\right)+3{\text{H}}_2\text{O}\left(l\right)$ .

Explanation of Solution

The molecular equation representing the reaction between perchloric acid and solid iron $\left(\text{III}\right)$ hydroxide is shown below.

  ${\text{3HClO}}_{\text{4}}\left(aq\right)+\text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\to \text{Fe}{\left({\text{ClO}}_{\text{4}}\right)}_{\text{3}}\left(aq\right)+3{\text{H}}_2\text{O}\left(l\right)$

The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the complete ionic equation representing the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and $\text{HCl}$ is shown below.

  $\begin{array}{l}{\text{3H}}^{+}\left(aq\right)+3{\text{ClO}}_{\text{4}}{}^{-}\left(aq\right)+\text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\to \\ {\text{Fe}}^{3+}\left(aq\right)+3{\text{ClO}}_{\text{4}}{}^{-}\left(aq\right)+3{\text{H}}_2\text{O}\left(l\right)\end{array}$

The net ionic equation is obtained by eliminating the spectator ions present on left and right side of the complete ionic equation. Therefore, the net ionic equation representing the formation of precipitate is shown below.

  ${\text{3H}}^{+}\left(aq\right)+\text{Fe}{\left(\text{OH}\right)}_3\left(s\right)\to {\text{Fe}}^{3+}\left(aq\right)+3{\text{H}}_2\text{O}\left(l\right)$

(d)

Interpretation Introduction

Interpretation: The molecular equation, complete ionic equation and net ionic equation representing the reaction of solid silver hydroxide and hydrobromic acid are to be stated.

Concept introduction: The chemical equation in which molecules of reactants and products are present is termed as molecular equation. The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the chemical equation which contains ions only is termed as complete ionic equation. The equation obtained by the elimination of spectator ions from the complete ionic equation is known as net ionic equation.

Answer to Problem 58E

The molecular equation is shown below.

  $\text{AgOH}\left(s\right)+\text{HBr}\left(aq\right)\to \text{AgBr}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)$

The complete ionic equation is shown below.

  $\text{AgOH}\left(s\right)+{\text{H}}^{+}\left(aq\right)+{\text{Br}}^{-}\left(aq\right)\to \text{AgBr}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)$

The net ionic equation is $\text{AgOH}\left(s\right)+{\text{H}}^{+}\left(aq\right)+{\text{Br}}^{-}\left(aq\right)\to \text{AgBr}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)$ .

Explanation of Solution

The molecular equation representing the reaction between solid silver hydroxide and hydrobromic acid is shown below.

  $\text{AgOH}\left(s\right)+\text{HBr}\left(aq\right)\to \text{AgBr}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)$

The substance that are strong electrolytes will get dissociate into their constituent ions. Therefore, the complete ionic equation representing the reaction between solid silver hydroxide and hydrobromic acid is shown below.

  $\text{AgOH}\left(s\right)+{\text{H}}^{+}\left(aq\right)+{\text{Br}}^{-}\left(aq\right)\to \text{AgBr}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)$

The net ionic equation is obtained by eliminating the spectator ions present on left and right side of the complete ionic equation.

Therefore, the net ionic equation representing the formation of precipitate is shown below.

  $\text{AgOH}\left(s\right)+{\text{H}}^{+}\left(aq\right)+{\text{Br}}^{-}\left(aq\right)\to \text{AgBr}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)$