Chapter 9, Problem 16PE

Interpretation Introduction

Interpretation:

The conventional, total ionic, and net ionic equations for the reaction between solutions of ammonium nitrate and sodium hydroxide are to be written.

Concept Introduction:

An ion-combination reaction is a reaction in which cation from one reactant combines with the anion from another reactant and form a particular kind of product. The product is an insoluble ionic compound that settles at the bottom of mixed solution. A chemical equation that shows the number of species or ions participating in the reaction is known as net ionic equation.

Answer to Problem 16PE

The conventional equation for the reaction between solutions of ammonium nitrate and sodium hydroxide is written below.

${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}\left(\text{aq}\right)+\text{NaOH}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)+{\text{NaNO}}_{\text{3}}\left(\text{aq}\right)$

The total ionic equation is written below.

${\text{NH}}_{\text{4}}{}^{+}\left(\text{aq}\right)+{\text{NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)+{\text{Na}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)+{\text{Na}}^{+}\left(\text{aq}\right)+{\text{NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)$ The net ionic equation is written below.

${\text{NH}}_{\text{4}}{}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

Explanation of Solution

The conventional equation for the reaction between solutions of ammonium nitrate and sodium hydroxide is written below.

${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}\left(\text{aq}\right)+\text{NaOH}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)+{\text{NaNO}}_{\text{3}}\left(\text{aq}\right)$

The ions of ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$ are ${\text{NH}}_{\text{4}}{}^{+}$ and ${\text{NO}}_{\text{3}}{}^{-}$. The ions of $\text{NaOH}$ are ${\text{Na}}^{+}$ and ${\text{OH}}^{-}$.

Therefore, the total ionic equation is written below.

${\text{NH}}_{\text{4}}{}^{+}\left(\text{aq}\right)+{\text{NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)+{\text{Na}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)+{\text{Na}}^{+}\left(\text{aq}\right)+{\text{NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)$

The sodium and nitrate ions get cancel out from both sides of the reaction.

Therefore, the net ionic equation is written below.

${\text{NH}}_{\text{4}}{}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

Conclusion

The conventional equation for the reaction between solutions of ammonium nitrate and sodium hydroxide is written below.

${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}\left(\text{aq}\right)+\text{NaOH}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)+{\text{NaNO}}_{\text{3}}\left(\text{aq}\right)$

The total ionic equation is written below.

${\text{NH}}_{\text{4}}{}^{+}\left(\text{aq}\right)+{\text{NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)+{\text{Na}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)+{\text{Na}}^{+}\left(\text{aq}\right)+{\text{NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)$ The net ionic equation is written below.

${\text{NH}}_{\text{4}}{}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)\to {\text{NH}}_{\text{3}}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$