Chapter 9.3, Problem 56SSC

Interpretation Introduction

Interpretation:

The chemical and net ionic equations when nitric acid mixed with aqueous potassium hydrogen carbonate to produce aqueous potassium nitrate needs to be determined.

Concept introduction:

Net ionic equations are ionic equations that comprise only the particles that participate in the reaction. Net ionic equations are written from complete ionic equations by removing all spectator ions. Ions which do not take part in a reaction are termed as spectator ions and they are not shown in net ionic equations.

Answer to Problem 56SSC

The chemical reaction is as follows:

${\text{2HNO}}_{\text{3}}\left(\text{aq}\right)+2{\text{KHCO}}_{\text{3}}\left(\text{aq}\right)\to 2{\text{KNO}}_{\text{3}}\left(\text{aq}\right){\text{+2H}}_{\text{2}}\text{O}\left(\text{l}\right){\text{+2CO}}_{\text{2}}\left(\text{g}\right)$

Net ionic equation is

${\text{H}}^{+}\left(\text{aq}\right)\text{+}{\text{HCO}}_{\text{3}}{}^{-}(aq)\to {\text{H}}_{\text{2}}\text{O}\left(l\right)+{\text{CO}}_{\text{2}}(g)$

Explanation of Solution

Nitric acid mixed with aqueous potassium hydrogen carbonate to produce aqueous potassium nitrate. The chemical reaction is-

${\text{2HNO}}_{\text{3}}\left(\text{aq}\right)+2{\text{KHCO}}_{\text{3}}\left(\text{aq}\right)\to 2{\text{KNO}}_{\text{3}}\left(\text{aq}\right){\text{+2H}}_{\text{2}}\text{O}\left(\text{l}\right){\text{+2CO}}_{\text{2}}\left(\text{g}\right)$

The ionic equation is given below:

${\text{2H}}^{+}\left(\text{aq}\right){\text{+2NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)+2{\text{K}}^{+}\left(\text{aq}\right){\text{+2HCO}}_{\text{3}}{}^{-}\left(\text{aq}\right)\to 2{\text{K}}^{+}\left(\text{aq}\right){\text{+2NO}}_{\text{3}}{}^{-}\left(\text{aq}\right){\text{+2H}}_{\text{2}}\text{O}\left(l\right)+2{\text{CO}}_{\text{2}}(g)$

Net ionic equation is as follows:

$\begin{array}{l}{\text{2H}}^{+}\left(\text{aq}\right)\text{+}\cancel{{\text{2NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)}+\cancel{2{\text{K}}^{+}\left(\text{aq}\right)}{\text{+2HCO}}_{\text{3}}{}^{-}\left(\text{aq}\right)\to \cancel{2{\text{K}}^{+}\left(\text{aq}\right)}\text{+}\cancel{{\text{2NO}}_{\text{3}}{}^{-}\left(\text{aq}\right)}{\text{+2H}}_{\text{2}}\text{O}\left(l\right)+2{\text{CO}}_{\text{2}}(g)\\ {\text{2H}}^{+}\left(\text{aq}\right)\text{+}{\text{2HCO}}_{\text{3}}{}^{-}(aq)\to {\text{2H}}_{\text{2}}\text{O}\left(l\right)+2{\text{CO}}_{\text{2}}(g)\\ {\text{H}}^{+}\left(\text{aq}\right)\text{+}{\text{HCO}}_{\text{3}}{}^{-}(aq)\to {\text{H}}_{\text{2}}\text{O}\left(l\right)+{\text{CO}}_{\text{2}}(g)\end{array}$

Conclusion

A net ionic equation only shows those particles which participate in the reaction.