Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of...

Question:

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO{eq}_3{/eq} and HI are mixed.

Ionic Equation:

Ionic equations involve the compounds dissolved in water in the form of dissociated ions. A net ionic equation represents the formation of precipitate because spectator ions are eliminated.

Answer and Explanation: 1

The balanced chemical equation for the reaction of aqueous solution of {eq}{\rm{MgS}}{{\rm{O}}_3}{/eq} and {eq}{\rm{HI}}{/eq} is given as follows:

{eq}{\rm{MgS}}{{\rm{O}}_3}\left( {aq} \right) + {\rm{HI}}\left( {aq} \right) \to {\rm{Mg}}{{\rm{I}}_2}\left( {aq} \right) + {\rm{S}}{{\rm{O}}_2}\left( g \right) + {{\rm{H}}_2}{\rm{O}}\left( l \right){/eq}

Because only a solution of compounds in an aqueous state dissociate, after the dissociation of compounds, the ionic equation is given as follows:

{eq}{\rm{M}}{{\rm{g}}^{2 + }}{\rm{ + SO}}_3^{2 - } + 2{{\rm{H}}^ + }{\rm{ + 2}}{{\rm{I}}^ - } \to {\rm{M}}{{\rm{g}}^{2 + }}{\rm{ + 2}}{{\rm{I}}^ - } + {\rm{S}}{{\rm{O}}_2}\left( g \right) + {{\rm{H}}_2}{\rm{O}}\left( l \right){/eq}

Here, the spectator ions are {eq}{\rm{M}}{{\rm{g}}^{2 + }}{/eq} and {eq}2{{\rm{I}}^ - }{/eq}. They are present on both the reactant side and the product side in equal amounts so after eliminating the spectator ions, the net ionic equation is as follows:

{eq}{\rm{SO}}_3^{2 - } + 2{{\rm{H}}^ + } \to {\rm{S}}{{\rm{O}}_2}\left( g \right) + {{\rm{H}}_2}{\rm{O}}\left( l \right){/eq}

Therefore, the net ionic equation for the reaction of aqueous solution of {eq}{\rm{MgS}}{{\rm{O}}_3}{/eq} and {eq}{\rm{HI}}{/eq} is {eq}\boxed{{\rm{SO}}_3^{2 - } + 2{{\rm{H}}^ + } \to {\rm{S}}{{\rm{O}}_2}\left( g \right) + {{\rm{H}}_2}{\rm{O}}\left( l \right)}{/eq}