Question

Write the net ionic equation for the equilibrium that is established when ammonium nitrate is dissolved in water.

Answer 1

$NH _{4} ^{+} + H_{2} O \ \textless \ ----\ \textgreater \ NH _{3} + H_{3}O ^{+}$Answer : - While dissolving nitrate in water the pH of water becomes slightly acidic. The reaction is explained below :

At the first stage ammonium nitrate is dissolved in water:-

$NH _{4} NO_{3} + H_{2} O ----\ \textgreater \ NH_{4} ^{+} + NO_{3} ^{-}$

In the later stage when excess of ammonium ions are produced in water then these ions react with water again producing acidic hydronium ions. 

A reversible reaction occurs at this stage. 

$NH _{4} ^{+} + H_{2} O \ \textless \ ----\ \textgreater \ NH _{3} + H_{3}O ^{+}$

So the net ionic equation for this reaction will be :-

$NH _{4} ^{+} + H_{2} O ----\ \textgreater \ NH _{3} + H_{3}O ^{+}$