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 ^(+)`