Answer
This is the net ionic reaction for the neutralization of added acids to this buffer:
$H^+(aq) + N{H_3}(aq) \lt -- \gt N{H_4}^+$
Work Step by Step
- Nitric acid: $HNO_3$.
When an acid is added to a buffer, its base is going to try to neutralize the added compound:
$HNO_3(aq) + NH_3(aq) \lt -- \gt N{O_3}^-(aq) + N{H_4}^+(aq)$
To write the net ionic equation, identify the totally ionizated/dissociated compounds: $HNO_3$, and break them into ions:
$H^+(aq) + N{O_3}^-(aq) + NH_3(aq) \lt -- \gt N{O_3}^-(aq) + N{H_4}^-(aq)$
- Remove the spectators ions:
$H^+(aq) + N{H_3}(aq) \lt -- \gt N{H_4}^+$
