Answer
Acid and base used to form this ion, respectively, : $HNO_2$ and $NaOH$,
Complete ionic equation:
$HNO_2(aq) + Na^+(aq) + OH^-(aq) -- \gt Na^+(aq) + NO{_2}^-(aq) + H_2O(l) $
Net ionic equation:
$HNO_2(aq) + OH^-(aq) -- \gt NO{_2}^-(aq) + H_2O(l) $
Work Step by Step
1. Identify the ions of the salt: $(NaNO_2)$:
$Na^+$ and $N{O_2}^-$:
To the cation, add a hydroxide ion: $NaOH$; this is the base.
To the anion, add a hydrogen ion: $HNO_2$; this is the acid.
2. Now, write the balanced overall equation between then, which is:
$Acid + Base -- \gt Salt + Water$
We already have the salt so:
$HNO_2(aq) + NaOH(aq) -- \gt NaNO_2(aq) + H_2O(l)$
3. Write the complete ionic equation.
- For the completely dissociated/ionized compounds, separate them by their ions:
$HNO_2(aq) + Na^+(aq) + OH^-(aq) -- \gt Na^+(aq) + NO{_2}^-(aq) + H_2O(l) $
* NaOH is a strong base, and $NaNO_2$ is soluble according to the table 3.1, because it is a compound with the $Na^+$ ion.
4. Remove the repeated ions:
$HNO_2(aq) + OH^-(aq) -- \gt NO{_2}^-(aq) + H_2O(l) $
This is the net ionic equation.
