## Chemistry: The Molecular Science (5th Edition)

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: $HNO_2(aq) + OH^-(aq) -- \gt NO{_2}^-(aq) + H_2O(l)$
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.