Chemistry: The Molecular Science (5th Edition)

Acid and base used to form this ion, respectively: $HNO_3$ and $Ba(OH)_2$ Complete ionic equation: $2H^+(aq) + 2NO{_3}^-(aq) + Ba^{2+}(aq) + 2OH^-(aq) -- \gt Ba^{2+}(aq) + 2NO{_3}^-(aq) + 2H_2O(l)$ Net ionic equation: $2H^+(aq) + 2OH^-(aq) -- \gt 2H_2O(l)$
1. Identify the ions of the salt: $(Ba(NO_3)_2)$: $Ba^{2+}$ and 2$N{O_3}^-$: To the cation, add a hydroxide ion: $Ba(OH)_2$; this is the base. To the anion, add a hydrogen ion: 2$HNO_3$; this is the acid. 2. Now, write the balanced overall equation between them, which is: $Acid + Base -- \gt Salt + Water$ We already have the salt, so: $2HNO_3(aq) + Ba(OH)_2(aq) -- \gt Ba(NO_3)_2(aq) + H_2O(l)$ Balance it: $2HNO_3(aq) + Ba(OH)_2(aq) -- \gt Ba(NO_3)_2(aq) + 2H_2O(l)$ 3. Write the complete ionic equation. - For the completely dissociated/ionized compounds, separate them by their ions: $2H^+(aq) + 2NO{_3}^-(aq) + Ba^{2+}(aq) + 2OH^-(aq) -- \gt Ba^{2+}(aq) + 2NO{_3}^-(aq) + 2H_2O(l)$ * $Ba(OH)_2$ is a strong base, and $Ba(NO_3)_2$ is soluble according to the table 3.1, because it is a compound with the $N{O_3}^-$ ion. ** $HNO_3$ is a strong acid, so it is completely dissociated. 4. Remove the repeated ions: $2H^+(aq) + 2OH^-(aq) -- \gt 2H_2O(l)$ This is the net ionic equation.