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

Complete ionic equation: $2H^+(aq) + S{O_4}^{2-}(aq) + Ba^{2+}(aq) + 2OH^-(aq) -- \gt Ba_2SO_4(s) + 2H_2O(l)$ Net ionic equation: $2H^+(aq) + S{O_4}^{2-}(aq) + Ba^{2+}(aq) + 2OH^-(aq) -- \gt Ba_2SO_4(s) + 2H_2O(l)$
1. Identify the salt produced by the mixture of this acid and this base. $H_2SO_4$ gives $SO{_4}^{2-}$ after reaction. $Ba(OH)_2$ gives $Ba^{2+}$ after reaction. Therefore, the salt formed is : $BaSO_4$ 2. Write the overall equation: $Acid + Base --\gt Salt + Water$ $H_2SO_4(aq) + Ba(OH)_2(aq) -- \gt BaSO_4(s) + H_2O(l)$ * The equation will be balanced if we add a "2" to the water molecules: $H_2SO_4(aq) + Ba(OH)_2(aq) -- \gt BaSO_4(s) + 2H_2O(l)$ ** According to table 3.1, $BaSO_4$ is not soluble in water. 3. On the totally dissociated/ionized compounds, write the separate ions: $2H^+(aq) + S{O_4}^{2-}(aq) + Ba^{2+}(aq) + 2OH^-(aq) -- \gt Ba_2SO_4(s) + 2H_2O(l)$ This is the complete ionic equation. 4. Remove the spectators ions: $2H^+(aq) + S{O_4}^{2-}(aq) + Ba^{2+}(aq) + 2OH^-(aq) -- \gt Ba_2SO_4(s) + 2H_2O(l)$ ** Notice, there are no repeated ions, so there are no spectators. This is the net ionic equation.