What is the net ionic equation for the reaction between MgSO4(aq) and Ba(NO3)2(aq)?

• A. Ba^{2+}(aq) + SO_4^{2-}(aq) ightarrow BaSO_4(s)
• B. BaSO_4(s) + 2NO_3^{-}(aq) ightarrow Ba^{2+}(aq) + SO_4^{2-}(aq)
• C. MgSO_4(aq) + Ba(NO_3)_2(aq) ightarrow Mg(NO_3)_2(aq) + BaSO_4(aq)
• D. Mg^{2+}(aq) + 2NO_3^{-}(aq) ightarrow Mg(NO_3)_2(aq)

Answer: (A)

Verified step by step guidance

1. Write the balanced molecular equation for the reaction between magnesium sulfate and barium nitrate: \(\mathrm{MgSO_4(aq) + Ba(NO_3)_2(aq) \rightarrow Mg(NO_3)_2(aq) + BaSO_4(s)}\).
2. Dissociate all strong electrolytes (soluble ionic compounds) into their ions to write the complete ionic equation: \(\mathrm{Mg^{2+}(aq) + SO_4^{2-}(aq) + Ba^{2+}(aq) + 2NO_3^{-}(aq) \rightarrow Mg^{2+}(aq) + 2NO_3^{-}(aq) + BaSO_4(s)}\).
3. Identify the spectator ions, which are ions that appear unchanged on both sides of the equation. Here, \(\mathrm{Mg^{2+}(aq)}\) and \(\mathrm{NO_3^{-}(aq)}\) are spectator ions.
4. Remove the spectator ions from the complete ionic equation to write the net ionic equation, which shows only the species that participate in the formation of the precipitate.
5. The net ionic equation is: \(\mathrm{Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s)}\), representing the formation of solid barium sulfate from its ions in solution.