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

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

Answer: (C)

Verified step by step guidance

1. Identify the reactants and products in the given reaction: magnesium sulfate (MgSO_4) and barium nitrate (Ba(NO_3)_2) are both aqueous, meaning they dissociate into their ions in solution.
2. Write the full ionic equation by breaking all strong electrolytes (soluble salts) into their constituent ions: MgSO_4(aq) dissociates into Mg^{2+}(aq) and SO_4^{2-}(aq), and Ba(NO_3)_2(aq) dissociates into Ba^{2+}(aq) and NO_3^{-}(aq).
3. Determine the precipitate formed by checking the solubility rules: BaSO_4 is insoluble and forms a solid precipitate, while Mg(NO_3)_2 remains soluble and stays dissociated in solution.
4. Write the net ionic equation by including only the species that participate in the formation of the precipitate: Ba^{2+}(aq) and SO_4^{2-}(aq) combine to form solid BaSO_4(s).
5. Exclude the spectator ions (ions that do not change during the reaction), which are Mg^{2+}(aq) and NO_3^{-}(aq), from the net ionic equation.