Which of the following is the correct net ionic equation for the reaction between MgSO4(aq) and Pb(NO3)2(aq)?

• A. Pb^{2+}(aq) + SO_4^{2-}(aq) → PbSO_4(s)
• B. Mg^{2+}(aq) + SO_4^{2-}(aq) → MgSO_4(s)
• C. Mg^{2+}(aq) + NO_3^{-}(aq) → Mg(NO_3)_2(aq)
• D. MgSO_4(aq) + Pb(NO_3)_2(aq) → Mg(NO_3)_2(aq) + PbSO_4(aq)

Answer: (A)

Verified step by step guidance

1. Write the balanced molecular equation for the reaction between magnesium sulfate and lead(II) nitrate: \(\mathrm{MgSO_4(aq) + Pb(NO_3)_2(aq) \rightarrow ?}\).
2. Identify the ions present in the aqueous solutions: \(\mathrm{MgSO_4}\) dissociates into \(\mathrm{Mg^{2+}(aq)}\) and \(\mathrm{SO_4^{2-}(aq)}\), and \(\mathrm{Pb(NO_3)_2}\) dissociates into \(\mathrm{Pb^{2+}(aq)}\) and \(\mathrm{NO_3^{-}(aq)}\).
3. Determine which ions will form a precipitate by checking the solubility rules. Lead(II) sulfate (\(\mathrm{PbSO_4}\)) is insoluble and will precipitate, while magnesium nitrate and magnesium sulfate remain soluble.
4. Write the net ionic equation by including only the ions that form the precipitate: \(\mathrm{Pb^{2+}(aq) + SO_4^{2-}(aq) \rightarrow PbSO_4(s)}\).
5. Confirm that spectator ions (ions that do not participate in the formation of the precipitate) such as \(\mathrm{Mg^{2+}}\) and \(\mathrm{NO_3^{-}}\) are omitted from the net ionic equation.