Multiple Choice
Which of the following is the complete ionic equation for the reaction between HCl(aq) and NaOH(aq)?
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6. Chemical Quantities & Aqueous Reactions
Complete Ionic Equations
Multiple Choice
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)
Verified step by step guidance1
Write the balanced molecular equation for the reaction between magnesium sulfate and lead(II) nitrate: \(\mathrm{MgSO_4(aq) + Pb(NO_3)_2(aq) \rightarrow ?}\).
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 \(\mathrm{NO_3^{-}(aq)}\).
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.
Write the net ionic equation by including only the ions that form the precipitate: \(\mathrm{Pb^{2+}(aq) + SO_4^{2-}(aq) \rightarrow PbSO_4(s)}\).
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.
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