Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.

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Identify the reactants and products in the reaction: Lead(II) nitrate (Pb(NO_3)_2) and potassium sulfate (K_2SO_4) are the reactants, while lead(II) sulfate (PbSO_4) and potassium nitrate (KNO_3) are the products.

Write the balanced molecular equation for the reaction: Pb(NO_3)_2(aq) + K_2SO_4(aq) \(\rightarrow\) PbSO_4(s) + 2KNO_3(aq).

Break down the soluble ionic compounds into their constituent ions to write the complete ionic equation: Pb^{2+}(aq) + 2NO_3^-(aq) + 2K^+(aq) + SO_4^{2-}(aq) \(\rightarrow\) PbSO_4(s) + 2K^+(aq) + 2NO_3^-(aq).

Identify and cancel out the spectator ions, which are ions that appear on both sides of the complete ionic equation: The spectator ions are 2K^+(aq) and 2NO_3^-(aq).

Write the net ionic equation by removing the spectator ions: Pb^{2+}(aq) + SO_4^{2-}(aq) \(\rightarrow\) PbSO_4(s).

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주요 개념

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Ionic Equations

Ionic equations represent the dissociation of soluble ionic compounds in solution. In these equations, strong electrolytes are shown as their constituent ions, allowing for a clearer understanding of the chemical species involved in a reaction. This is crucial for identifying which ions participate in the reaction and which remain unchanged.

Precipitation Reactions

Precipitation reactions occur when two soluble ionic compounds react to form an insoluble solid, known as a precipitate. In this case, lead(II) sulfate is the precipitate formed from the reaction of lead(II) nitrate and potassium sulfate. Understanding the solubility rules helps predict whether a precipitate will form in a given reaction.

Net Ionic Equations

Net ionic equations simplify ionic equations by removing spectator ions—ions that do not participate in the actual chemical reaction. This focuses on the species that undergo a change, providing a clearer picture of the reaction's essence. For the given reaction, the net ionic equation highlights the formation of solid lead(II) sulfate from lead(II) and sulfate ions.