Final answer:
The question involves a double-replacement precipitation reaction where mercury(II) nitrate and sodium phosphate form mercury(II) phosphate and sodium nitrate. The reaction exemplifies the application of solubility rules to predict precipitate formation.
Step-by-step explanation:
When aqueous solutions of mercury(II) nitrate and sodium phosphate are mixed, a precipitation reaction occurs, leading to the formation of a solid called mercury(II) phosphate and leaving behind an aqueous solution of sodium nitrate. This type of reaction is known as a double-replacement reaction where the cations and anions in the reacting compounds exchange partners to form new compounds.
To write the balanced chemical equation for this reaction, we can follow the pattern seen in similar precipitation reactions such as the formation of lead (II) chloride from lead (II) nitrate and sodium chloride:
- First, write the formulas for the reactants and products: Hg(NO₃)₂ + Na₃PO₄ → Hg₃(PO₄)₂ + NaNO₃.
- Then, balance the chemical equation to reflect the stoichiometry of the reaction.
This process demonstrates the use of solubility rules to predict which combinations of ions will result in the formation of a precipitate.