Mercury(I) ions (Hg₂²⁺) can be removed from solution by precipitation with Cl^- Suppose that a solution contains aqueous Hg₂(NO₃)₂. Write complete ionic and net ionic equations for the reaction of aqueous Hg₂(NO₃)₂ with aqueous sodium chloride to form solid Hg₂Cl₂ and aqueous sodium nitrate.

Key Concepts

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. For example, in the reaction between mercury(I) nitrate and sodium chloride, both compounds dissociate into their respective ions before the precipitation occurs.

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions react to form an insoluble solid, known as a precipitate. This process is driven by the formation of a compound that is not soluble in water, such as Hg2Cl2 in this case. Identifying the precipitate is crucial for writing the net ionic equation, which focuses on the species that undergo a change during the 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 results in an equation that highlights the essential components of the reaction, showing only the ions and molecules that undergo a change. For the reaction of Hg2(NO3)2 with NaCl, the net ionic equation will illustrate the formation of solid Hg2Cl2 from the reacting ions.