Final answer:
The net ionic equation for the reaction between an aqueous solution of Chromium (III) Chloride and aqueous lead (II) Nitrate, after eliminating spectator ions, is Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s), indicating the formation of a precipitate, lead (II) chloride.
Step-by-step explanation:
The reaction between an aqueous solution of Chromium (III) Chloride and an aqueous solution of lead (II) Nitrate involves a double replacement reaction, where the ions in the reactants switch partners. The products formed can include a precipitate if one of the new compounds is insoluble in water. Based on solubility rules, Chromium compounds and nitrates are generally soluble, while lead (II) chloride is not, leading to formation of a precipitate.
The net ionic equation for this reaction, after eliminating the spectator ions, is:
Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s)
This represents the formation of lead (II) chloride, which is insoluble and precipitates out of the solution.