When solutions of KCl and Pb(NO3)2 are mixed a precipitate forms. Write the molecular ionic and net ionic equations for this reaction.?

When solutions of KCl and Pb(NO3)2 are mixed, lead(II) chloride (PbCl2) precipitates. The molecular equation is:

[ \text{2 KCl (aq) + Pb(NO}_3\text{)}_2\text{ (aq) } \rightarrow \text{ 2 KNO}_3\text{ (aq) + PbCl}_2\text{ (s)} ]

The complete ionic equation is:

[ \text{2 K}^+ (aq) + \text{2 Cl}^- (aq) + \text{Pb}^{2+} (aq) + \text{2 NO}_3^- (aq) \rightarrow \text{2 K}^+ (aq) + \text{2 NO}_3^- (aq) + \text{PbCl}_2 (s) ]

The net ionic equation, showing only the species that participate in the formation of the precipitate, is:

[ \text{Pb}^{2+} (aq) + \text{2 Cl}^- (aq) \rightarrow \text{PbCl}_2 (s) ]