Question

What is the net ionic equation when aqueous solutions of Pb(NO3)2 and NH4Cl are mixed?

(a) NH4 (aq) NO3−(aq) → NH4NO3(s)
(b) Pb2 (aq) 2NO3−(aq) 2NH4 (aq) 2Cl− → PbCl2(s)
(c) 2NO3−(aq) 2NH4 (aq) NH4 (aq) NO3−(aq) → 2NO(g) 2H2O(l)
(d) Pb2 (aq) 2Cl−(aq) → PbCl2(s)

Answer 1

The net ionic equation for the reaction between aqueous solutions of Pb(NO3)2 and NH4Cl, which form PbCl2 as a precipitate, is Pb2+ (aq) + 2Cl-(aq) → PbCl2(s).

Step-by-step explanation:

When aqueous solutions of Pb(NO3)2 and NH4Cl are mixed, a precipitation reaction occurs because a solid product, PbCl2, forms. In a net ionic equation, we only include the ions that participate in the reaction to form the precipitate. The spectator ions are omitted. Therefore, the net ionic equation for the lead nitrate and ammonium chloride reaction is:

Pb2+ (aq) + 2Cl−(aq) → PbCl2(s)

This equation shows that lead ions (Pb2+) and chloride ions (Cl−) come together to form lead(II) chloride (PbCl2) as a solid precipitate. The nitrate (NO3−) and ammonium (NH4+) ions remain in solution as they are not part of the precipitate and therefore do not appear in the net ionic equation.