Based on the solubility rules, which of the following is the correct net ionic e

Question

Based on the solubility rules, which of the following is the correct net ionic equation for the reaction that occurs when solutions of lead (II) nitrate, Pb(NO_3)2, and ammonium chloride, NH_4Cl, are mixed? Pb(NO_3)_2(aq) plus_NH_4Cl(aq) rightarrow + Pb(NO_3)_2(aq) plus 2NH_4CI(aq) rightarrow NH_4NO_3 plus pbCl_2(s) Pb^plus 2 (aq) + 2CI^-(aq) rightarrow l_2(s) P b^plus 2 (aq) + 2NO_3^-(aq) + 2NH_4^+(aq) + 2Cl^-(aq) rightarrow 2NH_4^plus(aq) + 2NO_3^minus(aq) + PbCl_2(s) NH_4(aq) + NO_3^minus (aq) -> 2 NH_4 NO_3 (s) No reaction occurs when the solutions are mixed.

Explanation / Answer

If this is the equation:
Pb(NO3)2(aq) + 2 NH4Cl(aq) ---> NH4NO3(aq) + PbCl2(s)

when we strike out the spectator ions from option c, we are left with the following net ionic equations
The net ionic equation would be:
B. Pb+2(aq) + 2 Cl-(aq) ---> PbCl2(s)

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