Question

which of the following is the correct net ionic equation for the reaction that occurs when solutions of pb(no₃)₂ and nh₄cl are mixed?
pb(no₃)₂(aq) + 2nh₄cl(aq) → nh₄no₃(aq) + pbcl₂(s)
pb²⁺(aq) + 2cl⁻(aq) → pbcl₂(s)
pb²⁺(aq) + 2no₃⁻(aq) + 2nh₄⁺(aq) + 2cl⁻(aq) → 2nh₄⁺(aq) + 2no₃⁻(aq) + pbcl₂(s)
nh₄⁺(aq)+ no₃⁻(aq) → 2nh₄no₃(s)
no reaction occurs when the solutions are mixed.

Explanation:

Step1: Write the balanced molecular equation

$Pb(NO_3)_2(aq)+2NH_4Cl(aq)
ightarrow 2NH_4NO_3(aq) + PbCl_2(s)$

Step2: Write the complete ionic equation

$Pb^{2 +}(aq)+2NO_3^{-}(aq)+2NH_4^{+}(aq)+2Cl^{-}(aq)
ightarrow 2NH_4^{+}(aq)+2NO_3^{-}(aq)+PbCl_2(s)$

Step3: Identify and cancel out spectator ions

Spectator ions are $NH_4^{+}$ and $NO_3^{-}$. After canceling them, we get the net - ionic equation.
$Pb^{2+}(aq)+2Cl^{-}(aq)
ightarrow PbCl_2(s)$

Answer:

$Pb^{2+}(aq)+2Cl^{-}(aq)
ightarrow PbCl_2(s)$