Question

consider the reaction when aqueous solutions of lead(ii) nitrate and nickel(ii) chloride are combined. the net ionic equation for this reaction is: (be sure to specify states such as (aq) or (s). if a box is not needed leave it blank. if no reaction occurs leave all boxes blank and click on \submit\).

Explanation:

Step1: Write the molecular equation

Lead(II) nitrate is $Pb(NO_3)_2(aq)$ and nickel(II) chloride is $NiCl_2(aq)$. They react via a double - displacement reaction. The products are lead(II) chloride $PbCl_2(s)$ (since it is insoluble) and nickel(II) nitrate $Ni(NO_3)_2(aq)$. The molecular equation is $Pb(NO_3)_2(aq)+NiCl_2(aq)
ightarrow PbCl_2(s)+Ni(NO_3)_2(aq)$.

Step2: Write the complete ionic equation

The complete ionic equation shows all the ions in solution. $Pb^{2 +}(aq)+2NO_3^{-}(aq)+Ni^{2 +}(aq)+2Cl^{-}(aq)
ightarrow PbCl_2(s)+Ni^{2 +}(aq)+2NO_3^{-}(aq)$.

Step3: Write the net ionic equation

Cancel out the spectator ions ($Ni^{2+}$ and $NO_3^{-}$). The net ionic equation is $Pb^{2 +}(aq)+2Cl^{-}(aq)
ightarrow PbCl_2(s)$.

Answer:

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