Questions: Write the balanced NET ionic equation for the reaction when Pb(NO3)2 and RbCl are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.

Solution Steps

When lead(II) nitrate, \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\), and rubidium chloride, \(\mathrm{RbCl}\), are mixed in aqueous solution, they undergo a double displacement reaction. The products of this reaction are lead(II) chloride, \(\mathrm{PbCl}_{2}\), and rubidium nitrate, \(\mathrm{RbNO}_{3}\).

The balanced molecular equation is:

\[ \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(aq) + 2\mathrm{RbCl}(aq) \rightarrow \mathrm{PbCl}_{2}(s) + 2\mathrm{RbNO}_{3}(aq) \]

Next, we write the complete ionic equation by dissociating all strong electrolytes (soluble ionic compounds) into their constituent ions:

\[ \mathrm{Pb}^{2+}(aq) + 2\mathrm{NO}_{3}^{-}(aq) + 2\mathrm{Rb}^{+}(aq) + 2\mathrm{Cl}^{-}(aq) \rightarrow \mathrm{PbCl}_{2}(s) + 2\mathrm{Rb}^{+}(aq) + 2\mathrm{NO}_{3}^{-}(aq) \]

Spectator ions are ions that appear on both sides of the complete ionic equation and do not participate in the actual chemical reaction. In this case, the spectator ions are \(\mathrm{Rb}^{+}\) and \(\mathrm{NO}_{3}^{-}\).

After removing the spectator ions, the net ionic equation is:

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

Final Answer