Question

The following molecular equation represents the reaction that occurs when aqueous solutions of lead(II) nitrate and

chromium(II) chloride are combined.
Pb(NO-3)_2 (aq) + CrCl_2 (aq) —>PbCl_2 (s) + Cr(NO_3)_2 (aq)
Write the balanced net ionic equation for the reaction.

Answer 1

The balanced net ionic equation for the reaction of lead(II) nitrate with chromium(II) chloride is Pb2+(aq) + 2Cl-(aq) → PbCl2(s), which shows the formation of lead(II) chloride precipitate.

Step-by-step explanation:

To write the balanced net ionic equation for the reaction that occurs when aqueous solutions of lead(II) nitrate and chromium(II) chloride are combined, we need to first write the full ionic equation and then cancel out the spectator ions.

The full ionic equation is:

• Pb2+(aq) + 2NO3-(aq) + Cr2+(aq) + 2Cl-(aq) → PbCl2(s) + Cr2+(aq) + 2NO3-(aq)

Notice that the chromium ions (Cr2+) and the nitrate ions (NO3-) appear on both sides of the equation and therefore are spectator ions. Removing the spectator ions gives the net ionic equation:

• Pb2+(aq) + 2Cl-(aq) → PbCl2(s)

This is the balanced net ionic equation for the precipitation of lead(II) chloride when lead(II) nitrate reacts with chromium(II) chloride in aqueous solution, highlighting that lead(II) ions combine with chloride ions to form the insoluble salt, lead(II) chloride.