Need help chemistry ionic and net ionic equations?

Question

This is the equation I am having troble writing as ionic and net ionic equation.

K2CrO4 + Pb(NO3)2 --PbCrO4(s) + 2KNO3

Answer 1

In order to find the net ionic equation you must use a table of solutbilities to see which products are soluble in water and which will form a precipitate.

Here is a good hint: all nitrates are soluble, so that means that the potassium nitrate product is not going to form a precipitate and settle out of the solution. That leaves the lead chromate as the precipitate.

The ions that are left in the solution and do not precipitate out are the spectator ions. Spectator ions are not written in the net ionic equation - only the ions which form the precipitate.

K2CrO4 + Pb(NO3)2 ---> PbCrO4 + 2 KNO3

Cross off the ions which remain soluble before and after the reaction. In this case the nitrates and their cations.

2 K is crossed off and 2 NO3 is crossed off from both sides because they remain soluble in the products.

That leaves this as the net ionic equation:

CrO4 2- (aq) + Pb 2+ (aq) ---> PbCrO4 (s)