A solution contains the following ions: Hg2(2+) and Fe(2+). When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms. Write net ionic equations for the formation of each of the precipitates observed.

Hg2^+2 + 2Cl^- ==> Hg2Cl2(s)

Fe^+2 + CO3^-2 ==> FeCO3(s)
You should add (aq) after the ions

To write the net ionic equations for the formation of each precipitate, we need to first determine the chemical formulas of the precipitates formed.

Let's analyze each step in the process:

Step 1: Addition of potassium chloride (KCl):
The possible reaction can be between Hg2(2+) and Cl-. The chemical formula of the precipitate formed can be determined by balancing the charges of the ions involved. Since Hg2(2+) has a charge of +2 and Cl- has a charge of -1, we need two chloride ions to balance the charge of one mercury ion:

Hg2(2+) + 2Cl- -> Hg2Cl2 (s)

The net ionic equation for this reaction is:
Hg2(2+) + 2Cl- -> Hg2Cl2 (s)

Step 2: Addition of potassium sulfate (K2SO4):
Since no precipitate forms, we can assume that there is no reaction between the ions present in the solution. Hence, there is no net ionic equation in this step.

Step 3: Addition of potassium carbonate (K2CO3):
The possible reaction can occur between Fe(2+) and CO3(2-). Balancing the charges, we need two Fe(2+) ions to balance one CO3(2-) ion:

Fe(2+) + CO3(2-) -> FeCO3 (s)

The net ionic equation for this reaction is:
Fe(2+) + CO3(2-) -> FeCO3 (s)

Therefore, the net ionic equations for the formation of each precipitate observed are:
1) Hg2(2+) + 2Cl- -> Hg2Cl2 (s)
2) Fe(2+) + CO3(2-) -> FeCO3 (s)