Write the correct equation for the formation of a white precipitate on mixing together 10 mL each of 1 M calcium chloride, 1 M calcium bromide, 1 M calcium nitrate, 1 M sodium carbonate, 1 M potassium carbonate, and 1 M rubidium carbonate.

The net ionic equation is as follows:

Ca^2+(aq) + CO3^2-(aq) ==> CaCO3(s)

You can use that to write the molecular equations.

To determine the correct equation for the formation of a white precipitate, we need to consider the possible reactions that can occur between the given compounds. In this case, we have three calcium salts (chloride, bromide, and nitrate) and three carbonate salts (sodium carbonate, potassium carbonate, and rubidium carbonate).

Calcium salts generally react with carbonate salts to form insoluble calcium carbonate precipitate. The balanced equation for this reaction is:

Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)

Now, let's examine the possible reactions one by one:

1. Calcium chloride (CaCl2) + Sodium carbonate (Na2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
This reaction will form white precipitate calcium carbonate, but there are no chloride ions left, so it is not the complete equation.

2. Calcium bromide (CaBr2) + Sodium carbonate (Na2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
Similarly, this reaction also forms white precipitate calcium carbonate, but there are no bromide ions left, so it is not the full equation.

3. Calcium nitrate (Ca(NO3)2) + Sodium carbonate (Na2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
Again, this reaction produces calcium carbonate precipitate, but there are no nitrate ions left, so it is not the complete equation.

4. Calcium chloride (CaCl2) + Potassium carbonate (K2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
This reaction also forms white precipitate calcium carbonate, and there are no chloride ions or potassium ions left. However, the equation is still incomplete.

5. Calcium bromide (CaBr2) + Potassium carbonate (K2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
Similar to the previous equations, this reaction yields calcium carbonate as the white precipitate, but there are no bromide ions or potassium ions left. The equation is still not complete.

6. Calcium nitrate (Ca(NO3)2) + Potassium carbonate (K2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
Once again, this reaction will produce white precipitate calcium carbonate, but there are no nitrate ions or potassium ions left. The equation is still not the full equation.

7. Calcium chloride (CaCl2) + Rubidium carbonate (Rb2CO3):
Ca2+ (aq) + CO32- (aq) ⟶ CaCO3 (s)
Finally, this reaction forms white precipitate calcium carbonate, and there are no chloride ions or rubidium ions left. This is the complete equation!

Therefore, the correct equation for the formation of a white precipitate on mixing the given compounds is:

CaCl2 (aq) + Rb2CO3 (aq) ⟶ CaCO3 (s) + 2RbCl (aq)

Please note that this reaction assumes that all compounds are fully dissociated in water, and any spectator ions (ions that do not participate in the reaction) are not shown.