Ba(NO3)2 is added (BaCrO4 (s) is less soluble than BaCr2O7 (S))

provide an explanation

Thank You

an explanation for what?

2 CrO4 + 2H = Cr2O7 + H2O

Determine the color the solution would turn when each of the following is done to the reaction at equilibrium. provide an explanation for each.
a0 HCl is added (orange)
b) NaOH is added (yellow)
c) Ba(NO3)2 is added (BaCrO4 (s) is less soluble than BaCr2O7 (S)) (yellow)

but I need help provide an explanation
for each.

Thank you

It's all about Le Chatelier's Principle.

Why BaCr207 is less precipitate than BaCrO4

When Ba(NO3)2 is added to a solution, it dissociates into Ba2+ and NO3- ions. On the other hand, BaCrO4 and BaCr2O7 are both insoluble compounds.

BaCrO4 is less soluble than BaCr2O7 because of the solubility rules. The solubility of a compound is determined by the attractions between its ions and the interactions with the solvent molecules.

The solubility rules state that most nitrate (NO3-) compounds are soluble. Therefore, Ba(NO3)2 fully dissociates into Ba2+ and NO3- ions, which remain in the solution.

However, chromate (CrO4^2-) compounds have limited solubility. BaCrO4, being a chromate compound, does not completely dissociate in water. Instead, it forms a precipitate (solid) of BaCrO4, which settles at the bottom of the container.

BaCr2O7, on the other hand, is more soluble because it is a dichromate compound. The structure and properties of dichromate compounds allow for more solubility compared to chromate compounds. When BaCr2O7 is added to a solution, it dissociates partially, forming some Ba2+ and Cr2O7^2- ions in the solution while the remaining compound remains as a precipitate.

In summary, BaCrO4 is less soluble than BaCr2O7 due to the solubility rules and the nature of chromate and dichromate compounds.