Applying Le Chateliers principle, what can you conclude about the change 2CrO_4^(-2) -> Cr_2O_7^(-2) and its dependence on hydrogen ions, H^+?

1 Answer

Adding more hydrogen ions would favour the formation of Cr_2O_7^(-2)

Removing hydrogen ions would favour the formation of CrO_4^(-2)

Explanation:

The net ionic equation is:

2CrO_4^(-2) + "2H"^"+"⇌ Cr_2O_7^(-2) + "H"_2"O"

There are 2 H^+ ions on the LHS and none on the RHS.

Based on Le Chateliers Principle;

Adding more hydrogen ions (making conditions more acidic) would favour the formation of Cr_2O_7^(-2) because the equilibrium would shift to the side with fewer hydrogen ions to balance the system.

Removing hydrogen ions (making conditions more basic) would favour the formation of CrO_4^(-2) because the equilibrium would shift to the side with more hydrogen ions to balance the system.