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

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.