Question about chromate-dichromate equilibrium?

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Adding HCl to a chromate solution shifts the equilibrium to produce dichromate, resulting in an orange color due to the excess hydrogen ions. When HCl is added to a dichromate solution, the color change is similar, raising questions about the underlying chemistry. The equilibrium equation provided, 2[CrO4]^-2 + [H]+ <--> [Cr2O7]^-2 + H2O, is correct. Dissolving dichromate in pure water would not produce the same color change, indicating the role of hydrogen ions in the reaction. Understanding these dynamics is crucial for explaining the observed color changes in different conditions.
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Ok so when i add HCl to a chromate solution, it turns orange (dichromate) because the equilibrium shifts to the right, inorder to reduce the excess hydrogen ions from the HCl Acid.

But when I add HCl to dichromate, the color changes the same. How do i explain this phenomenon.

and is this the right equation?


2[CrO4]-2 + [H]+ <---> [Cr2O7]-2 + H2O
 
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Equation is OK.

Take a look at it - what would you expect if you dissolve dichromate in pure water?
 
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