In an aqueous dichromate solution, a strict chemical equilibrium exists: . At what approximate analytical value are the yellow chromate and orange dichromate ions universally established to exist in a

Question

In an aqueous dichromate solution, a strict chemical equilibrium exists: $Cr_2O_7^{2-} + H_2O \rightleftharpoons 2CrO_4^{2-} + 2H^+$. At what approximate analytical $pH$ value are the yellow chromate and orange dichromate ions universally established to exist in an exact, balanced equilibrium?

Prashant Kotian · Accepted Answer

Correct answer: B. The interconversion between chromate and dichromate is highly dependent. In acidic media (low ), dichromate is the predominant stable species. In basic media (high ), chromate is predominant. Experimental and thermodynamic data strictly establish that these two specific ions ( and ) exist in a finely balanced equilibrium at a specific of roughly .

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