CrO_4^{2-} (Yellow) changes to Cr_2O_7^{2-} ( | vedclass

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Question

(A) The interconversion between chromate $(CrO_4^{2-})$ and dichromate $(Cr_2O_7^{2-})$ ions is pH-dependent. The equilibrium reaction is: $2CrO_4^{2-

Vedclass · Accepted Answer

$6, 8$

Vedclass · Answer

(A) The interconversion between chromate $(CrO_4^{2-})$ and dichromate $(Cr_2O_7^{2-})$ ions is pH-dependent. The equilibrium reaction is: $2CrO_4^{2-} + 2H^+ \rightleftharpoons Cr_2O_7^{2-} + H_2O$. In acidic medium $(pH In basic medium $(pH > 7)$,the concentration of $H^+$ ions decreases (or $OH^-$ increases),shifting the equilibrium to the left,forming yellow chromate $(CrO_4^{2-})$. Thus,for the conversion of yellow to orange,$pH$ must be acidic ($x  7$,e.g.,$8$). Therefore,$x = 6$ and $y = 8$ is the correct pair.

$CrO_4^{2-}$ (Yellow) changes to $Cr_2O_7^{2-}$ (orange) in $pH = x$ and vice versa in $pH = y$,hence $x$ and $y$ are respectively:

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