The oxidation state of chromium in the final | vedclass

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(B) In an acidic medium, potassium dichromate $(K_{2}Cr_{2}O_{7})$ acts as a strong oxidizing agent. When it reacts with potassium iodide $(KI)$, the

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$+3$

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(B) In an acidic medium, potassium dichromate $(K_{2}Cr_{2}O_{7})$ acts as a strong oxidizing agent. When it reacts with potassium iodide $(KI)$, the iodide ions $(I^{-})$ are oxidized to iodine $(I_{2})$, and the chromium in the dichromate ion $(Cr_{2}O_{7}^{2-})$ is reduced to the chromic ion $(Cr^{3+})$. The balanced chemical equation is: $K_{2}Cr_{2}O_{7} + 6KI + 7H_{2}SO_{4} \rightarrow 4K_{2}SO_{4} + Cr_{2}(SO_{4})_{3} + 3I_{2} + 7H_{2}O$. In the product $Cr_{2}(SO_{4})_{3}$, the oxidation state of chromium is $+3$.

The oxidation state of chromium in the final product formed in the reaction between $KI$ and acidified $K_{2}Cr_{2}O_{7}$ solution is:

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