12.53 ml of 0.0509 M SeO 2 reacted with 25.52 ml 0.1 M CrSO 4 solution. In the reaction Cr 2 + was oxidized to Cr 3 + . To what oxidation state selenium was converted in the reaction?

Question

12.53 ml of 0.0509 M SeO 2 ​ reacted with 25.52 ml 0.1 M CrSO 4 ​ solution. In the reaction Cr 2 + was oxidized to Cr 3 + . To what oxidation state selenium was converted in the reaction?

TestHub · Accepted Answer

Moles Cr²⁺ = 25.52 m l × 0.1 M = 2.552 mm o l . Moles SeO₂ = 12.53 m l × 0.0509 M = 0.6378 mm o l . Cr²⁺ loses 1 e⁻. Total e⁻ lost = 2.552 mm o l . Each SeO₂ gains 2.552/0.6378 ≈ 4 e⁻. Initial Se oxidation state in SeO₂ is +4. Final Se oxidation state = 4 − 4 = 0 .

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