When an alkaline solution of K₂CrO₄ is treated with 3% H₂O₂ solution, red brown paramagnetic peroxochromate is obtained as per following equation:
$2 K_{2} {CrO}_{4} + 7 H_{2} O_{2} + 2 KOH ⟶ 2 K_{3} {CrO}_{8} + 8 H_{2} O$
The equivalent weight of K₂CrO₄ for above transformation must be (assuming M is the molar mass of K₂CrO₄)

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$\frac{M}{16}$

$\frac{M}{12}$

$\frac{M}{2}$

answer is B.

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Detailed Solution

Oxidation of Cr in K₃CrO₈ = V

${Cr}^{+ 6} ⟶ {Cr}^{+ 5}$

Equivalent mass $= \frac{M}{1}$ ̣

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