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Question: When an alkaline solution of K<sub>2</sub>CrO<sub>4</sub> is treated with 3% H<sub>2</sub>O<sub>2</s...

When an alkaline solution of K2CrO4 is treated with 3% H2O2 solution, red brown paramagnetic peroxochromate is obtained as per following equation.

2K2CrO4 + 7H2O2 + 2KOH ® 2 K3CrO8 + 8 H2O

The equivalent weight of K2CrO4 for above transformation must be (assuming M is the molar mass of K2CrO4)

A

M16\frac{M}{16}

B

M

C

M12\frac{M}{12}

D

M2\frac{M}{2}

Answer

M

Explanation

Solution

Oxidation of Cr in K3CrO8 = V

Cr+6 ® Cr+5

Equivalent mass = M1\frac{M}{1}