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Oxidizing Nature of Sulphuric Acid

25 mL of a so...

Question

$25$ mL of a solution containing ferrous sulphate and ferric sulphate, acidified with $H_{2} S O_{4}$ is reduced by metallic zinc. The solution requires $34.25$ mL of $0.1 N$ solution of $K_{2} C r_{2} O_{7}$ for oxidation. However, before reduction with zinc, $25$ mL of same solution requires $22.45$ mL of same $K_{2} C r_{2} O_{7}$ . Calculate the weight of $F e_{2} (S O_{4})_{3}$ present in gram per litre of the solution (in nearest integer).

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Solution

Potassium dichromate oxidizes ferrous sulphate to ferric sulphate. It has no impact on ferric sulphate. However, zinc reduces ferric sulphate to ferrous sulphate.

The normality of ferrous sulphate before reduction $= \frac{22.45 \times 0.1}{25} = 0.0898 N$

The normality of ferrous sulphate after reduction $= \frac{34.25 \times 0.1}{25} = 0.137 N$

The normality of mixture of ferrous sulphate and ferric sulphate is $0.137 N$ .

Amount of ferrous sulphate in mixture $= 0.0898 \times 152 = 13.6496 g / L$

The normality of ferric sulphate $= 0.137 - 0.0898 = 0.0472 N$

The amount of ferric sulphate in mixture $= 200 \times 0.0472 = 9.44 g / L$

Thus, the nearest integer is $9$ .

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