A dilute ferrous sulphate solution was gradually added to the beaker containing acidified potassium permanganate solution. The light purple colour of the solution fades and fin

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Solution

Q.
A dilute ferrous sulphate solution was gradually added to the beaker containing acidified potassium permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation

1 $K M n O_{4}$ is an oxidising agent, it oxidises $F e S O_{4}$ .

2 $F e S O_{4}$ acts as an oxidising agent and oxidises $K M n O_{4}$

3 The colour disappears due to dilution; no reaction is involved

4 $K M n O_{4}$ is an unstable compound and decomposes in presence of $F e S O_{4}$ to a colourless compound

Ans.
(1)

In this reaction, potassium permanganate $(K M n O_{4})$ is an oxidising agent. It oxidises ferrous sulphate to ferric sulphate in the presence of dilute $H_{2} S O_{4}$

$2 K M n O_{4} + 10 F e S O_{4} + 8 H_{2} S O_{4} \to K_{2} S O_{4} + 2 M n S O_{4} + 5 F e_{2} {(S O_{4})}_{3} + 8 H_{2} O$

The solution is coloured purple because of the KMnO?, and it eventually disappears when all the KMnO? in the solution is used.:

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