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

K M n O_{4}

is an oxidizing agent, it oxidizes

F e S O_{4}

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F e S O_{4}

acts as an oxidizing agent and oxidizes

K M n O_{4}

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The colour disappears due to dilution: no reaction is involved

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K M n O_{4}

is an unstable compound and decomposes in presence of

F e S O_{4}

to a colourless compound

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Solution

The correct option is A $K M n O_{4}$ is an oxidizing agent, it oxidizes $F e S O_{4}$
$K M n O_{4}$ is a strong oxidizing agent. It oxidizes $F e S O_{4}$ and itself is reduced to $M n S O_{4}$ .
$K M n O_{4}$ is purple in color whereas $M n S O_{4}$ is colorless.
$2 K M n O_{4} + 8 H_{2} S O_{4} + 10 F e S O_{4} \to K_{2} S O_{4} + 2 M n S O_{4} + 5 F e_{2} (S O_{4})_{3} + 8 H_{2} O$

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Question 6

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

Which of the following is the correct explanation for the observation?

(a) ${KMnO}_{4}$ is an oxidizing agent, it oxidises ${FeSO}_{4}$ .
(b) ${FeSO}_{4}$ acts as an oxidizing agent and oxidises ${KMnO}_{4}$ .
(c) The colour disappears due to dilution; no reaction is involved.
(d) ${KMnO}_{4}$ is an unstable compound and decomposes in presence of ${FeSO}_{4}$ to a colourless compound.