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- KMnO4 is an oxidising agent- it oxidises FeSO4 -b- FeSO4 acts as an oxidising agent and oxidises KMnO4 -c- The colour disappears due to dilution- no reaction is involved -d- KMnO4 is an unstable compound and decomposes in presence of FeSO4 to a colourless compound-

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Byju's Answer

Standard X

Chemistry

Redox Reaction

A dilute ferr...

Question

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) KMnO₄ is an oxidising agent, it oxidises FeSO₄

(b) FeSO₄acts as an oxidising agent and oxidises KMnO₄

(c) The colour disappears due to dilution; no reaction is involved

(d) KMnO₄ is an unstable compound and decomposes in presence of FeSO₄ to a colourless compound.

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Solution

The answer is A
KMnO4 itself gets reduced and oxidises Fe
oxidation no. of Mn goes from +7 to +2 (reduces), and that of Fe changes from +2 to +3 (Oxidises)

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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.