Question

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) ${\text{KMnO}}_4$ is an oxidizing agent, it oxidises ${\text{FeSO}}_4$.
(b) ${\text{FeSO}}_4$ acts as an oxidizing agent and oxidises ${\text{KMnO}}_4$.
(c) The colour disappears due to dilution; no reaction is involved.
(d) ${\text{KMnO}}_4$ is an unstable compound and decomposes in presence of ${\text{FeSO}}_4$ to a colourless compound.

Answer 1

Option (a) is correct.

Potassium permanganate $\left({\text{KMnO}}_4\right)$ in presence of dil. ${\text{H}}_2{\text{SO}}_4$ acts as a strong oxidizing agent and oxidises ferrous sulphate to ferric sulphate. Hence, the purple colour fades and finally disappears.