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?

K M n O_{4}

is an oxidising agent, and it oxidies

F e S O_{4}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

F e S O_{4}

acts as an oxidising agent and oxidises

K M n O_{4}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

The colour disappear due to dilution; no reaction is involved

No worries! We‘ve got your back. Try BYJU‘S free classes today!

K M n O_{4}

is an unstable compound and decomposes is presence of

F e S O_{4}

to a colourless compound

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $K M n O_{4}$ is an oxidising agent, and it oxidies $F e S O_{4}$
$F e S O_{4} + K M n O_{4}      P u r p l e c o l o u r + H_{2} S O_{4} ⟶ F e_{2} (S O_{4})_{3} + M n S O_{4} + K_{2} S O_{4} + H_{2} O$
$K M n O_{4}$ is an oxidizing agent and oxidizes $F e S O_{4} (F e^{+ 2})$ to $F e_{2} (S O_{4})_{3} (F e^{+ 3})$ .

Suggest Corrections

Similar questions

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.