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 $F e S O_{4}$
$F e S O_{4}$ acts as an oxidising agent and oxidises $K M n O_{4}$
The colour disappear due to dilution; no reaction is involved
$K M n O_{4}$ is an unstable compound and decomposes is presence of $F e S O_{4}$ to a colourless compound

Question

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 $F e S O_{4}$
$F e S O_{4}$ acts as an oxidising agent and oxidises $K M n O_{4}$
The colour disappear due to dilution; no reaction is involved
$K M n O_{4}$ is an unstable compound and decomposes is presence of $F e S O_{4}$ to a colourless compound

Toppr Admin · Accepted Answer

FeSO4-KMnO4-xE152-xE154-xE154-xE154-xE151-xE150-xE154-xE154-xE154-xE153-Purplecolour-H2SO4-x27F6-Fe2-SO4-3-MnSO4-K2SO4-H2OKMnO4 is an oxidizing agent and oxidizes FeSO4-Fe-2-xA0- to Fe2-SO4-3-Fe-3-

FeSO4+KMnO4Purplecolour+H2SO4⟶Fe2(SO4)3+MnSO4+K2SO4+H2OKMnO4 is an oxidizing agent and oxidizes FeSO4(Fe+2) to Fe2(SO4)3(Fe+3).

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