A dilute ferrous sulphate solution was gradually added to thebeaker containing acidified permanganate solution. The lightpurple colour of the solution fades and finally disappears.Which of the following is the correct explanation for theobservation?(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 presenceof FeSO4 to a colourless compound.
Question
A dilute ferrous sulphate solution was gradually added to thebeaker containing acidified permanganate solution. The lightpurple colour of the solution fades and finally disappears.Which of the following is the correct explanation for theobservation?(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 presenceof FeSO4 to a colourless compound.
Solution
The correct explanation for the observation is (a) KMnO4 is an oxidising agent, it oxidises FeSO4.
Here's the step by step explanation:
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Potassium permanganate (KMnO4) is a strong oxidising agent. This means it has the ability to gain electrons from other substances in a chemical reaction.
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Ferrous sulphate (FeSO4) is a reducing agent, meaning it can donate electrons in a chemical reaction.
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When the two solutions are mixed, KMnO4 oxidises FeSO4. In this process, KMnO4 gains electrons from FeSO4.
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As KMnO4 is reduced (gains electrons), its purple colour fades and eventually disappears. This is because the MnO4- ion in KMnO4, which is responsible for the purple colour, is reduced to Mn2+ ion, which is colourless.
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Therefore, the disappearance of the purple colour is due to the reduction of KMnO4 as it oxidises FeSO4, not due to dilution or decomposition of KMnO4.
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