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? [NCERT Exemplar] (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 the presence of FeSO4 to a colourless compound
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(a) KMnO4 is an oxidising agent, it oxidises FeSO4
Explanation:
Given that the beaker contains acidified permanganate solution. So we infer that the potassium permanaganate is in an acidic medium. So KMnO4 will be a strong oxidising agent here.
When diluted ferrous sulphate is gradually added to the beaker, the light purple colour fades and disappears. This is because the potassium permanganate oxidises ferrous sulphate into ferric sulphate.
2KMnO4 + 8H2SO4 + 10FeSO4 (Ferrous sulphate) → K2SO4 + 5Fe2(SO4)3 (Ferricsulphate) +2MnSO4+8H4O
So statement A is correct.
Please see the attached picture for the chemical equation.
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