A dilute ferrous sulphate solution was gradually added to a beaker containing acidified potassium permanganate solution. The light purple colour of the solution faded and finally disappeared. Which of the following is the correct explanation for the observation?
Question
A dilute ferrous sulphate solution was gradually added to a beaker containing acidified potassium permanganate solution. The light purple colour of the solution faded and finally disappeared. Which of the following is the correct explanation for the observation?
Solution
The observation can be explained by a redox reaction that occurs between potassium permanganate and ferrous sulphate. In this reaction, potassium permanganate (KMnO4) acts as an oxidizing agent and gets reduced to manganese dioxide (MnO2), which is colorless. On the other hand, ferrous sulphate (FeSO4) gets oxidized to ferric sulphate (Fe2(SO4)3).
The reaction can be represented as follows:
5FeSO4 + 2KMnO4 + 3H2SO4 → 5Fe2(SO4)3 + K2SO4 + 2MnSO4 + 8H2O
The light purple color of the potassium permanganate solution fades and finally disappears because the MnO4- ions (which give the solution its purple color) are reduced to MnO2, which is colorless. This indicates that all the MnO4- ions have been reduced and the reaction is complete.
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