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Potassium permanganate is prepared from pyrolusite (MnO2). Pyrolusite is fused with KOH in the presence of atmospheric oxygen or an oxidising agent like potassium nitrate or potassium chlorate to give potassium manganate, K2MnO4. The green mass is taken out with water and oxidized to potassium permanganate, electrolytically or by passing chlorine or ozone into solution. Electrolytic oxidation K2MnO4 2K+ + MnO42- H2O H+ + OH- During electrolysis manganate ions are oxidized to permanganate at anode At cathode hydrogen gas is liberated 2H2O + 2e- H2 + 2OH- Oxidation by chlorine 2K2MnO4 + Cl2 2KMnO4 + 2KCl Or, 2MnO42- + Cl2 2MnO4- + 2Cl Oxidation by ozone 2K2MnO4 + O3 + H2O 2KMnO4 + 2KOH + O2 Or, 2MnO42- + O3 + H2O 2MnO42- + 2OH- + O2 As a result of oxidation, the green colour of solution changes into purple. The purple solution containing KMnO4 is concentrated by evaporation which on cooling gives crystals of KMnO4. The manganate (MnO42-) and permanganate (MnO2-) ions are tetrahedral in shape. The manganate is paramagnetic with one unpaired electron but the permanganate is diamagnetic. The π-bonding takes place by overlie of p-orbitals of oxygen with d-orbitals of manganese. Properties Potassium permanganate is violet crystalline solid having m.p. 523 K. it is soluble in water and its aqueous solution is purple in colour. Result of heat: on heating, potassium permanganate changes into manganate and oxygen gas is evolved. 2KMnO4 K2MnO4 + MnO2 + O2 Effect of alkalies: on heating with alkalies, potassium permanganate converts into manganate and oxygen gas is evolved. 4KMnO4 + 4KOH 4K2MnO4 + 2H2O + O2 Oxidising properties: KMnO4 acts as a very powerful oxidising agent in acidic, neutral and alkaline media. The equations representing oxidation in these media are given below: In acidic medium 2KMnO4 + 3H2SO4 K2SO4 + 2MnSO4 + 3H2O + 5[O] Or, MnO4- + 8H+ + 5e- Mn2+ + 4H2O [ = + 1.52 V] In neutral or alkaline medium 2KMnO4 + H2O 2KOH + 2MnO2 + 3[O] Or, MnO4- + 2H2O + 3e- MnO2 + 4OH- [ = + 1.23 V]
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