Permanganate

A permanganate (p@r'maeNg@neit,_p3r-) is a chemical compound with the manganate(VII) ion, MnO4−, the conjugate base of permanganic acid. Because the manganese atom has a +7 oxidation state, the permanganate(VII) ion is a strong oxidising agent. The ion is a transition metal ion with a tetrahedral structure. Permanganate solutions are purple in colour and are stable in neutral or slightly alkaline media. The exact chemical reaction depends on the carbon-containing reactants present and the oxidant used. For example, trichloroethane (C2H3Cl3) is oxidised by permanganate ions to form carbon dioxide (CO2), manganese dioxide (MnO2), hydrogen ions (H+), and chloride ions (Cl−). 8MnO4- + 3C2H3Cl3 → 6CO2 + 8MnO2 + H+ + 4H2O + 9Cl- In an acidic solution, permanganate(VII) is reduced to the pale pink manganese(II) (Mn2+) with an oxidation state of +2. 8 H+ + MnO4− + 5 e− → Mn2+ + 4 H2O In a strongly basic or alkaline solution, permanganate(VII) is reduced to the green manganate ion, MnO42− with an oxidation state of +6. MnO4− + e− → MnO42− In a neutral solution, however, it gets reduced to the brown manganese dioxide MnO2 with an oxidation state of +4. 2 H2O + MnO4− + 3 e− → MnO2 + 4 OH− Permanganates can be produced by oxidation of manganese compounds such as manganese chloride or manganese sulfate by strong oxidizing agents, for instance, sodium hypochlorite or lead dioxide: 2 MnCl2 + 5 NaClO + 6 NaOH → 2 NaMnO4 + 9 NaCl + 3 H2O 2 MnSO4 + 5 PbO2 + 3 H2SO4 → 2 HMnO4 + 5 PbSO4 + 2 H2O It may also be produced by the disproportionation of manganates, with manganese dioxide as a side-product: 3 Na2MnO4 + 2 H2O → 2 NaMnO4 + MnO2 + 4 NaOH They are produced commercially by electrolysis or air oxidation of alkaline solutions of manganate salts (MnO42−). This is a common and strong disinfectant, used regularly to sanitize baths, toilets, and wash basins, or anything general like that. It is a cheap and extremely effective compound for the task. Permanganates(VII) are salts of permanganic acid.