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The oxidation states for the half-reaction involving the permanganate ion show that manganese is reduced.
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Permanganate ions are reduced to manganese(II) ions.
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Molecular model of permanganate ion, MnO42.
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The sulphur dioxide is recognizable by its smell and by its reducing properties in respect, for example, of permanganate ions.
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The half-reaction shown for permanganate ion occurs only in solutions that are 0.1 M or greater in strong acid.
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By contrast, the univalent anions perchlorate and permanganate ions are very difficult to protonate and so the corresponding acids are strong acids.
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Manganese(VII) chemistry is dominated by the manganate(VII) ion (permanganate).
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The oxidation of chloride ion to chlorine by permanganate at room temperature is normally slow.
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The first oxidising agent in the reaction is the permanganate ions.
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A difficulty arises when permanganate titrations of iron(II) are performed in the presence of chloride ion.
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The kinetics of the reaction is complex, and the manganese(II) ions formed catalyze the further reaction between permanganate and oxalic acid (formed in situ by the addition of excess sulfuric acid).
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An instance of ion-pair extraction is in the use of a ligand to enable oxidation by potassium permanganate, KMnO4, in an organic solvent.
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With the alkaline method, the chloride ions are not oxidized by potassium permanganate, so COD can be measured without the interference effect of the chloride ions.
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One explanation is that the mixture contains both the purple permanganate (MnO4–) and the green manganate ions (MnO42–), which combine to produce a blue solution.
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