Permanganate titration

A volumetric analysis method in which permanganate ions oxidize an analyte and indicate the endpoint through their color change.

Redox titration: A volumetric method that determines an analyte through an oxidation–reduction reaction with a titrant. Permanganate titration is a redox titration whose endpoint follows electron transfer.
Iron(II) determination: Quantitative measurement of iron in the +2 oxidation state by chemical analysis. Permanganate oxidizes Fe²⁺ to Fe³⁺ in a common volumetric assay.
Oxidation–reduction reaction: A chemical reaction in which electrons are transferred and oxidation states change. Permanganate consumes reducing equivalents by accepting electrons from the analyte.
Dichromate titration: A redox titration that uses dichromate ions as the oxidizing titrant. Unlike permanganate, dichromate is not usually a self-indicator and needs an endpoint indicator.
Permanganate ion: The purple MnO₄⁻ ion, a strong oxidizing agent that is reduced during many reactions. It is the colored oxidant delivered from the burette.
Oxalate determination: Quantitative measurement of oxalate ions or oxalic acid in a sample. Permanganate oxidizes oxalate to carbon dioxide in a widely taught titration.
Half-reaction method: A procedure for balancing redox equations by balancing oxidation and reduction separately. Balanced half-reactions establish the mole ratio used in calculations.
Iodometric titration: A titration that measures an oxidant by liberating iodine and titrating it with thiosulfate. It uses an indirect iodine endpoint rather than permanganate’s own color.
Nernst equation: An equation relating an electrode potential to the activities of oxidized and reduced species. It describes how changing reaction conditions affect the redox potential near the endpoint.
Chemical oxygen demand: An operational measure of oxygen-equivalent oxidant consumed by substances in a water sample. Permanganate-based methods estimate oxidizable pollution in some water-testing procedures.

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