Redox titration

A quantitative analysis in which an oxidizing or reducing titrant reacts with an analyte through electron transfer. The equivalence point is determined from the reaction’s stoichiometry.

Oxidation–reduction reaction: A chemical reaction in which electrons move between species, changing their oxidation states. Electron transfer between titrant and analyte is the defining reaction.
Permanganate titration: A redox titration using permanganate ion as the oxidizing titrant. Permanganate often serves as its own color indicator in acidic titrations.
Oxidation state: A bookkeeping value assigned to an atom to track electron distribution in compounds and ions. Changes in oxidation state identify the electron transfer being measured.
Acid–base titration: A quantitative analysis in which an acid reacts with a base and the endpoint reflects neutralization. It relies on proton transfer rather than the electron transfer defining this method.
Equivalence point: The point in a titration at which reactants have combined in their stoichiometric proportions. Its location marks the amount of titrant needed to react with the analyte.
Dichromate titration: A redox titration that uses dichromate ion as an oxidizing agent. Dichromate provides a stable oxidant for measuring reducing substances.
Half-reaction: An equation showing either oxidation or reduction separately, including electrons explicitly. Balancing paired half-reactions establishes the titration’s electron stoichiometry.
Complexometric titration: A titration in which a metal ion reacts with a ligand to form a complex. Its measured reaction is complex formation, not oxidation or reduction.
Redox indicator: A substance whose oxidized and reduced forms have different colors, signaling a change in solution redox conditions. A color change can reveal when the titration passes its endpoint.
Iodometry: An analytical method that measures an oxidant by releasing iodine and titrating it with thiosulfate. It converts many oxidizing analytes into measurable iodine.

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