Titration

Titration determines an analyte’s concentration by adding a measured amount of reagent until a defined reaction endpoint is reached.

Titrant: A solution of known concentration added to react with an analyte during a titration. Its measured volume and known concentration provide the amount used to calculate the analyte.
Molar concentration: The amount of a substance, in moles, per unit volume of solution. Titration results commonly express analyte concentration in moles per liter.
Acid–base titration: A titration that uses a neutralization reaction between an acid and a base. It measures acid or base concentration through neutralization and a detectable pH change.
Potentiometric titration: A titration that detects its endpoint by measuring electrode potential as titrant is added. It detects endpoints instrumentally when a visual indicator is unreliable or unsuitable.
Equivalence point: The point in a titration where reactants have combined in exact stoichiometric proportions. At this point, reaction stoichiometry relates the titrant amount to the analyte amount.
Burette: A graduated laboratory tube with a valve for dispensing measured volumes of liquid. It delivers titrant in controlled increments and records the volume used.
Redox titration: A titration based on an electron-transfer reaction between an oxidant and a reductant. It quantifies analytes that participate in oxidation–reduction reactions.
Conductometric titration: A titration that tracks changes in electrical conductivity as titrant is added. Conductivity changes can locate endpoints without relying on a color indicator.
Titration endpoint: The observed signal or change used to stop a titration. The endpoint is the practical stopping signal, which should closely match the equivalence point.
Pipette: A laboratory instrument for transferring a measured volume of liquid. A pipette can deliver a known sample volume before titration begins.

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