titrer

Titrer is a chemical analytical technique used to determine the concentration of an analyte in a solution by adding a reagent of known concentration, known as the titrant, until the reaction reaches its endpoint. The process is commonly described in English as titration, and the term titrer refers to the action of performing this procedure.

In a typical titration, a burette delivers the titrant into a known volume of the analyte, often contained in an Erlenmeyer flask. The volume of titrant added at the endpoint is recorded, and the endpoint is identified either by an observable change, such as a color shift produced by an indicator, or by instrumentation, such as a pH meter or potentiometric sensor. The equivalence point, where the quantities of titrant and analyte react according to their stoichiometry, defines the true end point of the reaction.

There are several classes of titration, including acid–base, redox, complexometric, and precipitation titrations. Each class uses a suitable indicator or sensor to signal the endpoint. Common indicators include phenolphthalein and methyl orange for acid–base titrations, while modern methods may rely on potentiometric or conductometric measurements.

Calculations from titration data determine the analyte’s concentration. With known titrant concentration and measured volumes, the relationship is governed by stoichiometry: the amount (in moles) of analyte equals the amount of titrant multiplied by the stoichiometric coefficient. Titration is widely used in chemistry and related fields for quality control, pharmaceutical analysis, environmental testing, and research.

Limitations include potential side reactions, incomplete reactions, and the need for accurate standard solutions and careful endpoint estimation to ensure reliable results.