Titrausten

Titrausten, commonly rendered in English as titrations, are a family of analytical techniques used to determine the concentration of an unknown solution by reacting it with a solution of known concentration (the titrant). The process is performed in a controlled way, often in a laboratory, and relies on stoichiometric relationships between the reacting species.

A typical titration uses a burette to deliver the titrant into the analyte in a flask, with an indicator or an instrumental signal to detect the endpoint. The endpoint is the observed point at which the reaction has progressed to completion; the equivalence point is the theoretical point where the reactants have reacted in exact stoichiometric proportions. Indicators change color at the endpoint; alternatively pH meters, conductometers, or potentiometric sensors can monitor the signal.

Common types include acid–base titration, redox titration, complexometric titration (for example with EDTA), precipitation titration, and coulometric titration. Each type uses a suitable indicator or sensor and a defined reaction stoichiometry.

Calculation in a simple case follows the relation C_a V_a = C_t V_t at the equivalence point, where C and V refer to the analyte and titrant, respectively. In practice, the endpoint may differ from the ideal equivalence point, requiring calibration or correction.

Applications span pharmaceutical analysis, environmental monitoring, food science, and clinical chemistry. Titrausten require careful standardization of the titrant, attention to temperature, and consideration of side reactions and impurities in the sample. The method became a foundational tool in quantitative chemistry during the 19th century as volumetric analysis developed.