Titrimetrisch

Titrimetrisch, or titrimetry, is a quantitative chemical analysis method in which the concentration of an analyte is determined by reacting it with a solution of known concentration (the titrant) and measuring the volume required to reach a defined endpoint. The fundamental principle is a stoichiometric reaction between analyte and titrant; knowing the reaction's stoichiometry and the titrant's concentration yields the analyte concentration. In Dutch, the term titrimetrisch is used for this approach, while in English it is commonly called titrimetry.

Typical equipment includes a burette to dispense the titrant and a vessel containing the sample (analyte). The endpoint is detected by an indicator that changes color, or by instrument-based measurements such as a pH meter, a conductivity meter, or a voltammetric/readout that signals the equivalence point. Accurate titration requires a properly standardized titrant solution and careful determination of the endpoint to minimize errors.

Common titrimetry methods are acid-base titrimetry (neutralization), redox titrimetry (oxidation-reduction), complexometric titrimetry (for example, with EDTA to determine metal contents), and argentometric/titrimetry (precipitation-based methods using silver ions).

Endpoint versus equivalence point: the theoretical point at which reaction is complete (equivalence) and the observed signal at endpoint. Methods include instrumental endpoints (pH or potential) and visual indicators. Calibration and standardization of titrants are crucial for accuracy.

Applications span pharmaceutical QC, environmental analysis, food chemistry, and research. Advantages include high accuracy and relative simplicity; limitations involve selectivity, potential side reactions, and reliance on stable standards. Titrimetry remains a foundational technique in analytical chemistry.