Titration Fundamentals and Methods

Titration purpose in quantitative analysis

In quantitative chemical analysis, titration (titrimetry/volumetric analysis) is used to determine the concentration of an analyte by reacting it with a titrant (a standard solution of known concentration). The titrant is added from a calibrated device (e.g., burette) in measured volumes until the reaction reaches a defined endpoint, which corresponds to the stoichiometric balance between titrant and analyte. The key measured quantity is the titration volume, which—together with the known titrant concentration and reaction stoichiometry—allows calculation of the analyte concentration. The purpose of titration is therefore to convert a chemical reaction into a quantitative measurement: by monitoring when the reaction is complete (endpoint/equivalence point) and recording how much titrant was required, analysts can accurately quantify unknown concentrations. Different titration types (acid–base, redox, complexometric, gas phase, etc.) use different reaction mechanisms and endpoint-detection methods (indicators, pH meters, potentiometers, conductivity, spectroscopy, precipitation cues, calorimetry), but all serve the same quantitative goal—determining analyte concentration from controlled, measured volumes of a standard reagent.

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History and etymology of titration

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