Titration

Titration is a quantitative chemical analysis method used to determine the concentration of an unknown solution by slowly adding a solution of known concentration, the titrant, until the reaction reaches a defined endpoint. The process relies on a predictable stoichiometric reaction between the analyte and the titrant.

In a typical setup, the analyte is placed in a flask and the titrant is delivered from a burette. A colorimetric indicator or a pH/voltage sensor signals the endpoint, which is the point at which the reaction has occurred in a way that corresponds closely to the equivalence point, where the reacting species are present in their stoichiometric proportions. The measured titrant volume, combined with its known concentration, allows calculation of the analyte’s concentration.

Common types include acid–base titrations, redox titrations, and complexometric titrations. For simple monoprotic acid–base reactions, the relationship M_A V_A = M_B V_B applies, reflecting stoichiometry between the two reactants. Indicators such as phenolphthalein or methyl orange provide a visible end point that approximates the equivalence point; in instrumental titrations, a pH meter or other detector can be used for higher precision.

Applications span chemical standardization, pharmaceutical quality control, environmental testing, and food analysis. Accuracy depends on proper technique, appropriate indicator choice, calibration of equipment, and accounting for titration errors and sample preparation.