titrationer

Titration is a quantitative chemical analysis method used to determine the concentration of an unknown solution by reacting it with a solution of known concentration, called the titrant. The reaction proceeds until the chemical equivalence point is reached, at which the reactants are present in stoichiometric proportions. In practice, the end point is detected by an indicator that changes color, a pH measurement, or another sensor signal.

A typical setup includes a burette to deliver the titrant, a flask containing the analyte solution, and a means to mix the solutions while monitoring the end point. The volume of titrant added at the end point is used, together with the known concentration of the titrant and the stoichiometry of the reaction, to calculate the analyte concentration. The common formula is C_analyte × V_analyte = C_titrant × V_titrant, with adjustments for aliquot volumes as needed.

There are several main types of titration. Acid-base titrations use pH indicators or pH meters to signal the end point. Redox titrations rely on changes in oxidation state and suitable indicators. Complexometric titrations, such as those using EDTA, determine metal ion concentrations. Precipitation titrations involve a reaction that forms a barely soluble product.

Accuracy depends on appropriate endpoint detection, proper standardization of the titrant, and control of experimental conditions. Titrations are widely used in pharmaceutical quality control, environmental and food analysis, and clinical chemistry, providing a reliable method for determining concentrations in a range of matrices.