Redokstitratsioone

Redokstitratsioone, also known as redox titrations, are a type of quantitative chemical analysis used to determine the concentration of an unknown substance by reacting it with a solution of known concentration. This reaction involves the transfer of electrons between the analyte (the substance being analyzed) and the titrant (the solution of known concentration). Oxidation, the loss of electrons, and reduction, the gain of electrons, occur simultaneously in a redox reaction.

In a typical redox titration, the titrant is added gradually to the analyte until the reaction is complete. The endpoint of the titration, where the reaction is considered finished, is usually indicated by a visual change, such as a color change, or by using an electrochemical method like potentiometry. Common indicators used in redox titrations change color at a specific potential, signaling the equivalence point where the moles of oxidant are stoichiometrically equivalent to the moles of reductant.

The principle behind redox titrations lies in the predictable nature of redox reactions and the use of standard solutions with known concentrations. By carefully measuring the volume of titrant required to reach the endpoint, the concentration of the analyte can be calculated using stoichiometry. These titrations are valuable tools in various fields, including environmental monitoring, pharmaceuticals, and industrial quality control, for determining the concentration of species like iron, iodine, or oxidizing agents.