Titraatioita

Titraatioita, known in English as titrations, are a fundamental quantitative chemical analysis technique. The primary goal of a titration is to determine the concentration of a specific substance, known as the analyte, in a solution. This is achieved by reacting the analyte with a solution of precisely known concentration, called the titrant.

The process involves the gradual addition of the titrant to the analyte solution. This addition continues until the reaction between the analyte and titrant is complete. This point of completion is known as the equivalence point. To visually identify the equivalence point, an indicator is often used. Indicators are substances that change color at or very near the equivalence point, signaling that the reaction is complete.

The volume of titrant added to reach the equivalence point is carefully measured. Using the known concentration of the titrant and the volume added, along with the stoichiometry of the reaction between the analyte and titrant, the concentration of the analyte can be calculated. Titrations are widely used in various fields, including chemistry, medicine, and environmental science, for their accuracy and reliability. Common types of titrations include acid-base titrations, redox titrations, and complexometric titrations, each employing different types of chemical reactions.