Titration
Titration
Titration (pronounced: /taɪˈtreɪʃən/) is a common laboratory method of quantitative chemical analysis that is used to determine the concentration of an identified analyte.
Etymology
The term "titration" comes from the Latin word titulus, which means "inscription or title". The French word titre, also from this origin, means "rank". Titration, by definition, is the determination of rank or concentration of a solution with respect to water with a pH of 7 (the known solution is usually acidic or basic) that reacts with a reagent of known concentration in a specific and well-defined reaction. The reaction's completion is usually marked by the color change of an indicator substance.
Procedure
A titrant or titrator (a solution of known concentration) is prepared to react with a solution of the analyte to determine concentration. During titration, the titrant is added to the analyte until the reaction is complete. The completion is usually marked by a color change due to an indicator.
Types of Titration
There are several types of titration methods in use. A few of the most common methods include acid-base titration, redox titration, complexometric titration, and precipitation titration.
Related Terms
- End point: The point during a titration when an indicator shows that the amount of reactant necessary for a complete reaction has been added to a solution.
- Equivalence point: The point at which the reactants are mixed in the stoichiometrically correct proportions.
- Indicator: A substance that changes color in response to a chemical change.
- pH: A measure of the acidity or basicity of a solution.
- Molarity: A measure of the concentration of a solute in a solution.
- Standard solution: A solution of known concentration.
External links
- Medical encyclopedia article on Titration
- Wikipedia's article - Titration
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