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Titration

Last updated

Jun 23, 2019
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- Chromatography I: TLC
- Acid-Base Titrations

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Titration is the slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization, which is often indicated by a color change. The solution called the titrant must satisfy the necessary requirements to be a primary or secondary standard. In a broad sense, titration is a technique to determine the concentration of an unknown solution.

Topic hierarchy

Acid-Base Titrations
Complexation Titration
Precipitation Titration
Redox Titration
Titration of a Strong Acid With A Strong Base
Titration of a strong acid with a strong base is the simplest of the four types of titrations as it involves a strong acid and strong base that completely dissociate in water, thereby resulting in a strong acid-strong base neutralization reaction. This titration requires the use of a buret to dispense a strong base into a container of strong acid, or vice-versa, in order to determine the equivalence point.
Titration of a Weak Acid with a Strong Base
A titration is a controlled chemical reaction between two different solutions.
Titration of a Weak Base with a Strong Acid
Data obtained through the process of titration can be used to compute the molarity and the correlated acidity of a solution at various times of the titration. The initial and final volumes of the analyte and titrant solutions, as well as the pH, or measure of acidity, are essential in calculating the total number of moles of analyte present. Once this information is determined, the molarity of the analyte can then be computed, because its volume was measured beforehand.
Titration of a Weak Polyprotic Acid
A weak polyprotic acid is an acid that is usually considered as weak acid in its monoprotic form (only one $H^+$ in the molecule), but instead has more than one H+ in the molecule, therefore making it a polyprotic acid.

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