Titrimetric Titration

Titrimetric methods of analysis provide quick and easy analyte determinations with high accuracy and precision. It is based on the chemical reaction between the analyte, or known as titrand and a reagent, the titrant: aA + tT products where A and T represent the analyte and titrant, respectively, and a and t are the stoichiometric coefficients.

This type of reaction gives us with a simple means to classify titrimetry into the following four categories: acid–base titrations, in which an acidic or basic titrant reacts with a titrand that is a base or an acid; complexometric titrations based on metal–ligand complexation; redox titrations, where the titrant is an oxidizing or reducing agent; and precipitation titrations, in which the reaction

The stoichiometric mixture is referred to as equivalence point. The product of the equivalence point volume, Veq, and the titrant’s concentration, CT, gives the moles of titrant reacting with the analyte. Moles of analyte can be calculated after finding out the stoichiometry of the titration reaction(s).

Sadly, there is no obvious indication that the equivalence point has been reached most of the time and we stop adding titrant when end point is reached where there will be some colour changes of a substance added to the solution containing the analyte. The substances are known as indicators. The difference between the end point volume and the equivalence point volume is known as titration error. If the differences between the end point and equivalence point volumes is small, then the titration error is insignificant and can be safely ignored.

Units of Concentration of Standard Solutions

The concentration of standard solutions (titrants) are basically expressed in units of either molarity (CM, or M) or normality (CN, or N).

Molarity (M) – is the number of moles of a material per liter of