Titratie in niet-waterige oplosmiddelen

The acid–base titrations occurring in the non-aqueous solvent are explained by the Bronsted–Lowry theory, where an acid behaves as a proton donor, and the base is the proton acceptor.

Most acid–base titrations are performed in an aqueous medium. Here, water competes with weaker acids or bases dissolved for proton donation or acceptance. This interference of water results in poor endpoints, necessitating the use of a non-aqueous solvent instead.

Non-aqueous solvents are also suitable for weak acids or bases that partially ionize in water. However, a non-aqueous solvent like ammonia, a stronger base than water, drives greater ionization, making acetic acid a strong acid in ammonia.

Non-aqueous solvents with a lower dissociation constant than water increase the pH [p-H] change at the equivalence point, giving a satisfactory endpoint in the titration curve of weak acids or bases.

Non-aqueous solvents are used in titrating organic analytes, which have poor solubility in water. There are four types of non-aqueous solvents: aprotic, protophilic, protogenic, and amphoteric.