Pyridine (right) is an essential portion of many biologically active compounds, such as nicotine and vitamin B6. Like ammonia, it has a nitrogen with a lone pair, which makes it act as a weak base. Because it is miscible in a wide range of solvents, from water to benzene, pyridine is one of the most important bases and solvents in organic syntheses. Account for its solubility behaviour in terms of intermolecular forces.

The electromagnetic forces of attraction or repulsion that act between atoms and other types of nearby particles are examples of intermolecular forces, which mediate interactions between molecules, e.g., atoms or ions.

Pyridine is dissolved in water because of the strong dipole-dipole intermolecular interactions (hydrogen bonding) that exist between the lone pair of electrons on N of pyridine and the solvent water molecules.

The structure of pyridine molecules makes it polar. It is a polar yet aprotic solvent as a result. It is fully miscible with a wide range of solvent including water and hexane.

Pyridine is not miscible in benzene because pyridine is polar and benzene is nonpolar, thus benzene is not capable of forming hydrogen bonds