Search results
Aniline is substantially less basic than methylamine, as is evident by looking at the pK a values for their respective ammonium conjugate acids (remember that the lower the pKa of the conjugate acid, the weaker the base).
- Amines as Nucleophiles
The reaction of aldehydes and ketones with ammonia or...
- 25.9 Amines as Bases
Indeed, aniline is a weaker base than cyclohexyl amine by...
- Amines as Nucleophiles
According to Lewis theory, the species which easily loses a pair of electron is Lewis base, Since, ammonia can lose easily electron pair while aniline cannot, thus ammonia is a stronger base than aniline.
Indeed, aniline is a weaker base than cyclohexyl amine by roughly a million fold, the same factor by which phenol is a stronger acid than cyclohexanol. This electron pair delocalization is accompanied by a degree of rehybridization of the amino nitrogen atom, but the electron pair delocalization is probably the major factor in the reduced ...
It explains why phenylamine is a weaker base than other primary amines, and summarises its reactions with acyl chlorides (acid chlorides), acid anhydrides and halogenoalkanes (haloalkanes or alkyl halides).
Aniline is a weak base. Aromatic amines such as aniline are, in general, much weaker bases than aliphatic amines. Aniline reacts with strong acids to form the anilinium (or phenylammonium) ion (C 6 H 5 −NH + 3). [20]
Amines are usually stronger bases than ammonia. (There are exceptions to this, though - particularly if the amine group is attached directly to a benzene ring.) Note: If you want to explore some of the reasons for the relative strengths of ammonia and the amines as bases you could follow this link.
Basicity of Aniline. Aniline is substantially less basic than methylamine, as is evident by looking at the pK a values for their respective ammonium conjugate acids (remember that the lower the pKa of the conjugate acid, the weaker the base).
