Like ammonia, amines are bases.[8] Compared to alkali metal hydroxides, amines are weaker (see table for examples of conjugate acid Ka values).
Reference 1: pKa and Kb.
Reference 2: methylamine (MeNH2), dimethylamine (Me2NH), trimethylamine (Me3N), ethylamine (EtNH2), aniline (PhNH2), 4-methoxyaniline (4-MeOC6H4NH2), N,N-Dimethylaniline (PhNMe2), 3-Nitroaniline (3-NO2-C6H4NH2), 4-Nitroaniline (4-NO2-C6H4NH2) and 4-trifluoromethylaniline (CF3C6H4NH2).
Source: http://en.wikipedia.org/wiki/Amine
Reference 2: methylamine (MeNH2), dimethylamine (Me2NH), trimethylamine (Me3N), ethylamine (EtNH2), aniline (PhNH2), 4-methoxyaniline (4-MeOC6H4NH2), N,N-Dimethylaniline (PhNMe2), 3-Nitroaniline (3-NO2-C6H4NH2), 4-Nitroaniline (4-NO2-C6H4NH2) and 4-trifluoromethylaniline (CF3C6H4NH2).
Source: http://en.wikipedia.org/wiki/Amine
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