Which one is more basic: acetamide or aniline? [duplicate]

Which one is more basic: acetamide or aniline?

I had approached the question by protonating both of the compounds. Then I judged them on the basis of the stability of the corresponding conjugate acid.

1. In $\ce{CH3CONH3+}$, due to resonance, a positive charge is created on the oxygen atom. So, resonance is not very effective here. Hence $\ce{ CH3CONH2}$ is not a good base.
2. In $\ce{C6H5NH3+}$, there is far better resonance which takes place.

From the above observations, I concluded that aniline is more basic.

I had another view that $\ce{C6H5NH2}$ is a basic type of compound rather being salt-like as is $\ce{CH3CONH2}$.

Am I going in the right direction to solve the problem?

• No. Acetamide, if it protonates, does so on oxygen. Consider the pKa's of these species or the pKb's of aniline and acetamide (which one can be extracted by aqueous acid from an ether solution of the two?) – user55119 Mar 11 '18 at 16:10
• Also you can consider availability of electron pair on N or O in both bases. Better resonance means lesser electron availability and weaker base.. So it seems O is most basic by that logic. – King Tut Mar 11 '18 at 16:11
• chemistry.stackexchange.com/questions/14017/… – Mithoron Mar 11 '18 at 18:50

In the case of aniline, the phenyl group is not a strong withdrawing group. Still, the phenyl group withdraws electron density from the nitrogen atom through resonance. However, anilines can be protonated by strong acids. You can observe that during the formation of a diazonium salt, where aniline is protonated by strong acids like $\ce{HCl}$.