Compounds containing Nitrogen

Statement I:
CH3NH2 is more basic than NH3 but C6H5NH2 is less basic than NH3.
Explanation:
Methylamine (CH3NH2) :
The −CH3 group is electron donating ( + I effect), which increases the electron density on nitrogen, making it more basic than ammonia.
Aniline ( C6H5NH2 ):
The lone pair on nitrogen gets delocalized into the benzene ring through resonance, reducing its availability to accept a proton.
So aniline is less basic than ammonia.
Hence, Statement I is correct.

Statement II:
The order of basic strength of amines in aqueous phase follows the order
(C2H5)3N>(C2H5)2NH>C2H5NH2.
Let's check this:
In the aqueous phase, basic strength is influenced by two factors:
+ I effect (electron donating alkyl groups increase basicity)
Solvation effect (stabilization of the conjugate ammonium ion)
In aqueous solution, the solvation effect is strong for primary > secondary > tertiary amines, because primary amines can form more hydrogen bonds.
However, the +1 effect increases as we move from primary ⟶ secondary ⟶ tertiary.
The combined effect in aqueous phase gives the observed order:
Secondary amine > Primary amine > Tertiary amine
That is:
(C2H5)2NH>C2H5NH2>(C2H5)3N
But the statement says the order is:
(C2H5)3N>(C2H5)2NH>C2H5NH2
This is incorrect in aqueous medium.