A) \[{{C}_{6}}{{H}_{5}}N{{H}_{2}}\]
B) \[{{({{C}_{2}}{{H}_{5}})}_{2}}NH\]
C) \[{{(C{{H}_{3}})}_{3}}N\]
D) \[{{C}_{6}}{{H}_{5}}NH{{C}_{6}}{{H}_{5}}\]
E) \[{{({{C}_{6}}{{H}_{5}})}_{3}}N{{H}^{+}}C{{l}^{-}}\]
Correct Answer: D
Solution :
\[{{({{C}_{2}}{{H}_{5}})}_{2}}\overset{\bullet \,\bullet }{\mathop{N}}\,H\](\[2{}^\circ \]amine) is strongest base. Basic nature of amines due to presences of lone pair of electron on nitrogen atom which is available for the bond formation with Lewis acid. Due to the + I effect\[2{}^\circ \]amine is better base than\[1{}^\circ \]amine and\[N{{H}_{3}}\]. In case of aromatic amines the lone pair on nitrogen atom involved in resonance, therefore, not available for bond formation, so aromatic amines are less basic.
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