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