Q. Decreasing order of basic nature in aqueous solutions
A) $C_{6}H_{5}NH_{2} > NH_{3} > CH_{3}NH_{2} > \left( CH_{3} \right)_{2}NH$
B) $NH_{3} > C_{6}H_{5}NH_{2} > CH_{3}NH_{2} > \left( CH_{3} \right)_{2}NH$
C) $\left( CH_{3} \right)_{2}NH > CH_{3}NH_{2} > NH_{3} > C_{6}H_{5}NH_{2}$
D) $CH_{3}NH_{2} > \left( CH_{3} \right)_{2}NH > NH_{3} > C_{6}H_{5}NH_{2}$
Explanation
(c)
Basic nature of an amine depends upon availability of lone pair on nitrogen atom. If lone pair is easily available the compound would be more basic.
Dut to +I effect of methyl group, methyl amine is more basic than ammonia and dimethyl amine is more basic than methyl amine. While aniline is a weaker base than ammonia due to delocalization of lone pair of nitrogen atom at different position.
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.