Arrange the following in the order of their b | vedclass

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(C) The basic strength of amines depends on the availability of the lone pair on the nitrogen atom. Electron-withdrawing groups (like $-NO_2$) decreas

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$d > a > b > c$

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(C) The basic strength of amines depends on the availability of the lone pair on the nitrogen atom. Electron-withdrawing groups (like $-NO_2$) decrease basicity by pulling electron density away from the nitrogen atom via inductive $(-I)$ and resonance $(-R)$ effects.$(a)$ Aniline: The lone pair is involved in resonance with the benzene ring.$(b)$ $p$-Nitroaniline: The $-NO_2$ group at the para position exerts a strong $-R$ effect,significantly reducing the basicity compared to aniline.$(c)$ $2,4$-Dinitroaniline: Two $-NO_2$ groups exert a very strong electron-withdrawing effect,making it the least basic.$(d)$ Ammonia $(NH_3)$: It does not have a benzene ring to delocalize the lone pair,making it more basic than the substituted anilines.Therefore,the order of basic strength is: $d > a > b > c$.

Arrange the following in the order of their basic strength:

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