Given are cyclohexanol (I),acetic acid (II),2 | vedclass

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(A) The acidic strength depends on the stability of the conjugate base formed after the loss of a proton $(H^+)$.$2,4,6-$trinitrophenol $(III)$ is the

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$III > II > IV > I$

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(A) The acidic strength depends on the stability of the conjugate base formed after the loss of a proton $(H^+)$.$2,4,6-$trinitrophenol $(III)$ is the most acidic because the phenoxide ion is highly stabilized by the strong $-I$ and $-M$ effects of three $-NO_2$ groups.Acetic acid $(II)$ is more acidic than phenol $(IV)$ because the carboxylate ion is stabilized by resonance between two electronegative oxygen atoms,whereas the phenoxide ion is stabilized by resonance within the aromatic ring.Phenol $(IV)$ is more acidic than cyclohexanol $(I)$ because the phenoxide ion is resonance-stabilized,while the cyclohexoxide ion has no such stabilization.Cyclohexanol $(I)$ is the least acidic as the alkyl group is electron-donating ($+I$ effect),which destabilizes the alkoxide ion.Therefore,the order of decreasing acidic strength is $III > II > IV > I$.

Given are cyclohexanol $(I)$,acetic acid $(II)$,$2,4,6-$trinitrophenol $(III)$ and phenol $(IV)$. The order of decreasing acidic character is:

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