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(D) The acidic strength of these species depends on the stability of the conjugate base (the corresponding amine). The more stable the conjugate base,

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$IV > I > II > III$

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(D) The acidic strength of these species depends on the stability of the conjugate base (the corresponding amine). The more stable the conjugate base,the stronger the acid.$(I)$ $CH_3NH_3^+$: Conjugate base is $CH_3NH_2$ (methylamine).$(II)$ $C_6H_5NH_3^+$: Conjugate base is $C_6H_5NH_2$ (aniline).$(III)$ $[H_2N-C(=NH)-NH_2]H^+$: Conjugate base is guanidine $(H_2N-C(=NH)-NH_2)$,which is a very strong base due to resonance stabilization of the cation,making the conjugate acid very weak.$(IV)$ $O_2N-C_6H_4-NH_3^+$: Conjugate base is $p$-nitroaniline. The $-NO_2$ group is a strong electron-withdrawing group $(EWG)$,which decreases the basicity of the amine,making the conjugate acid stronger.Comparing the acidity:$(IV)$ has a strong $-NO_2$ group,making it the strongest acid.$(I)$ is more acidic than $(II)$ because the phenyl group in $(II)$ is electron-withdrawing compared to the methyl group in $(I)$,but the conjugate base of $(II)$ is resonance stabilized,making $(II)$ a weaker acid than $(I)$.$(III)$ is the weakest acid because guanidine is a very strong base.Thus,the order of decreasing acidic strength is $IV > I > II > III$.

Arrange the following in order of their decreasing acidic strength:
$(I)$ $CH_3NH_3^+$
$(II)$ $C_6H_5NH_3^+$
$(III)$ $[H_2N-C(=NH)-NH_2]H^+$
$(IV)$ $O_2N-C_6H_4-NH_3^+$

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Arrange the following in order of their decreasing acidic strength:$(I)$ $CH_3NH_3^+$$(II)$ $C_6H_5NH_3^+$$(III)$ $[H_2N-C(=NH)-NH_2]H^+$$(IV)$ $O_2N-C_6H_4-NH_3^+$