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(A) The acidic strength of a compound depends on the stability of its conjugate base. The more stable the conjugate base,the stronger the acid.$I$: $1

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$II > I > III$

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(A) The acidic strength of a compound depends on the stability of its conjugate base. The more stable the conjugate base,the stronger the acid.$I$: $1,3$-cyclohexanedione. The conjugate base is stabilized by resonance with two carbonyl groups.$II$: Methyl $2$-oxocyclohexanecarboxylate derivative (specifically $2$-methoxycarbonyl-$1,3$-cyclohexanedione). The conjugate base is highly stabilized by resonance with two carbonyl groups and the ester group,and it is also stabilized by the electron-withdrawing effect of the ester group.$III$: Cyclohexanone. The alpha-hydrogens are much less acidic because the resulting enolate is only stabilized by one carbonyl group.Comparing the stability of the conjugate bases:$II$ has the most stable conjugate base due to the presence of three electron-withdrawing groups (two ketones and one ester) participating in resonance.$I$ has a stable conjugate base due to two ketone groups.$III$ has the least stable conjugate base due to only one ketone group.Therefore,the order of acidic strength is $II > I > III$.

Arrange the following in increasing order of their acidic strength:

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