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(C) The acidic strength of these compounds depends on the stability of the conjugate base formed after the removal of the $\alpha$-hydrogen. The stabi

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$B < A < C$

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(C) The acidic strength of these compounds depends on the stability of the conjugate base formed after the removal of the $\alpha$-hydrogen. The stability of the conjugate base is increased by the electron-withdrawing $-I$ effect of the substituent groups.In compound $C$,the $\alpha$-hydrogen is flanked by two carbonyl groups (ketones),which exert a strong $-I$ effect,making the conjugate base highly stable.In compound $A$,the $\alpha$-hydrogen is between a ketone and an ester group. The ester group is less electron-withdrawing than the ketone group.In compound $B$,the two ester groups are on the same carbon. While there are two groups,the steric hindrance and the specific electronic environment make the $\alpha$-hydrogen less acidic compared to the structure in $A$ where the electron-withdrawing groups are better positioned to stabilize the negative charge.Thus,the order of increasing acidic strength is $B < A < C$.

Rank the following compounds in the order of increasing acidic strength:

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