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(C) The basic strength of an anion is inversely proportional to its stability. The more stable the anion,the less basic it is.$1$. In compound $B$,the

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$C > A > B$

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(C) The basic strength of an anion is inversely proportional to its stability. The more stable the anion,the less basic it is.$1$. In compound $B$,the negative charge is at the para-position relative to the carbonyl group,allowing for extensive resonance stabilization through the carbonyl group.$2$. In compound $A$,the negative charge is at the alpha-position relative to the carbonyl group,which also allows for resonance stabilization,but it is less stable than the para-anion due to the proximity of the negative charge to the electronegative oxygen atom.$3$. In compound $C$,the negative charge is at the meta-position relative to the carbonyl group,where it cannot be delocalized by resonance into the carbonyl group. Thus,it is the least stable.Stability order of anions: $B > A > C$.Since basic strength $\propto \frac{1}{	ext{stability of anion}}$,the basic strength order is $C > A > B$.

Compare the basic strengths of the given compounds:

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