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A reaction is catalysed by \( \mathrm{H}^{+} \)ion. In presence of \( \mathrm{HA} \), rate constant is \( 2 \times 10^{-3} \mathrm{~min}^{-1} \) and in presence of \( \mathrm{HB} \)
\( \mathrm{P} \) rate constant is \( 1 \times 10^{-3} \mathrm{~min}^{-1} \). HA and \( \mathrm{HB} \) being strong

W acids, we may conclude that
(A) \( \mathrm{HB} \) is stronger acid than \( \mathrm{HA} \)
(B) \( \mathrm{HA} \) is stronger acid than HB.
(C) relative strength \( \mathrm{HA} \) and \( \mathrm{HB} \) is 2 .
(D) HA is weaker than \( \mathrm{HB} \) and relative strength is \( 0.5 \).
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