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A reaction is catalysed by $H^{+}$ ion, and In the rate law the dependence of rate is of first order with respect to the concentration of $H^{+}$ ions, in presence of HA rate constant is $2 \times 10^{- 3} \min^{- 1}$ and in presence of HB rate constant is $1 \times 10^{- 3} \min^{- 1}$ $HA$ and $HB$ have relative strength as :

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Detailed Solution

The ratio of rate constants,

$\frac{k_{1}}{k_{2}} = \frac{{[H^{+}]}_{HA}}{{[H^{+}]}_{HB}} \frac{k_{1}}{k_{2}} = \frac{2 \times 10^{- 9}}{1 \times 10^{- 3}} \frac{k_{1}}{k_{2}} = 2$

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