In acidic medium the rate of reaction between $Br{O}_3^{-}$ and $B{r}^{-}$ ion is given by the expression

$\frac{d\left(Br{O}_3^{-}\right)}{dt}=K \left[Br{O}_3^{-}\right] \left[B{r}^{-}\right] {\left[H^{+}\right]}^2$

Which of the following is correct?

 

For the reaction,

$\frac{\mathrm{d}\left[{\mathrm{BrO}}_3^{-}\right]}{\mathrm{dt}}=\mathrm{K} \left[{\mathrm{BrO}}_3^{-}\right] \left[{\mathrm{Br}}^{-}\right] {\left[{\mathrm{H}}^{+}\right]}^2$

The rate law equation indicates that it depends on the concentration of $\left[{\mathrm{BrO}}_3^{-}\right], \left[{\mathrm{Br}}^{-}\right]$ and twice the concentration of $\left[{\mathrm{H}}^{+}\right].$ This indicates that the rate affects by the concentration of acid and change in pH of the solution. It also signifies that if concentration $\left[{\mathrm{H}}^{+}\right]$ becomes twice, then the rate becomes four times.