In acidic medium the rate of reaction between ${\left({\mathrm{BrO}}_3\right)}^{-}\text{and }{\mathrm{Br}}^{-}$ ions is given by the expression.

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

doubling the concentration of ${\mathrm{H}}^{+}$ ions will increase the reaction rate by 4 times

rate of reaction is independent of the concentration of acid

the changes in $\mathrm{pH}$ of the solution will not affect the rate

rate constant of overall reaction is 4 ${\sec }^{-1}$