In acidic medium, the rate of reaction between `BrO_(3)^(ɵ)` and `Br^(ɵ)` is given by the expression
`(-d[BrO_(3)^(ɵ)])/(dt) =k[BrO_(3)^(ɵ)][Br^(ɵ)][H^(o+)]^(2)`

Options

A. The rate constant of overall reaction is `4s^(-1)`.
B. The rate of reaction is independent of the concentration of acid.
C. The change in `pH` of the solution will no affect the rate.
D. Doubling the concentration of `H^(o+)` ions will increase the reaction rate by `4` times.

Answer

D

Explanation

Order w.r.t. `[H^(o+)] = 2`.
Hence, doubling the concentration of `[H^(o+)]` ions will increase the reaction rate by `4` times.