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

Options

A. The rate constant of the reaction depends upon the concentration of `H^(o+)` ions.
B. The rate of reaction is independent of the concentration of the acid added.
C. Doubling the concentration of `H^(o+)` ions will increase the reaction rate by `4` times
D. The change in `pH` of the solution will affect the rate of reaction.

Answer

C, D

Explanation

Rate `prop [H^(o+)]^(2)`. Hence, doubling the concentration of `H^(o+)` ions will increase the reaction rate by `4` times. Also, the change in `pH` will change the concentration of `H^(o+)` and therefore, the rate will change.