In acidic medium the rate of reaction between `[BrO_(3)^(-)]` and `[Br^(-)]` ions given by the expression
`- (d[BrO_(3)^(-)])/(dt) = k [BrO_(3)^(-)][Br^(-)][H^(+)]^(2)`
It means
(i) rate of constant of the reaction depends upon the concentration of `H^(+)` ions
(ii) rate of reaction is independent of the concentration of acid added
(iii) the change in pH of the solution will affect the rate of reaction
(iv) doubling the concentration of `H^(+)` ions will increase the reactions rate by 4 items.

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.