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

Options

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

Answer

C, D

Explanation

Is wrong because rate constant at constant temperature, (b) is wrong because rate depends upon `[H^+]^2`, (c ) is correct be4cause change in pH mense change in `[H^+]^2`, (d) is correct because rate `prop [H^+]^2`.