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In acidic medium, the rate of reaction between ${[{BrO}_{3}]}^{-} and {Br}^{-}$ ions is given as
$- \frac{d {[{BrO}_{3}]}^{-}}{dt} = k [{BrO}_{3}^{-}] [{Br}^{-}] {[H^{+}]}^{2}$
It means that

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the change in pH of the solution will not affect the rate of reaction

rate constant of the reaction is 2 s-1

the reaction rate increases by 4 times on doubling the concentration of H+ ions.

All of the above

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detailed solution

Correct option is C

Since, the rate law contains [H+] term. This means that rate changes with variation in the value of pH.

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In acidic medium, the rate of reaction between BrO3−and Br− ions is given as −dBrO3−dt=kBrO3−Br−H+2It means that

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Ready to Test Your Skills?

free study material

In acidic medium, the rate of reaction between ${[{BrO}_{3}]}^{-} and {Br}^{-}$ ions is given as
$- \frac{d {[{BrO}_{3}]}^{-}}{dt} = k [{BrO}_{3}^{-}] [{Br}^{-}] {[H^{+}]}^{2}$
It means that