Question

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.
A. only (ii)
B. only (iii)
C. only (i) and (ii)
D. only (iii) and (iv)

Answer 1

Correct Answer - D
Is wrong because rate constant does not depend upon the concentrations of the reactant. (ii) is wrong because rate depends upon `[H^(+)]^(2)`
(iii)is correct because change in pH means change in `[H^(+)]` ions
(iv) is correct because rate `prop [H^(+)]^(2)`