Question

In acidic medium, the rate of reaction between $Br{O}_3^{-}$ and $B{r}^{-}$ is given by the expression $-\frac{d\left[Br{O}_3^{-}\right]}{dt}=k\left[Br{O}_3^{-}\right]\left[B{r}^{-}\right][H^{+}{]}^2$. It means:

• A. Rate constant of the reaction depends upon the concentration of $H^{+}$ ions only.
• 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 1

Answer: (C), (D)

The correct options are
C Doubling the concentration of H+ ions will increase the reaction rate by 4 times.
D The change in pH of the solution will affect the rate of reaction.

As per rate law, $\left[H^{+}\right]$ alters the rate of reaction. Thus, C and D are correct.