# Problem: Part BBy what factor will the rate of the reaction change if the pH decreases from 6.50 to 2.00? Express your answer numerically using two significant figures.Part CThe reaction is pH dependent even though the H+ ion does not appear in the overall reaction. Which of the following explains this observation?Check all that apply.a) The exponent of [H+] in the rate law is zero.b) H+ enters the reaction mechanism after the rate-determining step.c) H+ is an intermediate in the reaction mechanism.d) H+ serves as a catalyst in the reaction.

###### FREE Expert Solution

$\overline{)\left[{\mathbf{H}}^{\mathbf{+}}\right]{\mathbf{=}}{{\mathbf{10}}}^{\mathbf{-}\mathbf{pH}}}$

Suppose:

• rate 1 → pH = 6.5
• rate 1 → pH = 2.00

catalyst → does not appear in overall reaction ###### Problem Details

Part B

By what factor will the rate of the reaction change if the pH decreases from 6.50 to 2.00? Express your answer numerically using two significant figures.

Part C

The reaction is pH dependent even though the H+ ion does not appear in the overall reaction. Which of the following explains this observation?

Check all that apply.

a) The exponent of [H+] in the rate law is zero.

b) H+ enters the reaction mechanism after the rate-determining step.

c) H+ is an intermediate in the reaction mechanism.

d) Hserves as a catalyst in the reaction.