An enzyme-catalyzed reaction is carried out in solution containing 0.2M Tris (pKa = 8.1).

The pH of reaction mixture at the start is 7.8. As a result of the reaction, 0.033M of H+ is consumed. What will be
(a) the ratio of Tris (free base) to Tris (protonated form) at the beginning of the reaction?
(b) the ratio of Tris (free base) to Tris (protonated form) at the end of the reaction?
(c) the final pH of the reaction mixture?
(d) the final pH of the reaction mixture if no buffer was present?

Question

An enzyme-catalyzed reaction is carried out in solution containing 0.2M Tris (pKa = 8.1).

The pH of reaction mixture at the start is 7.8. As a result of the reaction, 0.033M of H+ is consumed. What will be 
(a) the ratio of Tris (free base) to Tris (protonated form) at the beginning of the reaction?
(b) the ratio of Tris (free base) to Tris (protonated form) at the end of the reaction?
(c) the final pH of the reaction mixture?
(d) the final pH of the reaction mixture if no buffer was present?

kira_yamato · Answer

Structure of Tris as follows:

aaronq · Answer

Use the Henderson-hasselbalch equaiton

kira_yamato · Answer

I've used the Henderson-Hasselbalch equation but I have no answer to pick any choices (especially for the last question). (This is actually a multiple choice question)

aaronq · Answer

So you're not getting the provided answers?