Textbook Problem 6D 9

[Natalie Vu 1I]

Hi,

I was trying to solve this problem but I didn't see how to find x using the percent deprotonation

[Maia V 1L]

First you multiply 0.024 x 0.110 M to get the molarity of H3O+ at the end of the reaction. You should get 0.00264 M. Then take the -log(0.00264) to get pH=2.58.

[905756606]

This question doesn't use the typical procedure we use to find 'X' per se but since we know that percentage deprotonation of a WA is [H3O+]/[HA initial]*100, we can rearrange this equation to find [H3O+] and therefore the pH. Hope this helps!