Go Back   Chemistry Help Forum > Chemistry Forums > Advanced Chemistry Forum

Advanced Chemistry Forum Organic chemistry, analytical chemistry, inorganic chemistry, physical chemistry, and biological chemistry questions go here.

Reply
 
Thread Tools Display Modes
Old Mar 5th 2017, 03:33 PM   #1
chemangel
Junior Member
 
Join Date: Mar 2017
Location: Los Angeles
Posts: 3
chemangel is on a distinguished road
Titration curve: need help explaining!

I need help with explaining these two curves. The left, Fig. 11-1(a), is a strong acid, HCl, titrated with a strong base, NaOH. The right, Fig. 11-1(b), is acetic acid titrated with NaOH as well.
I understand that for Fig. 11a, the different initial pH for the different concentrations are due to HCl dissociation, which is concentration dependent. But there are a couple things I don't understand about the curves.

1. Why are the initial pH of the acetic acid so similar to each other before the equivalence point if their concentrations are all different?

2. For all analytes in both figures, why is the amount of titrant the same to reach the equivalence point?

3. After equivalence point is reached, why do the curves behave similarly for both figures?
Attached Images
File Type: jpg Screen Shot 2017-03-05 at 3.38.40 PM.jpg (20.7 KB, 2 views)
chemangel is offline   Reply With Quote
Reply

  Chemistry Help Forum > Chemistry Forums > Advanced Chemistry Forum



Thread Tools
Display Modes



Facebook Twitter Google+ RSS Feed