Saturday
April 19, 2014

Homework Help: College Chemistry

Posted by Kim on Tuesday, April 9, 2013 at 4:31pm.

You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point.
The pH of the other half of the original solution is measured with a pH meter. The "neutralized" solution is added to the "original" solution and the pH of this combined "final" solution is also measured.
The following are the measured values:
Mass of unknown acid 1.2357 g
Volume of NaOH used in titration 16.04 mL
Concentration of the NaOH used 0.2098 M
pH of the original acid solution 2.02
pH of the final acid solution 3.29

CALCULATE the following
(a) Molecular Weight of Acid used in titration ___________________

(b) Molarity of UNKNOWN Acid solution from titration ___________________

(c) Ka of UNKNOWN Acid ___________________

(d) Concentration of undissociated Acid from pH measurements ___________________

(e) Total concentration of UNKNOWN acid from pH measurements ___________________

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry - i am calculating an unknown acid for both monoprotic and diprotic ...
chemistry - if your lab partner determined that there were 4.030 x 1020 atoms ...
chemistry - if your lab partner determined that there were 4.030 x 1020 atoms ...
chemistry - if your lab partner determined that there were 4.030 x 1020 atoms ...
Chemistry - Now if your lab partner determined that there were 5.001 x 1022 ...
Chemistry - If it were determined that there were 6.391 x 10^22 atoms of H in an...
Chemistry - A 0.5224g sample of an unknown monoprotic acid was titrated with 0....
chemistry - I looked up how to solve it but my answer is coming out wrong. I don...
chemistry - I looked up how to solve it but my answer is coming out wrong. I don...
chemistry - I looked up how to solve it but my answer is coming out wrong. I don...

Search
Members