Monday
September 22, 2014

Homework Help: org. chem

Posted by meghan on Friday, February 8, 2013 at 5:58pm.

How to start these problems out: Please help thank you
Use the Henderson-Hasselbach equation:
pH = pKa + log [A-]/[AH], where A- is the conjugate base and AH is the weak acid.

Calculate the pH of an acetate buffer in which the acetate concentration [CH3COO-] is 3.5 times greater than acetic acid [CH3COOH]. pKa = 4.74.

9. How would you prepare a 0.6 M acetate buffer with a pH = 4.0?

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

organic chem - . Use the Henderson-Hasselbach equation: pH = pKa + log [A-]/[AH...
Science - Given: Concentration of acetic acid 0.1M and 30mL used. Concentration ...
Chemistry - A buffer containing 1.2169 M of acid, HA, and 0.1431 M of its ...
CHEM REPOST...PLEASE CHEK! - Posted by Kat on Monday, March 2, 2009 at 11:21am. ...
Chemistry - If a researcher needs 0.50 L of 3.0 M nitrite buffer at pH 3.00, ...
Biochemistry - A person during a 24 hour period produced 1.40 litres of urine ...
CHEMISTRY HELP PLEASE - when I use henderson-hasselbach Ka of HOP4^2- = 4.8 x10...
PKA VALUES - I understand that the pH at the half equivalence point gives is the...
Chemistry - Hello, I have a question that reads, "What is the pH of a 0.01M (...
chemistry - hello, I can't seem to solve this question. i tried to look up ...

Search
Members