Saturday
August 30, 2014

Homework Help: Chemistry

Posted by Daniel on Wednesday, September 5, 2012 at 8:52pm.

How many moles of H2PO4 and HPO4 would be needed to prepare 1.0 L of a 0.01M phosphate buffer with a pH of 6.82?

Use the Henderson-Hasselbalch equation.
pH = pKa + log (base)/(acid).

Thank you, but I guess what my question should have been is what is the acid in this question and what is the base. I would assume that both H2PO4 and HPO4 are acids and phosphate is the base but Im not sure.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemisty - How many moles of H2PO4 and HPO4 would be needed to prepare 1.0 L of ...
chem: Drbob222 - Hi I have a follow up to a question that was answered ...
CHEMISTRY - pH= 7.44 What is the ratio of [H2PO4^-]/[HPO4^2-] What does the pH ...
College Chem 2 - which of the following has the highest buffer capacity? A 0....
chem - I posted a question earlier that I was having trouble with, but I was ...
chemistry 2 - which of the following has the highest bugger capacity? A 0.10M ...
chem - write an equation for which component of the phosphate buffer (H2PO4-/ ...
chemistry - use the Henderson-Hasselbalch equation to calculate the pH of a ...
Analytical Chemistry - Phosphoric acid is a triprotic acid with the following ...
Chemistry - Calculate the amount of NaH2PO4 and Na2HPO4 needed to prepare 100 mL...

Search
Members