Thursday
December 18, 2014

Homework Help: Chemistry

Posted by Ter on Monday, February 11, 2013 at 11:21am.

Consider 54.0 mL of a solution of weak acid HA (Ka = 1.00 10-6), which has a pH of 4.200. What volume of water must be added to make the pH = 5.500?

I found HA for both and then I used C1V1 = C2V2 plugging in the concentrations of HA in C1 and C2 and 0.054 for V1, but I'm still not getting the right answer. Please help!

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

AP Chemistry - Consider 67.0 mL of a solution of weak acid HA (Ka = 1.00 10-6), ...
Chemistry - Consider 57.5 mL of a solution of weak acid HA (Ka = 1.00 10-6), ...
Chemistry - Consider 51.5 mL of a solution of weak acid HA (Ka = 1.00 10-6), ...
Chemistry/pH- Weak Acid - Hi again! I have a new question, Can you help me? ...
Chemistry/pH- Weak Acid - Hi again! I have a new question, Can you help me? ...
biochemistry - The pH of 0.02M solution of a weak acid was measured at 7.6. What...
Chemistry - Consider 57.5 mL of a solution of weak acid HA (Ka = 1.00 10-6), ...
college chemistry - Consider the titration of a 50.0 mL sample of a 0.100 M ...
chem - Calculate the final concentration of a. 4.0 L of a 4.0 M HNO3 solution is...
Food Chemistry - Calculate the amounts and pH values for preparing the following...

Search
Members