home > q&a board > chemistry > topic: ph

Q BgQuestion:

Scholar
Karma Points: 345
Respect (96%):
posted by  sandybell on 9/11/2008 12:20:33 PM  |  status: Closed  

pH

Course Textbook Chapter Problem
N/A N/A N/A N/A
Question Details:
what is the pH of 0.5M acetic acid
 
please show how to do this
Bonus Point Alert! Earn +4 additional karma points for helping this annual member.

AAnswers:

Answer Question
Expert
Karma Points: 903
posted by Bob on 9/11/2008 1:00:41 PM  |  status: Live
Asker's Rating: Lifesaver   
sandybell's comment:
"thank you"
Response Details:
Here is a web-site that calulates the Ph for a .10m solution. You should be able to calculate your .5 m using the same procedure.
 
Guru
Karma Points: 2,074
posted by Xylene on 9/11/2008 1:29:41 PM  |  status: Live
Asker's Rating: Helpful   
sandybell's comment:
"thank you"
Response Details:
  [H+] = √(Ka x C)
  where [H+]  is the concentration of the acid
   Ka is the dissociation constant of the weak acid which is constant
   C is the concentration of the weak acid (given)
From the above information you can calculate the value of [H+]
   therefore pH = -log [H+]
Answer Question
Ask New Question

Join Cramster's Community

Cramster.com brings together students, educators and subject enthusiasts in an online study community. With around-the-clock expert help and a community of over 100,000 knowledgeable members, you can find the help you need, whenever you need it. Join for free today » How Cramster is different from tutoring »

Need Help In

Useful Links