March 29, 2024, 03:36:10 AM
Forum Rules: Read This Before Posting


Topic: Why is this a buffer system?  (Read 3805 times)

0 Members and 1 Guest are viewing this topic.

Offline nozo

  • Regular Member
  • ***
  • Posts: 36
  • Mole Snacks: +2/-0
  • Gender: Female
  • I'm a mole!
Why is this a buffer system?
« on: August 12, 2006, 02:07:21 PM »
Can someone kindly explain to me why the following is a buffer system?

5 ml of 1.00M HCl and 10 ml of 1.00M Sodium Acetate

I know it says that a buffer is a combo of a weak acid and its conj. base (vice-versa), but isn't HCl a strong acid ??? I'm so confused...

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27633
  • Mole Snacks: +1799/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Why is this a buffer system?
« Reply #1 on: August 12, 2006, 02:24:13 PM »
What will HCl do to acetate? Remember that acetic ion is a base.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline nozo

  • Regular Member
  • ***
  • Posts: 36
  • Mole Snacks: +2/-0
  • Gender: Female
  • I'm a mole!
Re: Why is this a buffer system?
« Reply #2 on: August 12, 2006, 02:37:59 PM »
What will HCl do to acetate? Remember that acetic ion is a base.

Ohhh... HCl reacts with the sodium acetate to produce acetic acid which is a weak acid... duhh.... lol, Thanks again Borek!

Sponsored Links