November 28, 2024, 07:51:10 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Titration 2  (Read 2695 times)

0 Members and 1 Guest are viewing this topic.

Offline Sayanthan

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Titration 2
« on: May 19, 2010, 10:56:38 AM »
When 20 mL of 0.300 mol/L HC2H3O2(aq) is titrated with 20 mL of 0.300 mol/L NaOH(aq), what is the pH of the solution at equivalence point?
Please include steps to completing this problem and thanks in advance. :)
Logged

Offline Schrödinger

  • Chemist
  • Sr. Member
  • *
  • Posts: 1162
  • Mole Snacks: +138/-98
  • Gender: Male
Re: Titration 2
« Reply #1 on: May 19, 2010, 01:40:38 PM »
You need to show us your attempt. Please read forum rules
Logged
"Destiny is not a matter of chance; but a matter of choice. It is not a thing to be waited for; it is a thing to be achieved."
- William Jennings Bryan

Offline Sayanthan

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Re: Titration 2
« Reply #2 on: May 19, 2010, 10:17:32 PM »
Because the two solutions have equal molarity, and HCl and NaOH react 1:1

Total volume of solution = 20+20 = 40 ml.
What is the molarity of 0.3 mol HCl dissolved in 40ml solution:
1000/40*0.3 = 7.5M

Because [HCl] = 7.5M, [H+] = 7.5M

pH = -log [H+]
pH = -log 7.5
pH = -0.88
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27863
  • Mole Snacks: +1813/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Titration 2
« Reply #3 on: May 20, 2010, 03:14:52 AM »
There is no HCl in this solution.

You are at the equivalence point.

http://www.titrations.info/acid-base-titration-equivalence-point-calculation
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info
Pages: [1]   Go Up
« previous next »
Sponsored Links