November 29, 2024, 03:23:40 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Strong Base Titration  (Read 3681 times)

0 Members and 1 Guest are viewing this topic.

Offline FouRRaW

  • Regular Member
  • ***
  • Posts: 72
  • Mole Snacks: +1/-0
Strong Base Titration
« on: June 05, 2006, 10:04:03 PM »
Why, when an unknown acid is titrated.  Why do we always use a strong Base as the titrant?

Isn't it something about neutralizing H3O+ ions??

If that is they case i just don't know why it's so important to neutralize the H3O+ ions??

Thanks
Logged

Offline Alberto_Kravina

  • Assault Chemist
  • Retired Staff
  • Full Member
  • *
  • Posts: 608
  • Mole Snacks: +70/-15
Re: Strong Base Titration
« Reply #1 on: June 06, 2006, 02:41:40 AM »
Quote
If that is they case i just don't know why it's so important to neutralize the H3O+ ions??
The most important thing about an acid base titration is that the H3O+ ions are neutralized.
The endpoint of this titration is when 100% H3O+ ions are neutralized
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: Strong Base Titration
« Reply #2 on: June 06, 2006, 02:56:09 AM »
Quote from: FouRRaW on June 05, 2006, 10:04:03 PM
Why, when an unknown acid is titrated.  Why do we always use a strong Base as the titrant?

You need as large pH change close to the equivalence point as possible. Think how this pH change depends on the strength of the titrant.
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info
Pages: [1]   Go Up
« previous next »
Sponsored Links