March 29, 2024, 04:21:18 AM
Forum Rules: Read This Before Posting


Topic: titration  (Read 2903 times)

0 Members and 1 Guest are viewing this topic.

Offline youxcrushxme

  • Very New Member
  • *
  • Posts: 1
  • Mole Snacks: +0/-0
titration
« on: September 04, 2007, 09:31:19 PM »
Quick question -

would diluting an unknown solution change the number of moles of titrant needed to completely titrate it? I feel like it wouldn't but I'm not sure :)

Thanks!

Offline enahs

  • 16-92-15-68 32-7-53-92-16
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 2179
  • Mole Snacks: +206/-44
  • Gender: Male
Re: titration
« Reply #1 on: September 04, 2007, 10:46:21 PM »
No.

Update to be more clear. As just "no" can imply you are either right or wrong! heh

No it will not change the number of moles required to titrate it. You are not changing the number of moles in the original solution, just the volume it is in.

« Last Edit: September 04, 2007, 11:14:58 PM by enahs »

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27633
  • Mole Snacks: +1799/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: titration
« Reply #2 on: September 05, 2007, 02:38:24 AM »
Define "completely titrate". To the real/theoretical endpoint? Dilution doesn't matter by definition. To the indicated endpoint? Volume of the titrated solution has to be taken into account.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Sponsored Links