May 14, 2024, 09:30:14 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Titration  (Read 1364 times)

0 Members and 1 Guest are viewing this topic.

Offline sun725

  • Regular Member
  • ***
  • Posts: 72
  • Mole Snacks: +1/-0
Titration
« on: March 15, 2017, 06:38:03 AM »
I have the following question:

50.00 mL of the solution (Fe2+ / Fe3+) consumes 13.73 mL of 0.01200 M EDTA when titrated at pH = 2.00.

50.00 mL of the solution (Fe2+ / Fe3+) consumes 29.62 mL of 0.01200 M EDTA when titrated at pH = 6.00.

What is the concentration (in ppm), respectively, Fe2+ and Fe3+ in the solution? (Remember that we assume that the density of water is equal to 1 g / mL when calculating the concentration in ppm (weight / volume)).

How to approach this question. Can anyone help me where to start in order for me to solve this question ...
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27680
  • Mole Snacks: +1801/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Titration
« Reply #1 on: March 15, 2017, 07:21:42 AM »
What is being complexed at each pH?
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info
Pages: [1]   Go Up
« previous next »
Sponsored Links