March 29, 2024, 12:01:03 PM
Forum Rules: Read This Before Posting


Topic: PH at standard condition  (Read 10055 times)

0 Members and 1 Guest are viewing this topic.

Offline stevenAitsover

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
PH at standard condition
« on: April 16, 2008, 11:16:05 AM »
What would be the PH of the solution at standard conditions? (HINT: What are the concentrations of all aqueous species at standard conditions?) Plz help

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27635
  • Mole Snacks: +1799/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: PH at standard condition
« Reply #1 on: April 16, 2008, 11:46:11 AM »
Solution of what?
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline stevenAitsover

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Re: PH at standard condition
« Reply #2 on: April 16, 2008, 11:51:58 AM »
3Co(s)+2NO3-+8H+(aq)-----> 3Co+2(aq) + 2NO(g) +4 H20(l)

Offline AWK

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7979
  • Mole Snacks: +555/-93
  • Gender: Male
Re: PH at standard condition
« Reply #3 on: April 16, 2008, 12:18:31 PM »
pH of reaction mixture will depend on the amount of acid used in this reaction.
You still have to be more precise. May be you are asking about pH of Co(NO3)2 solution?
AWK

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: PH at standard condition
« Reply #4 on: April 16, 2008, 12:47:03 PM »
Furthermore, "standard conditions" isn't as well defined as you'd think.  If they mean "standard conditions for temperature and pressure", we can look it up, but you don't seem to be using any gas, so we wouldn't even need it.  We're going to need the entire question, carefully written out, to see what level of difficulty your class is at, to give useful help.
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.

Sponsored Links