December 04, 2024, 02:35:40 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Buffer solutions volume ratio  (Read 8462 times)

0 Members and 2 Guests are viewing this topic.

Offline helpme89

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Buffer solutions volume ratio
« on: March 14, 2008, 11:37:26 PM »
so i have a question that is puzzling me so much i can not figure it out mabey you guys can guide me through it !
In what volume ratio should you mix 1.0 solutions of  NH4Cl and NH3 to produce a buffer solution having a pH = 9.70?

thank you
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27872
  • Mole Snacks: +1813/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Buffer solutions volume ratio
« Reply #1 on: March 15, 2008, 05:00:15 AM »
Google Henderson-Hasselbalch equation.
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline helpme89

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Re: Buffer solutions volume ratio
« Reply #2 on: March 15, 2008, 07:29:01 PM »
I ahve tried googling and calling other chemistry students buh no luck .. if someone could help me that would be very much appreciated!
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27872
  • Mole Snacks: +1813/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Buffer solutions volume ratio
« Reply #3 on: March 15, 2008, 07:32:33 PM »
Google and write Henderson-Hasselbalch equation.
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: Buffer solutions volume ratio
« Reply #4 on: March 15, 2008, 07:44:48 PM »
There is no way to solve this problem without using the Henderson-Hasselbalch equation.  I'm sure that very name is in the index of your text book, we need it to even start to figure out how to use the info you've been given.
Logged
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.

Offline helpme89

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Re: Buffer solutions volume ratio
« Reply #5 on: March 16, 2008, 10:34:35 PM »
sorry i misunderstood what you guys were trying to sya yes you need Henderson equation but i just do not know how to apply it to this question here it is :

 
pH = PKa + log (Base/ Acid)

much appreciation again!
 


Logged

Offline enahs

  • 16-92-15-68 32-7-53-92-16
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 2179
  • Mole Snacks: +206/-44
  • Gender: Male
Re: Buffer solutions volume ratio
« Reply #6 on: March 16, 2008, 10:42:03 PM »
So. You know the pH you want. You know your acids and bases. Look up the pKa. Solve for the ratio in the log term. Walk away.

Logged

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: Buffer solutions volume ratio
« Reply #7 on: March 17, 2008, 06:54:24 AM »
Good, now, which of your reagents is the acid, and which is the base?
Logged
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.
Pages: [1]   Go Up
« previous next »
Sponsored Links