January 16, 2025, 01:06:33 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: preparing a buffer  (Read 4149 times)

0 Members and 1 Guest are viewing this topic.

mikey14

  • Guest
preparing a buffer
« on: November 13, 2005, 03:17:34 AM »
Question:
How much .0036 M HCl should be added to .1 L of a .042 M ammonia solution to make a pH 8.8 buffer? State all assumptions.

I thought about using the Henderson-Hasselbach equation, but I don't think that would work. I also started with the equation: NH3 + H20 < = > NH4+  + OH-, knowing that NH4 is NH3's conjugate acid.

Any help is much appreciated!
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27895
  • Mole Snacks: +1816/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re:preparing a buffer
« Reply #1 on: November 13, 2005, 04:15:25 AM »
You are on the right track, continue!
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

mikey14

  • Guest
Re:preparing a buffer
« Reply #2 on: November 13, 2005, 12:31:58 PM »
I'm just not sure how the strong acid would affect it. I could use pOH=pKb+log(conj. acid/base), to get a ratio of the conj. acid /base. Then I'm stuck.
Thanks
Logged

Offline AWK

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7976
  • Mole Snacks: +555/-93
  • Gender: Male
Re:preparing a buffer
« Reply #3 on: November 14, 2005, 01:50:56 AM »
Strong acid reacts with base to form a salt. An axcessing ammonia and salt form a buffer soluta ion
« Last Edit: November 14, 2005, 01:51:41 AM by AWK »
Logged
AWK
Pages: [1]   Go Up
« previous next »
Sponsored Links