April 27, 2024, 12:26:40 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Using an ICE table to solve a Henderson-Hasselbalch problem  (Read 3602 times)

0 Members and 1 Guest are viewing this topic.

Offline StevenUSF

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Using an ICE table to solve a Henderson-Hasselbalch problem
« on: October 02, 2014, 09:51:30 PM »
In 0.1M solution of weak acid: pH=9.0, pKa=9.6. How much 5M KOH must be added for pH=10.0? My answer book suggests to use the HH equation, but I want to solve using an ICE table. Is the possible? If so, how?
« Last Edit: October 02, 2014, 10:03:30 PM by StevenUSF »
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27664
  • Mole Snacks: +1801/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Using an ICE table to solve a Henderson-Hasselbalch problem
« Reply #1 on: October 03, 2014, 04:42:43 AM »
ICE table works when your unknown is related to Change, in this question your unknown is Initial. Perhaps it is possible to somehow tweak ICE table approach, but I don't see how ATM.

You can use ICE table to find the exact pH of the buffer (once you know how it was prepared):

http://www.chembuddy.com/?left=buffers&right=with-ICE-table

Not that it makes much sense, as you can see the difference between 'exact' answer and the one yielded by HH equation is negligible.
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info
Pages: [1]   Go Up
« previous next »
Sponsored Links