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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: StevenUSF on October 02, 2014, 09:51:30 PM

Title: Using an ICE table to solve a Henderson-Hasselbalch problem
Post by: StevenUSF 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?

Title: Re: Using an ICE table to solve a Henderson-Hasselbalch problem
Post by: Borek 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.