re:Strange buffer properties
You are assuming a pH of 4.7 by solving for pH in the henderson
hasselbalch equation. The henderson hasselbalchquation depends on
the common ion effect and on high molarity of the solute.
So the pH will not drop either in the sea or in a bathtub or for any
solvent in which the solute makes up at least .1 molarity.
Hope this answers your question.
----== Posted via Newsfeed.Com - Unlimited-Uncensored-Secure Usenet News==----
[Only registered and activated users can see links. Click Here To Register...] The #1 Newsgroup Service in the World! >100,000 Newsgroups
---= 19 East/West-Coast Specialized Servers - Total Privacy via Encryption =---
Strange buffer properties
the tutor is right. The Henderson-Hasselbach equation is only valid
for "normal" dilution. If you want to calculate more precise pH values
in dilute solution, there must be considered many other aspects, which
you will probably learn in physical chemistry (thermodynamic effects).
For example, you has to consider the acivity coefficient of ions....
and some other aspects. Than soon you will have a very exicting
equation which a lot of (unknown?)parameters, some of them have to be
established by thermodynamic experiments.
Donīt worry, just learn hard to understand this..............
[Only registered and activated users can see links. Click Here To Register...]lid (GeneralChemTutor) wrote in message news:<firstname.lastname@example.org>...
|All times are GMT. The time now is 10:52 AM.|
Powered by vBulletin® Version 3.8.4
Copyright ©2000 - 2015, Jelsoft Enterprises Ltd.
Copyright 2005 - 2012 Molecular Station | All Rights Reserved