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I removed a section "Illustration of a buffer solution in action" because, to me at least, it was redundant with the following section, and the less well presented of the two. I hope that doesn't cause consternation.
Olin03:35, 9 March 2006 (UTC)reply
As far as I know, in the equation describing the buffering capacity there is an error. The last term should be multiplied by the proton concentration [H+]. In other words the term Ca*Ka should appear as Ca*Ka*[H+]. See e.g.
http://www.chembuddy.com/?left=pH-calculation&right=pH-buffer-capacity.
I have corrected the formula. The correct formula was in fact used in the spreadsheet with which the plot was produced, so the plot is OK and the figure of 33% is also OK.
Petergans (
talk)
19:42, 11 September 2008 (UTC)reply
pH of buffer and temperature
I think it is necessary to add a section highlighting that the pH of a buffer depends on temperature and this in turn varies for different acid/base systems. People in biosciences and medicine use a lot of systems with an optimal temperature of 37 C but forget that the 0-14 pH scale with neutral pH at 7.0 is at 25 C. Having worked in different labs I have seen many people making mistakes in reporting the pH of biological samples or preparing buffers with the wrong pH value for the temperature that they are going to be used at. Is someone, with experience in editing wiki articles, willing to do that? Cheers. —Preceding
unsigned comment added by
79.107.250.250 (
talk)
14:46, 14 July 2010 (UTC)reply
Why does the pH change less in a buffer solution?
This article is missing the "why". I think it would really benefit from an explanation of why pH changes in a buffer solution are smaller than in a non-buffer solution. —Preceding
unsigned comment added by
207.81.119.184 (
talk)
02:55, 15 October 2010 (UTC)reply
I've added a section outlining this called principles of buffering, as well as reorganising some of the sections which were all under 'acid dissociation constant'.
PiFanatic (
talk)
17:10, 15 January 2011 (UTC)reply
The current equation is incomplete, and the explanation of the increase in buffer capacity at the periphery is incorrect. The proper equation is as follows:
This equation correctly explains the increase in the periphery buffer capacity as the buffer capacity due to water (the [H] and Kw/[H] terms). A simple numerical simulation with and without these terms proves they are responsible for the periphery increases. This equation also elucidates how the buffer capacities of a mix of buffers interact (they're additive).
For sake of completeness here's a derivation of the above equation:
The letter size of AH, pH and A- is too large. It does not correspond to other lettering in the diagram
The placing of AH etc. is not clear enough
The caption A- is incorrect. It should be A-
The labelling on the right axis (pH) is horizontal. This is inconsistent with the left axis label.I have reverted to the svg. I can convert this diagram to png, using PaintShop, and shall do so in the next few days.
Petergans (
talk)
09:02, 29 July 2015 (UTC)reply
In this conext it is to do with chemistry. When some acid (or alkali) is added to a buffer solution the pH of the solution does not change as much as when the same amount of acid (or alkali) is added to a solution that does not contain a buffering agent. Here is a simple example to do at home: take a sip of some lemon juice, then add a pinch of baking soda (bicarbonate) to it and take another sip. It still tasted tart. But, if you add the same amouint of baking soda to a glass of water it will taste different. You can check the pH of the solutions with litmus paper.
Petergans (
talk)
08:50, 30 January 2016 (UTC)reply
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