Talk:Acid dissociation constant
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[edit] List of pKa values and compounds
Why is there a list?
- good question - it just adds length to an article that is already too long. Would anyone mind if I removed it? Conrad.Irwin 17:30, 21 March 2007 (UTC)
[edit]
shouldn't the last be pKe = pKa + pKb?
Yes, it should be. In addition, this page would probably be better placed under "acid dissociation constant" or simply "dissociation constant." I need to look up what my nearest chemistry book calls it. --ES2 19:00, 19 Aug 2004 (UTC)
In this case, Ke = Kw , so pKe = pKw = pKa + pKb
H Padleckas 15:09, 10 Apr 2005 (UTC)
Hi
It is wrong that the adicity constant ranges from 0 to 1. If the acid is almost totally disolved, the acidity constant will tend to infinity. It is true though, that the constant will tend to 0 if there is werry little disolution. /Asger Krüger 9 Nov 2004 This has been fixed. H Padleckas 15:09, 10 Apr 2005 (UTC)
[edit] Table of pKa values
Something looks wrong in this table of pKa values. Why are a bunch of bases listed in what should be an acid's table? H Padleckas 15:17, 10 Apr 2005 (UTC)
Theres really nothing 'technically' wrong with listing a pKb as a pKa as long as you know the difference, I'm going to have to call the whole table suspect now. Phosphate doesn't have a pKa or a pKb, phosphate is an ion. It is not a compound. Same goes for Borate. I'm further suspect now because all those amines that are listed could be compounds, but they could also be organic groups. I vote we strike the table and include a reference to the link currently labeled number one in a "See Also" section. EagleFalconn 21:40, 10 Apr 2005 (UTC)
Couldn't we put "ammonium" and "pyridinium," for example, instead of "ammonia" and "pyridine"? Olin
We could do it for ammonium, but that wouldn't work for pyridine. To my knowledge, a protonated pyridine is just called...a protonated pyridine. EagleFalconn 05:54, 8 February 2006 (UTC)
- Actually, a protonated pyridine IS called pyridinium! Olin
[edit] cleanup
I performed a cleanup and got rid of a lot of redundant and wordy (in my opinion, at least) information. I don't think I changed the content of the article, just tried to make it more precise. Olin
[edit] Separate basicity constant article
Shouldn't there really be a different basicity constant article? Olin 22:27, 18 February 2006 (UTC)
[edit] pKa H2S
When clicking the link for Hydrogen sulfide in the pKa table (listed at 7.00), the specific article says the pKa is 6.89. A pretty big difference. Someone who knows for sure should change one of the articles.
- It's not as big a difference as it seems, and it is a value which has not been measured (to my knowledge) for several decades... Physchim62 (talk) 08:34, 7 June 2006 (UTC)
[edit] Basicity formula
Inthe basicity formula, it reads: A–(aq) + H2O(l) ⇌ HA(aq) + OH–(aq)
Shouldn't the "A" (that I'm guessing means acid, at least in the acidic formula) be changed to B? B–(aq) + H2O(l) ⇌ HB(aq) + OH–(aq)
- No. Once the H+ leaves, what is left is an acid, regardless of the direction of reaction.
[edit] Article Cleanup Co-Ordination Point
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[edit] Discussion |
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[edit] 1/3 of the way there
Hi, I have majorly rewritten the first part of this article - but after that, I dont understand what it is on about. I dont know whether someone who does understand could perhaps simplify what is there. I was going to add some stuff about the stability of the ion affecting it - but I am not sure if that is covered under Factors that determine the relative strengths of acids and bases. Acidity in non-aqueous solutions seems to be a bit example specific and I am not sure of its relevance. I hope that what I have done is OK, and hope someone can help with the rest.
Conrad.Irwin 17:27, 21 March 2007 (UTC)
