|WikiProject Chemistry||(Rated Start-class, Mid-importance)|
Links from this article with broken #section links (check):
Ammonia is a weak base, not 'relatively strong'! Also, strong acids have weak conj base, but it is NOT necessarily the case for the reverse: weak acids typically have WEAK conjugate bases as well. Think acetic acid. Acetate is a weak conjugate base. — Preceding unsigned comment added by 220.127.116.11 (talk) 06:30, 7 July 2015 (UTC)
Hi, I'm not entirely sure, but it seems like the listing HFSbF5 Fluoroantimonic acid---SbF6− Hexafluoroantimonate ion in the base-acid table is placed in the wrong place. Shouldn't it be on top? Thanks. 18.104.22.168 (talk) 00:58, 6 March 2009 (UTC)
- I think you're correct, as Fluoroantimonic acid is a super acid. I'll make the appropriate change.--E8 (talk) 01:39, 13 March 2009 (UTC)
The equation shown in this article would only apply for a strong acid. A weak acid should have two-way arrows to indicate equilibrium. Fuzzform 01:38, 19 April 2007 (UTC)
- Agreed. I made a modification. Is this acceptable as general form, or would a case-by-case listing be necessary? Examples, perhaps?--E8 05:21, 27 April 2007 (UTC)
There's no "Conjugate Salt" page or even reference to it here.
I'd be happy to contribute to such a page or section.--E8 03:02, 26 April 2007 (UTC)
Ah guys, the conjugate base of a weak acid is not a weak base... That's simply wrong.
- True, but this has not been stated or implied. The article explicitly states: "The conjugate base of a weak acid is a strong base, and the conjugate base of a strong acid is a weak base, and vice versa." The article is clearly incomplete. If you would like to do a case-by-case analysis of conjugates, please do.--E8 17:31, 4 May 2007 (UTC)
- The conjugate base of a weak acid is not a strong base, as in the case of NH4+. It is only a strong base if the Ka value is very small. —Preceding unsigned comment added by 22.214.171.124 (talk) 21:42, 17 June 2009 (UTC)
Hi I'm currently studying for my IGCSE chemistry exam, I was trying to find out what Conjugate acids and bases were and this page seemed to offer the best explanation, but I'm still completely lost could someone please put up an explanation in simpler terms.
- Pick up a copy of an appropriate-level general chemistry textbook from a local library. Most will have a chapter dedicated to the concept of "conjugate." I do think this article requires a bit of attention; I'll try to set aside some time to add more substance and clarity to it.--E8 21:40, 8 October 2007 (UTC)
Ordering of Acids
Hi, just glanced at this page, and thought the ordering of your examples was a little strange... failed to notice it was ordered by pKa, so justifiably the changes were reverted. However, on more prolonged examination of the page, it became clear there is little to explain the concept of protonation/deprotonation and the factors affecting these.
"Conjugate Acid" being the title of the page seems odd, since conjugate bases are just as important, so the page should be entitled "Conjugate acid/base pairs".
The discussion of the theory behind this equilibrium is to be found on the acid dissociation constant page, so this page would perhaps serve better as an introduction to, and definition of, the topic. In light of this, I would suggest adding some more protonated species as examples of conjugate acids, rather than purely showing the technicalities of neutral acids being 'conjugate' to their anions.