Talk:Equivalence point

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Removed statement "Most of the time the equivalence point is at a pH of 7 and 50 mL of NaOH."

not all titrations are acid base.

Yes, what he said. Acid-base may be a good example though. I have reorganized this article, using acid-base as an example and giving an accurate definition. This was a quick patch job though.

Yep, what you guys said. A good example to build in would be the redox titration of hydrogen peroxide with potassium permanganate. No acid/base and no indicator present.

If you have equal ammounts of hydroium and hydroxide how can the ph not be 7?

Where did the above statement come from? I don't see where that is suggested. It is quite possible to mix equal volumetric, mass, or molar amounts of an acid and base and not have a pH of 7. - nick

The statement came from an anonymous editor - check the page history if you are unsure. All comments should be signed with four tildes, including your own if you don't mind. Now as for not having a pH of 7, this occurs when one species present (e.g. CHCO₂^-) is acidic or basic. Richard001 21:21, 5 June 2007 (UTC)

[edit] Merge from endpoint (chemistry)

They are not identical, but an endpoint is a form of equivalence point, so they should definitely be merged. Agreed? Richard001 21:21, 5 June 2007 (UTC)

Per our discussions elsewhere, yes.Bless sins 11:31, 6 June 2007 (UTC)

That's good enough for me. I don't have any time right now but if someone wants to move everything they can into this article please go ahead and do so. Richard001 11:51, 6 June 2007 (UTC)

A level chemistry states that an Endpoint is NOT an equivolence point. —Preceding unsigned comment added by 86.143.136.18 (talk) 18:07, 8 October 2007 (UTC)