Dear
Katrina007, Dear
All,
Sorry, but I think, a very confuse situation has now arrived, as everybody talks a different item!
First: Katrina007, after your second study the Chapter,
ALL the Statements you did are unexceptional correct.
Why: The equivalence point is
NOT defined as the equivalent concentration of the Base to their corresponding Acid, and therefore the answer of a pH of
5 is a quite good approximation for the reality, I think.
But why is it only an approximation?: As we don’t know the exact starting concentration and don’t know also the constancy of the titration volume, we cannot calculate the exact pH value.
The pH of
9, from the List, corresponds in this Example with the value where
[NH4 + ] and
[NH3] are equivalent, and this value is nearly independent of concentration influences at all.
A Picture for this circumstance you may see on the left side of:
http://www.p-forster.com/english/themes/Spectroscopy/Spectroscopy_FAQ.htm(
But keep in mind,
that the equivalence point is lying, - for titration with strong acid on the left boarder, - and for titration with strong base on the right boarder of the graph. )
I think you know in which physical constant both concentrations are relevant.
So the thumb-rule holds, which tells you that the
equivalence pH lies always on the side of the stronger titration partner.
Good Luck!
ARGOS
++P.S.: In titration with a strong acid, not the week acid is making pH 2, or similar.