If you are talking about the pH at the equivalence point in the titration of vinegar with say NaOH, then the pH is determined by the hydrolysis of the salt produced. In this case the salt is NaAc and the acetate ion hydrolyzes as follows and I will call the beginning concn of the acetate ion simply M since you didn't provide any data.
.........Ac^- + HOH ==> HAc + OH^-
I........M...............0.....0
C........-x.............x.......x
E.......M-x.............x.......x
Kb for Ac^- = (Kw/Ka for HAc) = (x)(x)/(M-x). Solve for x = (OH^-) and convert that to pH.
For 0.1 M solutions that will be very close to 8.7 give or take a little.
What is the average [H3O^+] of the vinegar solution at the neutralization point in the titration process? pls need help with this. i tried to research about it but can't find any answer or any explanations anout this. Thanks
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