[Mint]

I was doing an experiment in chemistry class involving titrations. I would heat up different samples of vinegar and titrate them using NaOH. The trend that I found was how when temperature increase, the pH of the endpoint decreases. Can someone explain why this happens to me please?

[Borek]

How large were the differences? How was the endpoint detected?

What do you know about endpoints? What do they depend on?

[Mint]

How large were the differences? How was the endpoint detected?

What do you know about endpoints? What do they depend on?

There was a pH decrease of about 1 from 25-100 degrees Celsius. The endpoint was calculated using the equilibrium expression and the pOH and pKw formulas.  Thats about all I know really.

[Vidya]

Understand the nature of acid you are using ---weak acid
Now at the endpoint acid is neutralized by strong base NaOH
This results in the formation of basic salt(do you know why??)
So endpoint pH expected here is basic.
AS you increase temperature --Ka (acid dissociation constant ) also increases and strength of the acid is more than what it was at low temperature. Can you now try to relate it with strength of the conjugate base and then pH at the equivalence point?