12. During the titration of acetic acid with sodium hydroxide, what happens to the pH of the solution in the erlenmeyer flask as the titration begin, proceeds toward, and reaches the equivalence point? Explain.

Question

12.	During the titration of acetic acid with sodium hydroxide, what happens to the pH of the solution in the erlenmeyer flask as the titration begin, proceeds toward, and reaches the equivalence point?  Explain.

abb0t · Answer

I don't fully remember titration that much, but I can explain the best I can what I remember. Basically, at equivalence point  the moles of your acid = moles of your base. However, it doesn't mean that your pH = 7 (neutral). What you'll observe is that there is a change in color as you reach that "equivalence point" in your flask. 

However, before you reach equivalence point, the amount of sodium hydroxide added will ionize completely, that means that you'll get $Na^+$ and $OH^-$
ince at the equivalence point the solution contains only the salt. However, for a weak acid, the salt contains the conjugate base, which is able to recombine with a proton. Thus, at the equivalence point of the titration of a weak acid with a strong base, the solution is only slightly basic :)