Can neutralization ever be complete?
The $\ce{K_a}$ expression for acetic acid, in aqueous solution, is given by:

$\ce{K_a} =\dfrac{\ce{[CH3COO-][H+]}}{\ce{[CH3COOH]}}$

The expression can be rearranged to give

$\ce{[CH3COOH]} = \dfrac{\ce{[CH3COO-][H+]}}{\ce{K_a}}$

so no matter what the pH, all the acetic acid will never be reacted. 

So in a titration let's assume that we start out with 0.1000 moles of whatever acid $\ce{[HA]_{initial}}$. 


After base has added and $0.1000 \gg \ce{[HA]_{final}}$ and thus $0.0001 \gt \ce{[HA]_{final}}$, then the reaction is  quantitatively complete. 

This is strictly a significant figures argument. You can't do a titration to 10 significant figures. 3 is decent, if you get 4 you're a magician. 
When 0.1000 moles of base have been added to the solution the equivalent point has been reached.

The key point is that the moles of base is equal to moles of acid, regardless of the pH.
When ever you get the "signal" that the titration is over you have reached the end point.

The signal could be, for example, a color change of an indicator, the swing of the needle on a pH meter, or the formation of a precipitate.