# Why do we assume 100% ionization for acetic acid (a weak acid)? [closed]

This is about a titration. The base titrant used is sodium hydroxide.

$$\ce{CH3COOH <=> H+ + CH3COO-}$$
The base, $$\ce{NaOH}$$, keeps consuming $$\ce{H+}$$ during a titration, as a result acetic acids keeps on providing $$\ce{H+}$$ to maintain the equilibrium in water until all the acetic acid is converted into acetate ion.