# 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.

## closed as off-topic by Jon Custer, user55119, Todd Minehardt, A.K., MithoronApr 14 at 21:53

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$$\ce{CH3COOH <=> H+ + CH3COO-}$$
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.