According to the experiment procedure, given that the NaOH solution has a concentration of 0.100M, and that the vinegar (acetic acid) has a concentration of 5.0% m/m (mass percent), what volume (mL) of titrant would be required to reach the “equivalence point” if you place 2.500g of vinegar in the flask (show calculations)?

Answer 1

5% acetic acid is 5 g acid/100 g soln. Acid to titrate is 5g x (2.5/100) = 0.125 g acid. Convert to moles. moles = grams/molar mass.
Then moles acid = moles NaOH at the equivalence point.
moles NaOH = M x L. Solve for L and convert to mL.