determining the volume of base needed to titrate

Question

A chemistry student weighs out 0.310g of ascorbic acid H2C6H6O6, a diprotic acid, into a 250.mL

 volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1000 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits.

Answer 1

H₂C₆H₆O₆ + 2NaOH ==> Na₂C₆H₆O₆ + 2H₂O ... balanced equation for the neutralization reaction

mols H₂C₆H₆O₆ present = 0.310 g x 1 mol H₂C₆H₆O₆ / 176.1 g = 0.00176 mols

mols NaOH required = 0.00176 mols H₂C₆H₆O₆ x 2 mols NaOH / 1 mol H₂C₆H₆O₆ = 0.00352 mols NaOH

Volume of 0.1000 M NaOH = 0.00352 mols x 1 L / 0.1000 mols = 0.0352 L = 352 mls (3 sig. figs.)