(Molarity) Using the same approach calculate how many milliliters of 0.140 M NaOH are needed to completely neutralize 27.4 mL of 0.398 M H2C4H4O6.

Answer 1

H₂C₄H₄O₆ = a diprotic acid (tartaric acid)

2NaOH + H₂C₄H₄O₆ ==> Na₂C₄H₄O₆ + 2H₂O ... balanced equation for neutralization

mols H₂C₄H₄O₆ present = 27.4 ml x 1 L /1000 ml x 0.398 mol/L = 0.00983 mols

mols NaOH needed = 0.00983 molsH₂C₄H₄O₆ x 2 mols NaOH / mol H₂C₄H₄O₆ = 0.0197 mols NaOH

volume of 0.140 M NaOH needed: 0.0197 mols x 1 L / 0.140 mol = 0.141 L = 141 mls