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14.27mL of a solution of the diprotic acid H2SO4 is titrated, and 53.90 mL of 0.35M...

14.27mL of a solution of the diprotic acid H2SO4 is titrated, and 53.90 mL of 0.35M NaOH is required to reach the equivalence point. What is the originial concentration of the acid solution?

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Answer #1

millimoles of NaOH = 53.90 x 0.350 = 18.865

H2SO4   +   2 NaOH    --------------> Na2SO4   +   2 H2O

    1                 2

1 mol H2SO4 ------------> 2 mol NaOH

    ??             ------------> 18.865 mol NaOH

moles of H2SO4 = 18.865 / 2 = 9.4325

moles = Moalrity x volume

9.4325 = Molarity x 14.27

Moalrity = 0.661 M

originial concentration of acid = 0.66 M

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