A 1.00 ml aliquot of a concentrated H2SO4 solution is diluted to exactly 100.00 ml
in a volumetric flask. A 10.00 ml aliquot of this diluted H2SO4 required 32.94 ml
of a 0.1093 M NaOH solution to reach an endpoint.

1. Write the balanced chemical reaction describing this titration.







2. Calculate the number of moles of NaOH delivered in the titration.







3. Calculate the number of moles of H2SO4 present in the 10.00 ml aliquot used for titration.







4. Calculate the molarity of the H2SO4 in the 10.00 ml aliquot used for titration.







5. What was the molarity of the original undiluted H2SO4 solution?