A 5.00-mL sample of phosphoric acid, H3PO4, is diluted to 100.0 mL. Then, a 10.00-mL portion of the dilute acid is titrated with 0.2145 M NaOH solution. (a) Write a balanced equation for the reaction of sulfuric acid with sodium hydroxide. (b) If 28.50 mL of NaOH solution is required to reach end-point, calculate the molar concentration of H2SO4 in the dilute solution. (c) What is the molar concentration of H2SO4 in the original sample?

A 5.00-mL sample of phosphoric acid, H3PO4, is diluted to 100.0 mL. Then, a 10.00-mL portion of the dilute acid is titrated with 0.2145 M NaOH solution. (a) Write a balanced equation for the reaction of sulfuric acid with sodium hydroxide. (b) If 28.50 mL of NaOH solution is required to reach end-point, calculate the molar concentration of H2SO4 in the dilute solution. (c) What is the molar concentration of H2SO4 in the original sample?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 26P

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