a) 50.00 mL of 0.1500 M NaOH is used to titrate 15.25 mL of H3PO4 to the endpoint (neutralization). Calculate the molarity of the H3PO4. b) 20.00 mL of 1.00 M KOH is used to titrate 25.00 mL of HC2H3O2 to the endpoint (neutralization). Calculate the molarity of the HC2H302.

a) 50.00 mL of 0.1500 M NaOH is used to titrate 15.25 mL of H3PO4 to the endpoint (neutralization). Calculate the molarity of the H3PO4. b) 20.00 mL of 1.00 M KOH is used to titrate 25.00 mL of HC2H3O2 to the endpoint (neutralization). Calculate the molarity of the HC2H302.

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 92A

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

a) 50.00 mL of 0.1500 M NaOH is used to titrate 15.25 mL of H3PO4 to the endpoint (neutralization).
Calculate the molarity of the H3PO4.
b) 20.00 mL of 1.00 M KOH is used to titrate 25.00 mL of HC2H3O2 to the endpoint (neutralization).
Calculate the molarity of the HC2H302.

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