A student performs a titration of 37.0 mL of a phosphoric acid (H:PO4) solution of unknown concentration with a standardized 1.25 M NAOH solution. The titration requires 26.2 mL of base to reach the third equivalence point. What is the concentration of the H3PO4 solution?

A student performs a titration of 37.0 mL of a phosphoric acid (H:PO4) solution of unknown concentration with a standardized 1.25 M NAOH solution. The titration requires 26.2 mL of base to reach the third equivalence point. What is the concentration of the H3PO4 solution?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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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.

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Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
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