A 0.350 g sample of a diprotic acid is dissolved in water and titrated with 0.320 M NaOH. What is the molar mass of the acid if 36.6 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: 68 g/mol

A 0.350 g sample of a diprotic acid is dissolved in water and titrated with 0.320 M NaOH. What is the molar mass of the acid if 36.6 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: 68 g/mol

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.22QAP

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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 0.350 g sample of a diprotic acid is dissolved in water
and titrated with 0.320 M NaOH. What is the molar mass
of the acid if 36.6 mL of the NaOH solution is required to
neutralize the sample? Assume the volume of NaOH
corresponds to the second equivalence point.
molar mass:
68
g/mol
Incorrect

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