A solution of 50.0 mL of 0.20 M H2SO4 is titrated with 1.0 M of LIOH. H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O What volume of LiOH is required to neutralize the acid completely? Vol LiOH = [?] mL Hint: Be careful of the mole ratios! Vol LiOH (mL) Enter

A solution of 50.0 mL of 0.20 M H2SO4 is titrated with 1.0 M of LIOH. H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O What volume of LiOH is required to neutralize the acid completely? Vol LiOH = [?] mL Hint: Be careful of the mole ratios! Vol LiOH (mL) Enter

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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.

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A solution of 50.0 mL of 0.20 M H2SO4
is titrated with 1.0 M of LiOH.
H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O
What volume of LiOH is required to
neutralize the acid completely?
Vol LiOH = [?] mL
Hint: Be careful of the mole ratios!
Vol LiOH (mL)
Enter

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