In a titration experiment, a 5.00-mL sample of sulfuric acid, H2SO4, from a car battery is diluted with de-ionized water to 100.0 mL. A 20.00-mL portion of the diluted acid is titrated with 0.2025 M NaOH solution. If 42.00 mL of the NaOH solution is required to neutralize the dilute acid, what is the molar concentration of H2SO4 in the original solution taken from the battery? The acid-base reaction occurs as follows: H2SO(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(l) (A) 0.2126 M (B) 0.4252 M (C) 4.25 M (D) 8.50 M

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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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In a titration experiment, a 5.00-mL sample of sulfuric acid, H₂SO₄, from a car battery is diluted with de-ionized water to 100.0 mL. A 20.00-mL portion of the diluted acid is titrated with 0.2025 M NaOH solution. If 42.00 mL of the NaOH solution is required to neutralize the dilute acid, what is the molar concentration of H₂SO₄ in the original solution taken from the battery? The acid-base reaction occurs as follows:

H₂SO(aq) + 2NaOH(aq) --> Na₂SO₄(aq) + 2H₂O(l)

(A) 0.2126 M

(B) 0.4252 M

(D) 8.50 M

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