How many mL of a 1.06 M H,SO4 solution are required to titrate 33.0 mL of a 0.920M KOH solution?H2SO4(aq) + 2KOH(aq)--> K2SO4(aq) + 2H2O(1).O 6.09 mLO 9.82 mLO 43.1 mlO 17.3 mLO 17.1 mLO 14.3 mLO 22.8 mLO 31.5 mL

Given data, Molarity of H2SO4 solution = 1.06 M Molarity of KOH solution = 0.920 M Volume of KOH…

Answered: How many mL of a 1.06 M H,SO4 solution…

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

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Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.145E

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How many mL of a 1.06 M H,SO4 solution are required to titrate 33.0 mL of a 0.920 M KOH solution? H2SO4(aq) + 2KOH(aq) --> K2SO,(aq) + 2H2O(1). O 6.09 mL O 9.82 mL O 43.1 mL O 17.3 mL O 17.1 mL O 14.3 mL O 22.8 mL O 31.5 mL