What volume of a 0.313 M perchloricacid solution is required to neutralize 15.3mL of a 0.185 M barium hydroxidesolution?mL perchloric acid What volume of a 0.107 M potassiumhydroxide solution is required toneutralize 11.9 mL of a 0.142 Mperchloric acid solution?mL potassiumhydroxide

Ba(OH)2(aq) + 2 HClO4 (aq) ⇌ Ba(ClO4)2 (aq) + 2H2O(l)Moles of Ba(OH)2 = 0.0153L × 0.185mol1L= 0.00283molAt neutralization,2 ×Moles of Ba(OH)2 = Moles of HClO4Moles ofHClO4 = 0.00566molVolume of HClO4 = 0.00566mol × 1L0.313mol = 0.0181LVolume of HClO4 = 18.1mL KOH(aq) + HClO4 (aq) ⇌ KClO4(aq) + H2O(l)Moles of HClO4 = 0.0119L × 0.142mol1L= 0.00169molAt neutralization,Moles of KOH = Moles of HClO4Moles of KOH = 0.00169molVolume of KOH = 0.00169mol × 1L0.107mol = 0.0158LVolume of KOH = 15.8mL

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What volume of a 0.313 M perchloric acid solution is required to neutralize 15.3 mL of a 0.185 M barium hydroxide solution? |mL perchloric acid

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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