1. Calculate the molarity of H3O+ and the molarity of OH-, as well as the pH of thefollowing solutions of strong acids and bases at 25°C.а) 0.001 М НCІex: pH = -log(0.001 M) = 3.0; pKw = -log(1.00 x 1014) = 14.000 = pH + pOH;pOH = 14.000 – 3.0 = 11.0; [OH] = 1 x 1011 M%3Db) 0.125 M HNO3c) 0.0031 M NaOHd) 0.012 M Ba(ОН)2е) 2.1x104 М HCIOA

Strong acid are those which can completely dissociate into water to give H+ ion Example = HCl, HNO3…

1. Calculate the molarity of H3O+ and the molarity of OH-, as well as the pH of the following solutions of strong acids and bases at 25°C. a) 0.001 М НCI ex: pH = -log(0.001 M) = 3.0; pKw = -log(1.00 x 10-14) = 14.000 = pH + pOH; РОН 3 14.000 - 3.0 %3D 11.0%; [ОН]%31x 1011 М %3D %3D %3D b) 0.125 М HNO3 c) 0.0031 M NAOH d) 0.012 M Ba(ОН)2

1. Calculate the molarity of H3O+ and the molarity of OH-, as well as the pH of the following solutions of strong acids and bases at 25°C. a) 0.001 М НCI ex: pH = -log(0.001 M) = 3.0; pKw = -log(1.00 x 10-14) = 14.000 = pH + pOH; РОН 3 14.000 - 3.0 %3D 11.0%; [ОН]%31x 1011 М %3D %3D %3D b) 0.125 М HNO3 c) 0.0031 M NAOH d) 0.012 M Ba(ОН)2

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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