In an acid-base titration, the neutralization of 20.00 mL of a solution of KOH (potassium hydroxide) of unknown concentration required the addition of 21.50 mL of 0.1532 M HNO3 (nitric acid). Calculate the molarity of the potassium hydroxide solution. Place your answer in the box. Express your answer using only a number or numbers without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.

In an acid-base titration, the neutralization of 20.00 mL of a solution of KOH (potassium hydroxide) of unknown concentration required the addition of 21.50 mL of 0.1532 M HNO3 (nitric acid). Calculate the molarity of the potassium hydroxide solution. Place your answer in the box. Express your answer using only a number or numbers without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.

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

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 101AE: You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final...

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