A solution of 25.00 mL solution of 0.2500 M HBr is titrated with a standardized 0.1242 M solution of NaOH at 25°C. a) What is the pH of the HBr solution before NaOH is added? b) How many mililiters of NaOH are required to reach the equivalence point? Write balanced chemical equation of reaction and full calculation. c) What is the pH of solution at 1.0 mL before the equivalence point? d) A 20 mL solution of unknown concentration of H2SO4 was titrated with the same solution of NaOH (c=0.1242 M). Write balance chemical equation of neutralization and calculate the unknown concentration of H2SO4 if the equivalence point was reached when 37 mL of NaOH were added.

A solution of 25.00 mL solution of 0.2500 M HBr is titrated with a standardized 0.1242 M solution of NaOH at 25°C. a) What is the pH of the HBr solution before NaOH is added? b) How many mililiters of NaOH are required to reach the equivalence point? Write balanced chemical equation of reaction and full calculation. c) What is the pH of solution at 1.0 mL before the equivalence point? d) A 20 mL solution of unknown concentration of H2SO4 was titrated with the same solution of NaOH (c=0.1242 M). Write balance chemical equation of neutralization and calculate the unknown concentration of H2SO4 if the equivalence point was reached when 37 mL of NaOH were added.

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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