A student in chemistry lab creates a buffer by making a 1.25 L solution that has 1.50 moles of sodium hypobromite (NaBrO) and 2.50 moles of hypobromous acid (HBrO), Ka = 2*10^-9 1. What is the initial pH of the buffer? 2. What is the pH of when 0.025 moles of NaOH are added to 50.0 mL of buffer solution? 3. Without calculating, would you expect the change in pH to be larger or smaller if 0.025 moles of HCl was added to 50.0 mL of the buffer instead? Explain.
A student in chemistry lab creates a buffer by making a 1.25 L solution that has 1.50 moles of sodium hypobromite (NaBrO) and 2.50 moles of hypobromous acid (HBrO), Ka = 2*10^-9 1. What is the initial pH of the buffer? 2. What is the pH of when 0.025 moles of NaOH are added to 50.0 mL of buffer solution? 3. Without calculating, would you expect the change in pH to be larger or smaller if 0.025 moles of HCl was added to 50.0 mL of the buffer instead? Explain.
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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A student in chemistry lab creates a buffer by making a 1.25 L solution that has 1.50 moles of
sodium hypobromite (NaBrO) and 2.50 moles of hypobromous acid (HBrO), Ka = 2*10^-9
1. What is the initial pH of the buffer?
2. What is the pH of when 0.025 moles of NaOH are added to 50.0 mL of buffer solution?
3. Without calculating, would you expect the change in pH to be larger or smaller if 0.025 moles
of HCl was added to 50.0 mL of the buffer instead? Explain.
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