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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.43QE: A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the...
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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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