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Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.11 mol NaOH is added, and calculate the pH after 0.25 mol HCI is added to the original solution. Ka=7.2x10-4 pH = pH = when NaOH is added when HCI is added

Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.11 mol NaOH is added, and calculate the pH after 0.25 mol HCI is added to the original solution. Ka=7.2x10-4 pH = pH = when NaOH is added when HCI is added

Chemistry: Principles and Practice
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 16.44QE
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Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.11 mol NaOH is added, and calculate the pH after 0.25 mol HCI is added to the original solution. Ka = 7,2x10-4 pH = pH when NaOH is added when HCI is added
Transcribed Image Text:Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.11 mol NaOH is added, and calculate the pH after 0.25 mol HCI is added to the original solution. Ka = 7,2x10-4 pH = pH when NaOH is added when HCI is added
Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0015 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3x10-7 Concentration = M
Transcribed Image Text:Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0015 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3x10-7 Concentration = M
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