Consider 1.0 L of a solution which is 0.60 M HF and 0.75 M NaF. (Ka for HF = 7.2×10-4). Part 1 Calculate the pH of this solution. pH = Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCl. pH = Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH. pH =
Consider 1.0 L of a solution which is 0.60 M HF and 0.75 M NaF. (Ka for HF = 7.2×10-4). Part 1 Calculate the pH of this solution. pH = Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCl. pH = Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH. pH =
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 112CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...
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Consider 1.0 L of a solution which is 0.60 M HF and 0.75 M NaF.
(Ka for HF = 7.2×10-4).
Part 1
Calculate the pH of this solution.
pH =
Part 2
Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCl.
pH =
Part 3
Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.
pH =
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