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What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 10-4) and 0.200 mol of NaF to which 0.070 mol of HCI were added?

What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 10-4) and 0.200 mol of NaF to which 0.070 mol of HCI were added?

Chemistry
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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Notes: my answer was 3.24 and it was wrong
7:27 PM Wed May 31 Gestion 16 of 140 What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10-4) and 0.200 mol of NaF to which 0.070 mol of HCI were added? un for additional resources
Transcribed Image Text:7:27 PM Wed May 31 Gestion 16 of 140 What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10-4) and 0.200 mol of NaF to which 0.070 mol of HCI were added? un for additional resources
Your submission: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 10-4) and 0.200 mol of NaF to which 0.070 mol of HCI were added? Incorrect, 1 attempt remaining 3.24 Question 15 of 14 here or pull up for additional resources Retry Feedback: Note the presence of an acid and its conjugate base in this buffer solution to which acid has been added. To solve this problem, you will need to plug the appropriate pKa value into the Henderson-Hasselbalch equation. Recall the relationship between pka and pKb for a given conjugate acid-base pair.
Transcribed Image Text:Your submission: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 10-4) and 0.200 mol of NaF to which 0.070 mol of HCI were added? Incorrect, 1 attempt remaining 3.24 Question 15 of 14 here or pull up for additional resources Retry Feedback: Note the presence of an acid and its conjugate base in this buffer solution to which acid has been added. To solve this problem, you will need to plug the appropriate pKa value into the Henderson-Hasselbalch equation. Recall the relationship between pka and pKb for a given conjugate acid-base pair.
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