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How many moles of potassium hydroxide would have to be added to 245 mL of a 0.346 M acetic id solution, in order to prepare a buffer with a pH of 4.960? Ka = 1.8x10-5

How many moles of potassium hydroxide would have to be added to 245 mL of a 0.346 M acetic id solution, in order to prepare a buffer with a pH of 4.960? Ka = 1.8x10-5

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
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**Problem 5: Buffer Preparation Calculation** How many moles of potassium hydroxide would have to be added to 245 mL of a 0.346 M acetic acid solution, in order to prepare a buffer with a pH of 4.960? The acid dissociation constant (\(K_a\)) is given as \(1.8 \times 10^{-5}\). --- This problem is designed to test your understanding of buffer solutions and the use of the Henderson-Hasselbalch equation to calculate the amounts needed to achieve a certain pH in a buffer solution. Make sure to review the concepts of weak acids, bases, and the relationship between pH, pKa, and the concentrations of acid and its conjugate base in a solution.
Transcribed Image Text:**Problem 5: Buffer Preparation Calculation** How many moles of potassium hydroxide would have to be added to 245 mL of a 0.346 M acetic acid solution, in order to prepare a buffer with a pH of 4.960? The acid dissociation constant (\(K_a\)) is given as \(1.8 \times 10^{-5}\). --- This problem is designed to test your understanding of buffer solutions and the use of the Henderson-Hasselbalch equation to calculate the amounts needed to achieve a certain pH in a buffer solution. Make sure to review the concepts of weak acids, bases, and the relationship between pH, pKa, and the concentrations of acid and its conjugate base in a solution.
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