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calculate the pH

calculate the pH

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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**Title: Calculating pH with the Henderson-Hasselbalch Equation** **Instructions:** Use the Henderson-Hasselbalch equation to calculate the pH of each solution. **Explanation:** The Henderson-Hasselbalch equation is commonly used in chemistry to determine the pH of a buffer solution. It is expressed as: \[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] Where: - \(\text{pKa}\) is the acid dissociation constant. - \([\text{A}^-]\) is the concentration of the conjugate base. - \([\text{HA}]\) is the concentration of the acid. This formula relates the pH of a solution to the pKa and the ratio of the concentrations of the dissociated and undissociated forms of the acid present in the solution. It is especially useful for calculating the pH during the preparation of buffer solutions.
Transcribed Image Text:**Title: Calculating pH with the Henderson-Hasselbalch Equation** **Instructions:** Use the Henderson-Hasselbalch equation to calculate the pH of each solution. **Explanation:** The Henderson-Hasselbalch equation is commonly used in chemistry to determine the pH of a buffer solution. It is expressed as: \[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] Where: - \(\text{pKa}\) is the acid dissociation constant. - \([\text{A}^-]\) is the concentration of the conjugate base. - \([\text{HA}]\) is the concentration of the acid. This formula relates the pH of a solution to the pKa and the ratio of the concentrations of the dissociated and undissociated forms of the acid present in the solution. It is especially useful for calculating the pH during the preparation of buffer solutions.
**Part A** Consider a solution that is 0.190 M in HC₂H₃O₂ and 0.110 M in KC₂H₃O₂. **Task** Express your answer using two decimal places.
Transcribed Image Text:**Part A** Consider a solution that is 0.190 M in HC₂H₃O₂ and 0.110 M in KC₂H₃O₂. **Task** Express your answer using two decimal places.
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