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Calculate the pH of a 0.268M sodium acetate solution.

Calculate the pH of a 0.268M sodium acetate solution.

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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**Problem Statement:** Calculate the pH of a 0.268 M sodium acetate solution. --- **Explanation:** This task involves determining the pH of a sodium acetate solution using its concentration. Sodium acetate is a salt that can influence the pH of a solution when dissolved in water. Calculating the pH involves understanding the hydrolysis of acetate ions, which results in a basic solution. **Approach:** 1. **Write the chemical equation** for the hydrolysis of acetate ions (CH₃COO⁻). 2. **Use the ionization constant (Kₐ)** of acetic acid to find the base dissociation constant (K_b) for acetate ions. 3. **Set up the equilibrium expression** to find the concentration of hydroxide ions (OH⁻). 4. **Calculate the pH** from the pOH obtained. This is a standard problem in the study of acid-base chemistry, particularly in buffer solutions and salt hydrolysis.
Transcribed Image Text:**Problem Statement:** Calculate the pH of a 0.268 M sodium acetate solution. --- **Explanation:** This task involves determining the pH of a sodium acetate solution using its concentration. Sodium acetate is a salt that can influence the pH of a solution when dissolved in water. Calculating the pH involves understanding the hydrolysis of acetate ions, which results in a basic solution. **Approach:** 1. **Write the chemical equation** for the hydrolysis of acetate ions (CH₃COO⁻). 2. **Use the ionization constant (Kₐ)** of acetic acid to find the base dissociation constant (K_b) for acetate ions. 3. **Set up the equilibrium expression** to find the concentration of hydroxide ions (OH⁻). 4. **Calculate the pH** from the pOH obtained. This is a standard problem in the study of acid-base chemistry, particularly in buffer solutions and salt hydrolysis.
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