Calculate the pH of 0.05 M sodium acetate solution if the p Ka of acetic acid is 4.74

Name: Problem 43, Chapter 11: Numerical problems in Physical Chemistry for IIT-JEE
Uploaded: 2021-11-22T05:06:46-08:00
Duration: 1 min 49 s
Channel: Himanshu Kushwaha
Description: Calculate the pH of 0.05 M sodium acetate solution if the p Ka of acetic acid is 4.74

step 1 In this question we have been given a solution of sodium acetate CH3 COONA and we have been give

Calculate the pH of 0.05 M sodium acetate solution if the p...

Key Concepts

Acid-Base Equilibrium

This concept deals with the dynamic balance between acids and bases in solution, where weak acids and bases only partially dissociate. It involves understanding how the acid dissociation constant (Ka) quantifies the extent of ionization of a weak acid and how its conjugate base behaves in water.

Salt Hydrolysis

Salt hydrolysis occurs when a salt derived from a weak acid (or weak base) reacts with water to produce hydroxide or hydronium ions, thereby altering the pH of the solution. This concept is crucial for determining the pH of solutions that are not neutral because the anion or cation undergoes a reaction with water.

Relationship between Ka and Kb

For a conjugate acid-base pair, the acid dissociation constant (Ka) and base dissociation constant (Kb) are interrelated through the water ionization constant (Kw). This relationship allows for the determination of the basicity of the conjugate base when the Ka of the weak acid is known, which is key to evaluating the pH of its salt solution.

pH Calculation in Weak Acid/Conjugate Base Solutions

Calculating pH in solutions involving weak acids and their conjugate bases often requires setting up an equilibrium expression that accounts for the hydrolysis reaction. Whether using the Henderson-Hasselbalch equation for buffer systems or deriving the pOH from the Kb value, this concept encompasses the steps necessary to quantitatively relate ion concentrations to the pH of the solution.

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