Solubility of CH₃COOH decreases in presence of CH₃COONa due to:

Correct option is A

The correct answer is: (A) Common ion effect

Explanation:

• The solubility of acetic acid (CH₃COOH) decreases in the presence of sodium acetate (CH₃COONa) due to the common ion effect.
• Both compounds release the acetate ion (CH₃COO⁻) in solution.
• The excess of the common ion (CH₃COO⁻) from sodium acetate suppresses the ionization of acetic acid, thereby reducing its solubility.

Information Booster:

• The common ion effect is an application of Le Chatelier’s Principle.
• It is observed when a weak electrolyte and a strong electrolyte share a common ion.
• Acetic acid is a weak acid, and sodium acetate is a strong electrolyte.
• The pH of the solution increases due to reduced H⁺ ion concentration.
• This principle is widely used in buffer preparation and salt analysis.

Additional Information:

• Increased temperature generally increases solubility, not decreases it.
• Ion pairing refers to attraction between oppositely charged ions, not relevant here.
• Oxidation involves electron loss; acetic acid is not oxidized in this context.