Hydrolysis Of Salts

Step 1: For a salt of weak acid and weak base: Kh=(Kw)/(KₐKb)
Step 2: Kh=frac10⁻14(1.8×10⁻5)(1.8×10⁻5) =3.09×10⁻5
Step 3: Degree of hydrolysis: h=√(Kh)=√3.09×10⁻5 =5.56×10⁻3
Step 4: Percentage hydrolysis: %h = h×100 = 0.556%

Step 1: Understanding the Concept
Salt hydrolysis occurs when the ions of a salt react with water to produce acidity or alkalinity. This typically happens with salts derived from a weak acid or a weak base. Salts of strong acids and strong bases do not undergo hydrolysis and form neutral solutions.

Step 2: Detailed Explanation
1. Sodium acetate (CH COONa): Salt of a weak acid (Acetic acid) and a strong base (NaOH). The acetate ion ( ) undergoes anionic hydrolysis, making the solution basic. 2. Ammonium chloride (NH Cl): Salt of a strong acid (HCl) and a weak base (Ammonium hydroxide). The ammonium ion ( ) undergoes cationic hydrolysis, making the solution acidic. 3. Sodium carbonate (Na CO ): Salt of a weak acid (Carbonic acid) and a strong base (NaOH). It undergoes hydrolysis to form a basic solution. 4. Sodium chloride (NaCl): Salt of a strong acid (HCl) and a strong base (NaOH). Both and ions are spectator ions; they do not react with water.

Step 3: Final Answer
Sodium chloride does not undergo hydrolysis.