Question

The relationship between the values of osmotic pressure of
0.1 M solutions of KNO₃(P₁) and CH₃COOH(P₂) is :
(a) P₁/P₁ + P₂ = P₂/P₁ + P₂
(b) P₁ > P₂
(d) P₂ > P₁ (d) P₁ = P₂

Answer 1

answer : option (b) P₁ > P₂

From Van't Hoff formula of osmotic pressure,

π = iCRT , i is Van't Hoff factor, C is concentration, R is universal gas constant and T is temperature in Kelvin.

here KNO3 is strong electrolyte so it dissociates 100% into aqueous solution while CH3COOH is weak acid so, it dissociates partially. then, i of KNO3 > i of CH3COOH

then, osmotic pressure of KNO3 > osmotic pressure of CH3COOH [ because C, R and T are same for both solutions]

hence, option (b) is correct choice.

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Answer 2

Answer:

Explanation:

π = iCRT , i is Van't Hoff factor, C is concentration, R is universal gas constant and T is temperature in Kelvin.

here KNO3 is strong electrolyte so it dissociates 100% into aqueous solution while CH3COOH is weak acid so, it dissociates partially. then, i of KNO3 > i of CH3COOH

then, osmotic pressure of KNO3 > osmotic pressure of CH3COOH [ because C, R and T are same for both solutions]

hence, option (b) is correct choice.

also read similar questions : For the reaction equilibrium, 2NOBr (g) 2NO (g) + Br2 (g), If PBr2 = P/9 at equilibrium and P is total pressure. The rat...