At 25$^\circ$C, the highest osmotic pressure is exhibited by 0.1 M solution of

Question

Which one of the following is not correct for an ideal solution?

Answer 1

To determine which 0.1 M solution exhibits the highest osmotic pressure at 25^\circC, we need to analyze the concept of osmotic pressure.

Osmotic pressure ($\Pi$) is given by the formula:

\Pi = iCRT

i = van 't Hoff factor (number of particles the solute dissociates into)
C = molarity of the solution
R = universal gas constant
T = temperature in Kelvin

Given that the molarity ($C$) and temperature ($T$) are constant for each solution, the osmotic pressure is directly proportional to the van 't Hoff factor ($i$).

For CaCl_2, it dissociates into 3 ions: 1 Ca²⁺ and 2 Cl⁻, hence i = 3.
For KCl, it dissociates into 2 ions: 1 K⁺ and 1 Cl⁻, hence i = 2.
Glucose and urea are non-electrolytes, meaning they do not dissociate into ions. Both have i = 1.

Since osmotic pressure is highest for solutions with the highest van 't Hoff factor, CaCl_2 would normally exhibit the highest osmotic pressure because it has an $i$ value of 3.

However, the provided correct answer is urea, suggesting a problem in either the question or its provided answer. Assuming the answer you're given is correct under specific constraints not mentioned here, the logic typically would not support that conclusion based on provided options and standard chemical behavior.

Answer 2

To determine which 0.1 M solution exhibits the highest osmotic pressure at 25^\circC, we need to analyze the concept of osmotic pressure.

Osmotic pressure ($\Pi$) is given by the formula:

\Pi = iCRT

i = van 't Hoff factor (number of particles the solute dissociates into)
C = molarity of the solution
R = universal gas constant
T = temperature in Kelvin

Given that the molarity ($C$) and temperature ($T$) are constant for each solution, the osmotic pressure is directly proportional to the van 't Hoff factor ($i$).

For CaCl_2, it dissociates into 3 ions: 1 Ca²⁺ and 2 Cl⁻, hence i = 3.
For KCl, it dissociates into 2 ions: 1 K⁺ and 1 Cl⁻, hence i = 2.
Glucose and urea are non-electrolytes, meaning they do not dissociate into ions. Both have i = 1.

Since osmotic pressure is highest for solutions with the highest van 't Hoff factor, CaCl_2 would normally exhibit the highest osmotic pressure because it has an $i$ value of 3.

However, the provided correct answer is urea, suggesting a problem in either the question or its provided answer. Assuming the answer you're given is correct under specific constraints not mentioned here, the logic typically would not support that conclusion based on provided options and standard chemical behavior.

At 25$^\circ$C, the highest osmotic pressure is exhibited by 0.1 M solution of

The Correct Option is D

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