Question

Identify correct statements from following regarding \(0.2 \text{M}\) urea and \(0.2 \text{M}\) sucrose solutions.

• A. The urea solution is hypertonic to sucrose solution.
• B. The osmotic pressure of urea solution is higher than that of sucrose solution.
• C. These solutions exhibit same osmotic pressure.
• D. The sucrose solution is hypotonic to urea solution.

Hint:

Osmotic pressure depends on the number of particles, and both solutes are nonelectrolytes.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept:
Osmotic pressure is a colligative property: \(\pi = iCRT\). It depends on the concentration of dissolved particles, not on what they are.

Step 2: Key Formula or Approach:
Urea and sucrose are both molecular solutes that do not dissociate, so \(i = 1\) for each.

Step 3: Detailed Explanation:
Both solutions are \(0.2\) M and at the same temperature, so \(\pi_{urea} = \pi_{sucrose} = 0.2RT\).
Solutions with the same osmotic pressure are called isotonic.
Statements A and D call one solution hypertonic or hypotonic to the other, and statement B claims a higher pressure for urea. These need unequal osmotic pressures, so they are all false. Only statement C is correct.

Final Answer:
The two solutions have the same osmotic pressure, option (C). \[ \boxed{\text{Same osmotic pressure}} \]