Which of the two has lower freezing point, 2m NaCl or 5m NaCl aqueous solution?a)2m NaCl solutionb)Both have same freezing pointc)5m NaCl solutiond)The solutions cannot freezeCorrect answer is option 'C'. Can you explain this answer?

Question

Answer

∆Tf=i×Kf×m   :. So 5m NaCl aqueous solution will have lower  freezing point

Answer

Because there colligative property is high  to 2m  solution

Answer

From colligative property we know,∆Tf is proportional to m(molality). Pure water solvent would have freezing point at 0 degree celcius. Now ∆Tf is more for 5m compared to 2m. Therefore freezing point is lower for 5m solution compared to 2m solution. Hence option C

Answer

Explanation:

The freezing point of a solution is influenced by the concentration of solute particles in the solution. According to Raoult's Law, the presence of a non-volatile solute lowers the freezing point of a solvent.

1. Raoult's Law:
According to Raoult's Law, the vapor pressure of a solvent above a solution is directly proportional to the mole fraction of the solvent in the solution. This law can be extended to the freezing point of a solution as well.

2. Freezing Point Depression:
Freezing point depression is a colligative property, which means it depends on the number of solute particles rather than their nature. The formula for freezing point depression is:

ΔTf = Kf × m
where ΔTf is the change in freezing point, Kf is the cryoscopic constant, and m is the molality of the solution.

3. Comparison:
In this case, we are comparing a 2m NaCl solution with a 5m NaCl solution. The molality of the solutions is different, which means the concentration of solute particles is different.

As per Raoult's Law and freezing point depression, a higher concentration of solute particles will lead to a greater decrease in the freezing point. Therefore, the 5m NaCl solution will have a lower freezing point compared to the 2m NaCl solution.

4. Conclusion:
Based on the above explanation, the correct answer is option 'C' - the 5m NaCl solution has a lower freezing point.

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