
11. Larutan berikut yang mempunyai titik beku terendah adalah larutan.. A. 0,1 mol urea dalam 1000 gram air

B. 0,1 gram natrium klorida (M = 58,5) dalam 1000 gram air C. 0,2 gram glukosa dalam (M1 = 180) dalam 500 gram air

D. 0,09 mol urea dalam 500

air gram

009

E.

500

1,0 gram glukosa (M, = 180) dalam 1000

01

2.169 (berbandin

gram air

sekitar 5,4 molal. 

To determine which solution has the lowest freezing point, we need to apply the concept of **freezing point depression**. The freezing point of a solution is lower than that of the pure solvent, and the amount by which the freezing point is lowered depends on the molality of the solution and the number of particles the solute dissociates into.

### Freezing Point Depression Formula:
\[
\Delta T_f = i \cdot K_f \cdot m
\]
- \(\Delta T_f\) is the freezing point depression.
- \(i\) is the van 't Hoff factor (the number of particles the solute dissociates into).
- \(K_f\) is the cryoscopic constant (a property of the solvent).
- \(m\) is the molality of the solution (moles of solute per kilogram of solvent).

### Analyzing Each Option:
1. **Option A:** \(0.1 \, \text{mol urea in 1000 grams of water}\)
   - Urea does not dissociate, so \(i = 1\).
   - Molality \(m = \frac{0.1 \, \text{mol}}{1 \, \text{kg}} = 0.1 \, \text{mol/kg}\).
   - \(\Delta T_f = 1 \cdot K_f \cdot 0.1 \, \text{mol/kg} = 0.1 K_f\).

2. **

Explore the concept of freezing point depression in solutions by analyzing different scenarios. Learn how to determine the solution with the lowest freezing point using key formulas and principles of colligative properties. Suitable for high school students studying chemistry.

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