A solution of 0.1 molal urea in water has a freezing point depression of how much? (K_f for water = 1.86 °C kg/mol)
Practice Questions
1 question
Q1
A solution of 0.1 molal urea in water has a freezing point depression of how much? (K_f for water = 1.86 °C kg/mol)
0.186 °C
0.372 °C
0.186 K
0.372 K
Freezing point depression = K_f * m = 1.86 * 0.1 = 0.186 °C
Questions & Step-by-step Solutions
1 item
Q
Q: A solution of 0.1 molal urea in water has a freezing point depression of how much? (K_f for water = 1.86 °C kg/mol)
Solution: Freezing point depression = K_f * m = 1.86 * 0.1 = 0.186 °C
Steps: 6
Step 1: Identify the formula for freezing point depression, which is ΔT_f = K_f * m.
Step 2: Understand that ΔT_f is the change in freezing point, K_f is the freezing point depression constant for the solvent (water in this case), and m is the molality of the solution.
Step 3: Note the values given: K_f for water is 1.86 °C kg/mol and the molality (m) of urea is 0.1 molal.
Step 4: Plug the values into the formula: ΔT_f = 1.86 °C kg/mol * 0.1 mol/kg.
Step 5: Calculate the result: 1.86 * 0.1 = 0.186 °C.
Step 6: Conclude that the freezing point depression of the solution is 0.186 °C.
