If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the freezing point depression?
Practice Questions
1 question
Q1
If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the freezing point depression?
0 °C
1.86 °C
3.72 °C
5.58 °C
The freezing point depression is calculated using the formula ΔTf = i * Kf * m. For a non-electrolyte, i = 1, Kf for water = 1.86 °C kg/mol, and m = 1 mol/kg gives ΔTf = 1.86 °C.
Questions & Step-by-step Solutions
1 item
Q
Q: If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the freezing point depression?
Solution: The freezing point depression is calculated using the formula ΔTf = i * Kf * m. For a non-electrolyte, i = 1, Kf for water = 1.86 °C kg/mol, and m = 1 mol/kg gives ΔTf = 1.86 °C.
Steps: 6
Step 1: Understand the formula for freezing point depression, which is ΔTf = i * Kf * m.
Step 2: Identify the values needed for the formula. For a non-electrolyte solute, the van 't Hoff factor (i) is 1.
Step 3: Find the value of Kf for water, which is 1.86 °C kg/mol.
Step 4: Determine the molality (m) of the solution. Since 1 mole of solute is dissolved in 1 kg of water, m = 1 mol/kg.
Step 5: Plug the values into the formula: ΔTf = 1 * 1.86 °C kg/mol * 1 mol/kg.
