If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the

If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the freezing point depression?

If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the freezing point depression?

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.
Step 6: Calculate the result: ΔTf = 1.86 °C.

Freezing Point Depression – The decrease in the freezing point of a solvent when a solute is added, calculated using the formula ΔTf = i * Kf * m.
Colligative Properties – Properties that depend on the number of solute particles in a solution, not their identity.
Non-Electrolyte Behavior – Non-electrolytes do not dissociate into ions in solution, hence the van 't Hoff factor (i) is 1.