If 1 mole of a non-volatile solute is dissolved in 1 kg of water, what is the expected change in boiling point? (Kb for water = 0.512 °C kg/mol)
Practice Questions
1 question
Q1
If 1 mole of a non-volatile solute is dissolved in 1 kg of water, what is the expected change in boiling point? (Kb for water = 0.512 °C kg/mol)
0.512 °C
1.024 °C
2.048 °C
0.256 °C
Boiling point elevation = i * Kb * m = 1 * 0.512 * 1 = 0.512 °C.
Questions & Step-by-step Solutions
1 item
Q
Q: If 1 mole of a non-volatile solute is dissolved in 1 kg of water, what is the expected change in boiling point? (Kb for water = 0.512 °C kg/mol)
Solution: Boiling point elevation = i * Kb * m = 1 * 0.512 * 1 = 0.512 °C.
Steps: 6
Step 1: Understand that we are calculating the change in boiling point when a solute is added to a solvent (water).
Step 2: Identify the formula for boiling point elevation: ΔT = i * Kb * m.
Step 3: Determine the values needed for the formula: i (van 't Hoff factor) = 1 for a non-volatile solute, Kb (boiling point elevation constant for water) = 0.512 °C kg/mol, and m (molality) = 1 mole of solute in 1 kg of water.
Step 4: Plug the values into the formula: ΔT = 1 * 0.512 * 1.
Step 5: Calculate the result: ΔT = 0.512 °C.
Step 6: Conclude that the expected change in boiling point is 0.512 °C.
