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Molar Mass and Freezing Point Depression

Molar Mass and Freezing Point Depression. Lab Prep. Key Points. It is the number of solute particles, not their identity, which determines the magnitude of the boiling-point elevation and freezing point depression.

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Molar Mass and Freezing Point Depression

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  1. Molar Mass and Freezing Point Depression Lab Prep

  2. Key Points • It is the number of solute particles, not their identity, which determines the magnitude of the boiling-point elevation and freezing point depression. • Properties based only on the number of solute particles and not their identity are known as colligative properties.

  3. Real World Applications • Antifreeze protects a car’s engine from heat and cold. • Salt is used in making ice cream and on highways and bridges because it depresses the freezing point.

  4. Molarity (M) • Number of moles of solute in one liter of solution M = mol solute/volume of solution (L) *Volume varies with temperature

  5. Molality (m) • Moles of solute per kg of solvent m = mol of solute/kg of solvent (mass) *Independent of temperature If the mass of the solvent is known then the moles of solute can be calculated: moles of solute = (m) (kg of solvent)

  6. Constants • Kf molal freezing point depression constant • Kb molal boiling point elevation constant • m = ΔTf / Kf

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