CHEM 001 Lecture Notes - Lecture 30: Boiling-Point Elevation, Freezing-Point Depression, Osmotic Pressure
Document Summary
Colligative properties: boiling point elevation for volatile solutes. A. boiling point elevation can only be applied to nonvolatile solutes, not volatile solutes. Because volatile solutes can increase (or decrease) vapor pressure and thus decrease (or increase) boiling point, respectively which obviously isn"t a fucking elevation. C. however, i f you know the heat of solution, predictions can be made on what will happen to the boiling point when volatile solutes are added, Endothermic ( positive) heat of solution: weaker bonds higher vapor pressure decreased boiling point. Exothermic ( negative) heat of solution: stronger bonds lower vapor pressure increased boiling point. B. impurities (the solute) interrupt the crystal lattice and lower the freezing point by fucking up the ability of the dipoles to neatly arrange. C. equation ( for an ideally dilute solution): t = kfmi. 2 . kf = specific constant of the substance being frozen. 3 . m = molality not molarity or mass.