Frequently Asked Questions
What is molality and how is it different from molarity?
Molality (m) = moles of solute / kilograms of solvent. Molarity (M) = moles of solute / liters of solution. The key difference: molality uses mass of solvent (not volume of solution) and does not change with temperature. Molarity changes slightly when solutions expand or contract with temperature. This is why molality is preferred for colligative property calculations.
What is boiling point elevation?
Dissolving a non-volatile solute raises the boiling point of a solvent by delta_Tb = i x Kb x m, where i is the van't Hoff factor (number of particles per formula unit), Kb is the ebullioscopic constant of the solvent (0.512 degrees C kg/mol for water), and m is molality. Adding 1 mol of NaCl (i=2) to 1 kg of water raises the boiling point by about 1.02 degrees C.
What is the van't Hoff factor?
The van't Hoff factor (i) accounts for the number of particles a solute dissociates into. Non-electrolytes like glucose: i = 1. Strong electrolytes: NaCl = 2 (Na+ and Cl-), MgCl2 = 3, AlCl3 = 4. Ion pairing at higher concentrations causes i to be slightly less than the theoretical value. For colligative properties, all particles count equally regardless of charge.
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