Chem-To-Go Lesson 37 Unit 9 COLLIGATIVE PROPERTIES
DEFINITION: a physical property of a solution that differs from the physical property of the solvent due to the presence of the solute particles; the number of solute particles determines the severity of the property’s change BOILING POINT ELEVATION The boiling point of a solution will be higher than the normal boiling point of the solvent. EXAMPLE: Salt water boils at a higher temperature than pure water. FREEZING POINT DEPRESSION The freezing point of a solution will be lower than the normal freezing point of the solvent. EXAMPLE: Salt water freezes at a lower temperature than pure water.
IONIC SOLUTES Ionic solutes dissociate as they dissolve creating MORE solute particles. COVALENT SOLUTES Covalent solutes do not dissociate as they dissolve. NUMBER OF SOLUTE PARTICLES
∆T f = K f m i ∆T f = change in freezing pt. K f = freezing point constant for the solvent (will be given) m = molality i = number of ions present in solute (USE ONLY WITH IONIC SOLUTES) FREEZING POINT DEPRESSION K f of water = 1.86°C/m What is the new freezing point when 15.0g NaCl is dissolved into 200 mL of water?
∆T b = K b m i ∆T b = change in boiling pt. K b = boiling point constant for the solvent (will be given) m = molality i = number of ions present in solute (USE ONLY WITH IONIC SOLUTES) BOILING POINT ELEVATION K b of water = 0.52°C/m What is the new boiling point when 15.0g NaCl is dissolved into 200 mL of water?
CIVIL ENGINEERING APPLICATION: How many grams of NaCl would need to be added to the water to change the freezing temperature of 200 mL to -8°C? MORE ADVANCED EXAMPLE