Clutch Prep is now a part of Pearson
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Solubility and Intermolecular Forces
Solutions: Mass Percent
Percent Concentrations
Parts per Million (ppm)
Solubility: Temperature Effect
Intro to Henry's Law
Henry's Law Calculations
Solution Stoichiometry
Electrolytes (Simplified)
The Colligative Properties
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Boiling Point Elevation Calculations

Concept #1: Boiling Point Elevation

Boiling Point of the solvent will increase with the addition of a solute.

Example #1: Calculate the boiling point of a 3.71 m aqueous CaBr2 solution.

Practice: An ethylene glycol solution contains 25.2 g of ethylene glycol (C2H6O2) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.

Practice: Pure water boils at 100ºC. What is the new boiling point of water after the addition of 13.12 g aluminum chloride, AlCl3, to 615 g water?

Practice: What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15ºC?

Practice: Carbon dioxide is dissolved in 722 mL of benzene with a density of 1.59 g/mL. What mass of carbon dioxide would you add to make the boiling point of the solution 104.7ºC?