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Ch.12 - SolutionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Solutions: Solubility and Intermolecular Forces
Parts per Million (ppm)
Mole Fraction
Solutions: Mass Percent
Types of Aqueous Solutions
Intro to Henry's Law
Henry's Law Calculations
The Colligative Properties
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure
Vapor Pressure Lowering (Raoult's Law)
Additional Guides
The Freezing Point Depression (IGNORE)
Jules Bruno

Boiling point elevation

Boiling point represents one of our four colligative properties

Boiling point elevation formula

The equation for boiling point elevation is i multiplied by kb multiplied by m. 

i represents your Van’t Hoff factor. That’s just the number of ions your solute will breakup into. If your solute is ionic, it breaks up into ions. If your solute is covalent, then it doesn't break up into ions at all; it stays intact so i equals 1. 

If you wanna take a closer look at the Van’t Hoff factor, make sure you take a look at our chapter videos and concept videos and see how we approach calculating the Van’t Hoff factor based on a specific solute given. 

Now we’re going to say that the lower case m is molality, which represents the moles of solute divided by kilograms of solvent. 

Kb represents the boiling point constant of our solvent. 

Below, I’ve provided some common types of solvents. We have water, benzene, chloroform and ethanol. You’re not expected to memorize all of their normal boiling points as well as their boiling point constants. But for water, I would recommend you memorize those. You should know that pure water boils at 100°Celsius. All you really have to remember other than that is that its boiling point constant is 0.51°Celsuis/molality. 

How to calculate boiling point

How do we apply this formula to figuring out the boiling point of a solution? We’re going to say that the boiling point of a solution equals the boiling point of the pure solvent plus my change in boiling point. Let’s say that we found that our change in our boiling point was equal to 0.7°C once we’ve plugged these variables in. We know that water boils at a temperature of 100°C. When I add solute to the pure solvent, the boiling point goes up that’s why it’s called boiling point elevation; there’s an increase in boiling point. I would just add my change in my boiling point temperature so it equals 100.7°C. That’d be the new boiling point of my solution. 


Remember, besides boiling point, we also have freezing point, osmotic pressure and Raoult’s Law, which deals with vapor pressure, as our three other colligative properties. Remember, the colligative properties help to explain what happens to a pure solvent as I add solute to it gradually over time. It causes changes in these four colligative properties. Make sure you take a look at our chapter videos and concept videos dealing with the colligative properties and the common types of problems that usually appear when discussing these four different types of properties.

Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.