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

Solution: What is the freezing point of an aqueous solution that boils at 104.6 °C?

Problem

What is the freezing point of an aqueous solution that boils at 104.6 °C?

Solution

We have to calculate the freezing point of an aqueous solution that boils at 104.6 °C.


When a nonvolatile solute is dissolved in a solvent, the freezing point of the resulting solution is always lower than the freezing point of pure solvent. This property of solutions is called the freezing point depression.

The formula for freezing point depression is:

Tf = i·Kf·m

Where,

ΔTf = change in freezing point

i = van ‘t Hoff constant (i = 1 for nonelectrolytes)

Kf =freezing point depression constant

m = molality of solution


When a nonvolatile solute is dissolved in a solvent, the boiling point of the resulting solution is always higher than the boiling point of pure solvent. This property of solutions is called the boiling point elevation.

The formula for boiling point elevation is:

Tb = i·Kb·m

Where,

ΔTb = change in boiling point

i = van ‘t Hoff constant (i = 1 for nonelectrolytes)

Kb = boiling point elevation constant

m = molality of solution

Solution BlurView Complete Written Solution