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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
Sections
Solutions: Solubility and Intermolecular Forces
Molality
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
Osmosis
Osmotic Pressure
Vapor Pressure Lowering (Raoult's Law)
Additional Guides
The Freezing Point Depression (IGNORE)
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Next SectionHenry's Law Calculations

According to Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase. 

Intro to Henry's Law 

Concept #1: Intro to Henry's Law Concept 1

Example #1: In general, as the temperature increases, the solubility of a gas in a given liquid _______, and the solubility of most solids in a given liquid _______.

Which of the following is true for the solubility of KBr (s) and CH3(CH2)3CH3 (g) in water?  

Previous SectionTypes of Aqueous Solutions
Next SectionHenry's Law Calculations