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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)

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Henry's Law Calculations

Concept #1: Henry's Law Formula

Example #1: Calculate the solubility of carbon dioxide gas, CO2, when its Henry’s Law Constant is 8.20 x 102 M/atm at 3.29 atm?

Concept #2: Henry’s Law (2 Point Form)

The 2 Point Form of Henry's Law Formula is used when dealing with 2 pressures and 2 solubilities of a given gas.

Example #2: At a pressure of 2.88 atm the solubility of dichloromethane, CH2Cl2, is 0.384 mg/L. If the solubility decreases to 0.225 mg/L, what is the new pressure?

Practice: Henry’s Law Constant for nitrogen in water is 1.67 × 10-4 M • atm–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?

Practice: At 0°C and 1.00 atm, as much as 0.84 g of O2 can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O2 dissolve in 1.0 L of water?

Practice: The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry’s Law Constant for oxygen in water at this temperature is 5.3 × 10–5 M/atm.