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

Using Henry's Law Formula, the solubility of a given gas can be calculated. 

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)

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 x 10–4 M•atm–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?

Practice: At 0ºC and 1.00 atm, as much as 0.84 g of O2 can dissolve in 1.0 L of water. At 0ºC 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 x 10-5 M/atm.