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:
The partial pressure of O2 in air at sea level is 0.21 atm . The solubility of O2 in water at 20 oC , at 1 atm gas pressure, is 1.38 10-3  M (from Table 13.1 in your textbook).
Using Henrys law and the data in the introduction, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 oC and an atmospheric pressure of 670 torr .

Solution: The partial pressure of O2 in air at sea level is 0.21 atm . The solubility of O2 in water at 20 oC , at 1 atm gas pressure, is 1.38 10-3  M (from Table 13.1 in your textbook).Using Henrys law and the

Problem

The partial pressure of O2 in air at sea level is 0.21 atm . The solubility of O2 in water at 20 oC , at 1 atm gas pressure, is 1.38 10-3  M (from Table 13.1 in your textbook).

Using Henrys law and the data in the introduction, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 oC and an atmospheric pressure of 670 torr .