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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)

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Osmotic Pressure Calculations

Concept #1: Osmotic Pressure Formula

Example #1: Calculate the osmotic pressure of a solution containing 18.30 mg of ZnO in 15.1 mL of solution at 26ºC.

Practice: The osmotic pressure of blood is 5950.8 mmHg at 41°C. What mass of glucose, C6H12O6, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.

Practice: The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25°C. What is the molar mass of insulin? (1 atm = 760 torr)