Ch.12 - SolutionsWorksheetSee all chapters
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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 freezing-point depression of a 0.091-m solution of CsCl is 0.320˚C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440˚C. In which solution does ion association appear to be gre

Solution: The freezing-point depression of a 0.091-m solution of CsCl is 0.320˚C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440˚C. In which solution does ion association appear to be gre

Problem

The freezing-point depression of a 0.091-m solution of CsCl is 0.320˚C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440˚C. In which solution does ion association appear to be greater? Explain.

Solution

The problem asks us to find which solution has a greater ion association using freezing point depression data. We can determine which has a greater ion association indirectly from the  Van’t Hoff factor The Van’t Hoff factor is the number of ions created once the compound dissociates. A higher Van't Hoff factor means greater dissociation and lesser association. Inversely, a lower Van't Hoff factor means greater ion association.


The freezing point depression equation is:


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