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: A 5 g sample of CaI2 is completely dissolved in 22 g of water, what is the freezing point of the solution? Assume complete dissociation of the salt. Kf for water is 1.86°C/m.

Solution: A 5 g sample of CaI2 is completely dissolved in 22 g of water, what is the freezing point of the solution? Assume complete dissociation of the salt. Kf for water is 1.86°C/m.

Problem

A 5 g sample of CaI2 is completely dissolved in 22 g of water, what is the freezing point of the solution? Assume complete dissociation of the salt. Kf for water is 1.86°C/m.

Solution

We’re being asked to find the freezing point of a solution when CaI2 is dissolved in water. When calculating the freezing point of a solution, we’re going to use the equation for Freezing Point Depression.


∆Tf = change in freezing point = Tf pure solvent –Tf solution
Kf = freezing point depression constant
i = van' t Hoff factor of the solute = no. of ions
m = molality


Let’s first calculate the molality of the solution.

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