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: Calculate the freezing point of a aqueous solution of K2SO4,Calculate the freezing point of a 0.100 m aqueous solution of K2SO4, taking interionic attractions into consideration by using the vant Hoff

Solution: Calculate the freezing point of a aqueous solution of K2SO4,Calculate the freezing point of a 0.100 m aqueous solution of K2SO4, taking interionic attractions into consideration by using the vant Hoff

Problem

Calculate the freezing point of a aqueous solution of K2SO4,

Calculate the freezing point of a 0.100 m aqueous solution of K2SO4, taking interionic attractions into consideration by using the vant Hoff factor (i for 0.100 m K2SO4 = 2.32).

Solution

We’re being asked to determine the freezing point of an aqueous K2SO4solution. Aqueous means that K2SO4 was dissolved in water.


When calculating the freezing point of a solution, we’re going to use the Freezing Point Depression equation


Freezing Point Depression:

ΔTf =i·Kf·m 

where 

ΔTf = change in freezing point = Tf pure solvent  - Tf solvent

Kf = freezing point depression constant

i = van't Hoff factor of the solute = no. of ions

m = molality

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