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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: When 13.62 g (about one tablespoon) of table sugar (sucrose, C12H22O11) is dissolved in 241.5 mL of water (density 0.997 g/mL), the final volume is 250.0 mL (about one cup).Would the syrup freeze in a typical freezer (-18 C)? Why or why not?

Solution: When 13.62 g (about one tablespoon) of table sugar (sucrose, C12H22O11) is dissolved in 241.5 mL of water (density 0.997 g/mL), the final volume is 250.0 mL (about one cup).Would the syrup freeze in a

Problem

When 13.62 g (about one tablespoon) of table sugar (sucrose, C12H22O11) is dissolved in 241.5 mL of water (density 0.997 g/mL), the final volume is 250.0 mL (about one cup).

Would the syrup freeze in a typical freezer (-18 C)? Why or why not?

Solution

We’re being asked to determine whether a syrup freezes at a typical freezer (-18°C).


The syrup is prepared by dissolving 13.62 g of table sugar (sucrose, C12H22O11) in 241.5 mL of water for which the final volume of the solution is 250.0 mL.


To answer this, we need to determine the freezing point of the solution and compare it to the temperature of a typical freezer. When calculating the freezing point of a solution, we’re going to use the equation for Freezing Point Depression.


Tf=i·Kf·m

∆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


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