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

Solution: Urea is a common fertilizer with the formula CO(NH2)2 that is sometimes used as a chemical deicer for icy road surfaces in the winter months. Adding a solute to a solvent causes the freezing point to

Problem

Urea is a common fertilizer with the formula CO(NH2)2 that is sometimes used as a chemical deicer for icy road surfaces in the winter months. Adding a solute to a solvent causes the freezing point to be lowered and allows the solvent to remain liquid at lower temperatures. 

The value of Kf for water is 1.86°C/m, and its normal freezing point is 0.00°C, Urea is a nonvolatile nonelectrolyte solute. 

What molality of urea is required to lower the freezing point of ice water by 2.63°C? 

Part 2

Using your answer from Part 1, calculate the mass of urea that must be added to 427 mL of water (density 1.00 g/mL) to lower the freezing point by 2.63°C.