- Ch.1 - Matter, Measurement & Problem Solving106
- Ch.2 - Atoms & Elements97
- Ch.3 - Molecules, Compounds & Chemical Equations134
- Ch.4 - Chemical Quantities & Aqueous Reactions115
- Ch.5 - Gases98
- Ch.6 - Thermochemistry84
- Ch.7 - Quantum-Mechanical Model of the Atom49
- Ch.8 - Periodic Properties of the Elements81
- Ch.9 - Chemical Bonding I: The Lewis Model79
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory78
- Ch.11 - Liquids, Solids & Intermolecular Forces41
- Ch.12 - Solids and Modern Material35
- Ch.13 - Solutions66
- Ch.14 - Chemical Kinetics83
- Ch.15 - Chemical Equilibrium52
- Ch.16 - Acids and Bases107
- Ch.17 - Aqueous Ionic Equilibrium130
- Ch.18 - Free Energy and Thermodynamics74
- Ch.19 - Electrochemistry87
- Ch.20 - Radioactivity and Nuclear Chemistry50
- Ch.21 - Organic Chemistry143
Chapter 13, Problem 87b
Calculate the freezing point and boiling point of each aqueous solution, assuming complete dissociation of the solute. b. 21.5 g of CuCl2 in 4.50⨉102 g water
Video transcript
A solution contains 50.0 g of heptane (C7H16) and 50.0 g of octane (C8H18) at 25 °C. The vapor pressures of pure heptane and pure octane at 25 °C are 45.8 torr and 10.9 torr, respectively. Assuming ideal behavior, answer the following: d. Why is the composition of the vapor different from the composition of the solution?
A solution contains a mixture of pentane and hexane at room temperature. The solution has a vapor pressure of 258 torr. Pure pentane and hexane have vapor pressures of 425 torr and 151 torr, respectively, at room temperature. What is the mole fraction composition of the mixture? (Assume ideal behavior.)
A glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the freezing point and boiling point of the solution.
Calculate the freezing point and boiling point of each aqueous solution, assuming complete dissociation of the solute. c. 5.5% NaNO3 by mass (in water)
What mass of salt (NaCl) should you add to 1.00 L of water in an ice cream maker to make a solution that freezes at -10.0 °C? Assume complete dissociation of the NaCl and density of 1.00 g>mL for water.
Use the van't Hoff factors in Table 13.9 to calculate each colligative property: a. the melting point of a 0.100 m iron(III) chloride solution