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Ch.13 - Properties of Solutions
All textbooksBrown 14th EditionCh.13 - Properties of SolutionsProblem 4
Chapter 13, Problem 4

Which two statements about gas mixtures are true? [Section 13.1] (a) Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. (b) Just like water and oil don’t mix in the liquid phase, two gases can be immiscible and not mix in the gas phase. (c) If you cool a gaseous mixture, you will liquefy all the gases at the same temperature. (d) Gases mix in all proportions in part because the entropy of the system increases upon doing so.

Verified step by step guidance
1
Step 1: Understand the concept of gas mixtures. Gases tend to mix with each other due to their high kinetic energy and the large distances between particles, which minimize intermolecular forces.
Step 2: Evaluate statement (a). Consider the nature of gas particles and their interactions. Gases are generally able to mix because the particles are far apart, reducing the effect of intermolecular forces.
Step 3: Evaluate statement (b). Compare the behavior of gases to liquids like water and oil. Unlike liquids, gases do not have significant intermolecular forces that prevent mixing, so they are typically miscible.
Step 4: Evaluate statement (c). Consider the process of cooling a gas mixture. Different gases have different boiling points, so they do not liquefy at the same temperature.
Step 5: Evaluate statement (d). Consider the role of entropy in gas mixing. Mixing gases increases the disorder or entropy of the system, which is a driving force for mixing.
Related Practice
Open Question
A solution contains 0.115 mol H2O and an unknown number of moles of sodium chloride. The vapor pressure of the solution at 30 °C is 25.7 torr. The vapor pressure of pure water at this temperature is 31.8 torr. Calculate the number of grams of sodium chloride in the solution. (Hint: Remember that sodium chloride is a strong electrolyte.)
Textbook Question

This figure shows the interaction of a cation with surrounding water molecules. (b) Which of the following explanations accounts for the fact that the ion–solvent interaction is greater for Li+ than for K+? a. Li+ is of lower mass than K+. b. The ionization energy of Li is higher than that for K. c. Li+ has a smaller ionic radius than K+. d. Li has a lower density than K. e. Li reacts with water more slowly than K. [Section 13.1]

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Textbook Question

Consider two ionic solids, both composed of singly charged ions, that have different lattice energies. (b) If not, which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute–solvent interactions are the same for both solids. [Section 13.1]

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Open Question
The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. Assuming that the volumes of the solute and solvent are additive, what is the molarity of thiophene in the solution?
Open Question
If you compare the solubilities of the noble gases in water, you find that solubility increases from smallest atomic weight to largest, specifically: Ar < Kr < Xe. Which of the following statements is the best explanation? [Section 13.3] (a) The heavier the gas, the more it sinks to the bottom of the water and leaves room for more gas molecules at the top of the water. (b) The heavier the gas, the more dispersion forces it has, and therefore the more attractive interactions it has with water molecules. (c) The heavier the gas, the more likely it is to hydrogen-bond with water. (d) The heavier the gas, the more likely it is to make a saturated solution in water.
Textbook Question

The structures of vitamins E and B6 are shown below. Predict which is more water soluble and which is more fat soluble. [Section 13.3]

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