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Chapter 13: Problem 36

Indicate whether each statement is true or false: (a) If you compare the solubility of a gas in water at two different temperatures, you find the gas is more soluble at the lower temperature. (b) The solubility of most ionic solids in water decreases as the temperature of the solution increases. (c) The solubility of most gases in water decreases as the temperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised. (d) Some ionic solids become less soluble in water as the temperature is raised.

Short Answer

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(a) True: Gas solubility increases at lower temperatures due to Le Chatelier's principle. (b) False: Most ionic solids have increased solubility at higher temperatures. (c) True: Gas solubility decreases at higher temperatures due to breaking of hydrogen bonds. (d) True: Some ionic solids become less soluble at higher temperatures if the dissolution process is exothermic.

Step by step solution

01

Statement (a) states that if you compare the solubility of a gas in water at two different temperatures, you find the gas is more soluble at the lower temperature. This statement is true, due to a principle called Le Chatelier's principle. When the temperature is lowered, the solubility of a gas in water increases because the exothermic dissolution process is favored. #b-tag_title# Determine the truth of statement (b) about solubility of most ionic solids

Statement (b) states that the solubility of most ionic solids in water decreases as the temperature of the solution increases. This statement is false. In fact, the solubility of most ionic solids in water increases as the temperature of the solution increases. This is because an increase in temperature provides more kinetic energy to the solution, allowing for the lattice energy of the ionic solid to be overcome more easily, leading to increased solubility. #c-tag_title# Determine the truth of statement (c) about solubility of gases in water and hydrogen bonding
02

Statement (c) states that the solubility of most gases in water decreases as the temperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised. This statement is true. As the temperature increases, the kinetic energy of the water molecules also increases, causing them to break their hydrogen bonds with the gas molecules. This results in a decrease in gas solubility at higher temperatures. #d-tag_title# Determine the truth of statement (d) about solubility of some ionic solids at higher temperatures

Statement (d) states that some ionic solids become less soluble in water as the temperature is raised. This statement is true. While most ionic solids become more soluble in water at higher temperatures, there are a few exceptions where the solubility decreases. This occurs when the dissolution process is exothermic (releases heat), and according to Le Chatelier's principle, increasing the temperature would shift the equilibrium to favor the reverse, undissolved state.

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Most popular questions from this chapter

The solubility of \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3} \cdot 9 \mathrm{H}_{2} \mathrm{O}\) in water is 208 \(\mathrm{g}\) per 100 \(\mathrm{g}\) of water at \(15^{\circ} \mathrm{C}\) . A solution of \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3} \cdot 9 \mathrm{H}_{2} \mathrm{O}\) in water at \(35^{\circ} \mathrm{C}\) is formed by dissolving 324 \(\mathrm{g}\) in 100 \(\mathrm{g}\) of water. When this solution is slowly cooled to \(15^{\circ} \mathrm{C},\) no precipitate forms. (a) Is the solution that has cooled down to \(15^{\circ}\) Cunsaturated, saturated, or supersaturated? (b) You take a metal spatula and scratch the side of the glass vessel that contains this cooled solution, and crystals start to appear. What has just happened? (c) At equilibrium, what mass of crystals do you expect to form?

A sulfuric acid solution containing 571.6 \(\mathrm{g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) per liter of solution has a density of 1.329 \(\mathrm{g} / \mathrm{cm}^{3} .\) Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, ( \mathbf{d} ) ~ t h e ~ m o l a r i t y ~ o f ~ \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in this solution.

If you compare the solubilities of the noble gases in water, you find that solubility increases from smallest atomic weight to largest, Ar \(<\mathrm{Kr}<\mathrm{Xe} .\) 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.

Aerosols are important components of the atmosphere. Does the presence of aerosols in the atmosphere increase or decrease the amount of sunlight that arrives at the Earth's surface, compared to an "aerosol-free" atmosphere? Explain your reasoning.

Calculate the molarity of the following aqueous solutions: (a) 0.540 \(\mathrm{g}\) of Mg \(\left(\mathrm{NO}_{3}\right)_{2}\) in 250.0 \(\mathrm{mL}\) of solution, \((\mathbf{b}) 22.4 \mathrm{gof}\) \(\mathrm{LiClO}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O}\) in 125 \(\mathrm{mL}\) of solution, \((\mathrm{c}) 25.0 \mathrm{mL}\) of 3.50 \(\mathrm{M}\) \(\mathrm{HNO}_{3}\) diluted to 0.250 \(\mathrm{L}\)
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