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Chapter 13: Problem 33

A beaker of water is initially saturated with dissolved air. Explain what happens when He gas at \(1 \mathrm{~atm}\) is bubbled through the solution for a long time.

Short Answer

Expert verified
When helium gas is bubbled through the water, the water, despite being saturated with air, will start to dissolve the helium gas. This is because the water's saturation applies to the air, not the helium. The amount of helium dissolved will be determined by its partial pressure and the nature of helium's solubility in water.

Step by step solution

01

Grasp the Initial Situation.

The beaker is initially filled with water which is saturated with dissolved air. Saturated means that the water has absorbed all the air it can under the given conditions, so no more air can dissolve in the water under those conditions.
02

Understand the Implication of He Gas,

When bubbles of He (helium) gas at 1 atm are passed through the water, this introduces another gas to the system. According to Henry's law, the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the liquid's surface. In simpler terms, the greater the pressure of the gas above the liquid, the more of it will dissolve into the liquid.
03

Deduct the Outcome of Interaction

Even though the water is already saturated with air, because helium is a different gas, it will begin to dissolve into the water. The quantity of helium that dissolves will be determined by its partial pressure and the nature of helium itself in terms of its solubility in water. So, even though the water is saturated with air, it can still dissolve other gases like helium, particularly when they are introduced under pressure.

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Most popular questions from this chapter

Acetic acid is a weak acid that ionizes in solution as follows: $$ \mathrm{CH}_{3} \mathrm{COOH}(a q) \rightleftharpoons \mathrm{CH}_{3} \mathrm{COO}^{-}(a q)+\mathrm{H}^{+}(a q) $$ If the freezing point of a \(0.106 \mathrm{~m} \mathrm{CH}_{3} \mathrm{COOH}\) solution is \(-0.203^{\circ} \mathrm{C},\) calculate the percent of the acid that has undergone ionization.

Liquids A (molar mass \(100 \mathrm{~g} / \mathrm{mol}\) ) and \(\mathrm{B}\) (molar mass \(110 \mathrm{~g} / \mathrm{mol}\) ) form an ideal solution. At \(55^{\circ} \mathrm{C}\), A has a vapor pressure of \(95 \mathrm{mmHg}\) and \(\mathrm{B}\) has a vapor pressure of \(42 \mathrm{mmHg}\). A solution is prepared by mixing equal masses of \(\mathrm{A}\) and \(\mathrm{B}\). (a) Calculate the mole fraction of each component in the solution. (b) Calculate the partial pressures of \(\mathrm{A}\) and \(\mathrm{B}\) over the solution at \(55^{\circ} \mathrm{C}\). (c) Suppose that some of the vapor described in (b) is condensed to a liquid. Calculate the mole fraction of each component in this liquid and the vapor pressure of each component above this liquid at \(55^{\circ} \mathrm{C}\).

Define boiling-point elevation and freezing-point depression. Write the equations relating boilingpoint elevation and freezing-point depression to the concentration of the solution. Define all the terms, and give their units.

A \(262-\mathrm{mL}\) sample of a sugar solution containing \(1.22 \mathrm{~g}\) of the sugar has an osmotic pressure of 30.3 \(\mathrm{mmHg}\) at \(35^{\circ} \mathrm{C}\). What is the molar mass of the sugar?

Give two examples of a volatile liquid and two examples of a nonvolatile liquid.
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