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Chapter 12: Problem 87

What effect does increasing pressure have on the solubility of gaseous solutes? Explain your answer.

Short Answer

Expert verified
Increasing pressure has a direct positive effect on the solubility of gaseous solutes, as described by Henry's Law (\( C = kP \)). Higher pressure causes more gas molecules to dissolve into the liquid, resulting in a higher concentration of dissolved gas. Therefore, higher pressure leads to higher solubility for gaseous solutes.

Step by step solution

01

Understand Henry's Law

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. Mathematically, it can be expressed as: \[ C = kP \] Where: - \(C\) is the solubility (molar concentration) of the gas in the liquid - \(k\) is a constant specific to the solute-solvent system (Henry's Law Constant) - \(P\) is the partial pressure of the gas above the liquid
02

Explain the Pressure-Solubility Relationship

The relationship between pressure and solubility, as described by Henry's Law, implies that when the pressure above the liquid is increased, the solubility of the gaseous solute in the liquid will also increase. This occurs because an increase in pressure causes more gas molecules to dissolve into the liquid and reach an equilibrium between the dissolved and undissolved states, resulting in a higher concentration of dissolved gas in the liquid.
03

The Effect of Increasing Pressure on Solubility

In conclusion, according to Henry's Law, increasing pressure has a direct positive effect on the solubility of gaseous solutes. As the pressure above the liquid increases, more gas molecules dissolve into the liquid phase, leading to a higher concentration of dissolved gas. So, higher pressure results in higher solubility for gaseous solutes.

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Most popular questions from this chapter

Propionic acid has one acidic proton per molecule. A solution is prepared by dissolving \(0.273 \mathrm{~g}\) of propionic acid in enough water to yield \(100.0 \mathrm{~mL}\) of solution. This solution is neutralized by \(36.82 \mathrm{~mL}\) of \(0.1001 \mathrm{M} \mathrm{NaOH}(a q)\). (a) What is the molar concentration of the propionic acid? (b) What is the molar mass of propionic acid?

Suppose \(250.0 \mathrm{~mL}\) of a \(0.600 \mathrm{M}\) solution of barium nitrate is combined with enough \(0.500 \mathrm{M}\) sodium sulfate solution to precipitate the maximum amount of barium sulfate. What volume of the sodium sulfate solution is required?

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(a) How many grams of \(\mathrm{NaOH}\) are needed to prepare \(500.0 \mathrm{~mL}\) of a \(0.300 \mathrm{M} \mathrm{NaOH}\) solution? (b) Describe how you would make this solution, including the equipment needed.
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