Chapter 13: Problem 27
Discuss the factors that influence the solubility of a gas in a liquid.
Short Answer
Expert verified
Solubility of a gas in a liquid is influenced by temperature, pressure, the nature of the gas and liquid, and the presence of other solutes.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Temperature Effect on Gas Solubility
Temperature plays a significant role in determining the solubility of a gas in a liquid. Typically, gas solubility decreases as the temperature increases.
This is because higher temperatures give rise to increased kinetic energy among gas molecules, encouraging them to escape into the air rather than staying dissolved.
Consequently, cooler liquids tend to retain more dissolved gas compared to warmer ones.
This is because higher temperatures give rise to increased kinetic energy among gas molecules, encouraging them to escape into the air rather than staying dissolved.
Consequently, cooler liquids tend to retain more dissolved gas compared to warmer ones.
- This behavior is essential in understanding why carbonated drinks become "flat" when left out at room temperature: the gas dissolves less effectively.
- In aquatic environments, warmer water temperatures can lead to decreased oxygen levels, posing a threat to fish and other marine life.
Pressure and Gas Solubility
Pressure has a direct impact on how much gas can dissolve in a liquid. As pressure above a liquid increases, more gas molecules are forced into the solution, enhancing gas solubility.
This concept is crucial in various industries. For example, in carbonated beverage production, carbon dioxide is dissolved in the liquid under high pressures.
When you open the bottle, the pressure is lowered, and the gas escapes, creating bubbles.
This concept is crucial in various industries. For example, in carbonated beverage production, carbon dioxide is dissolved in the liquid under high pressures.
When you open the bottle, the pressure is lowered, and the gas escapes, creating bubbles.
- Higher pressure conditions yield greater gas solubility.
- The pressure-solubility relationship is pivotal to processes such as scuba diving, where changes in pressure can affect gas dissolution in the blood.
Henry's Law
Henry's Law provides a quantitative relationship between gas pressure and solubility. This law states that the amount of dissolved gas in a liquid is directly proportional to the gas's partial pressure over the liquid.
So, when the pressure increases, the amount of gas that can be dissolved also increases. Mathematically, it is expressed as:
\[ C = kP \]
Where \( C \) is the concentration of the dissolved gas, \( k \) is Henry's law constant, and \( P \) is the partial pressure of the gas.
So, when the pressure increases, the amount of gas that can be dissolved also increases. Mathematically, it is expressed as:
\[ C = kP \]
Where \( C \) is the concentration of the dissolved gas, \( k \) is Henry's law constant, and \( P \) is the partial pressure of the gas.
- This law helps predict how gases will behave under different pressure and temperature conditions.
- It is crucial for designing industrial processes involving gas absorption and purification.
Polarity and Solubility
The solubility of gases is also influenced by the polarity of both the gas and the solvent. Polar gases dissolve more easily in polar solvents due to the strong interactions between similar charges.
In contrast, non-polar gases find non-polar solvents more accommodating. This principle is encapsulated in the famous saying: "like dissolves like."
The solubility behavior can be attributed to intermolecular forces, such as hydrogen bonding in polar substances.
In contrast, non-polar gases find non-polar solvents more accommodating. This principle is encapsulated in the famous saying: "like dissolves like."
The solubility behavior can be attributed to intermolecular forces, such as hydrogen bonding in polar substances.
- Polar gases like ammonia mix well with polar liquids like water.
- Non-polar gases like methane prefer non-polar solvents like benzene.
- Understanding polarity is essential in applications ranging from pharmaceuticals to environmental science.
Salting-Out Effect
The salting-out effect is a phenomenon where the solubility of a gas in a liquid is reduced by the presence of salts or other solutes in the solution.
Adding salt to water decreases the water's ability to dissolve gases. This happens because ions from the salt attract water molecules, leaving fewer water molecules available to interact with gas molecules.
As a result, gases are "squeezed out" of the solution.
Adding salt to water decreases the water's ability to dissolve gases. This happens because ions from the salt attract water molecules, leaving fewer water molecules available to interact with gas molecules.
As a result, gases are "squeezed out" of the solution.
- This effect affects industrial gas purification processes.
- It is common in chemical and environmental engineering, where solute presence can significantly alter gas dissolution rates.
- In some cases, controlling the salting-out effect can be useful for removing unwanted gases from liquids.
