Textbook Question
Which of the following in each pair is likely to be more soluble in water: (c) HCl or ethyl chloride (CH3CH2Cl)? Explain in each case.
Ch.13 - Properties of Solutions
Chapter 13, Problem 36
Indicate whether each statement is true or false:(c) The solubility of most gases in water decreases as thetemperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised.
Verified step by step guidance1
Understand the relationship between gas solubility and temperature: Generally, the solubility of gases in liquids decreases with an increase in temperature.
Consider the kinetic energy of gas molecules: As temperature increases, the kinetic energy of gas molecules also increases, making them more likely to escape from the liquid into the gas phase.
Examine the role of hydrogen bonding: While water does form hydrogen bonds, the decrease in gas solubility with increasing temperature is primarily due to increased kinetic energy, not the breaking of hydrogen bonds.
Evaluate the statement: The statement suggests that the decrease in solubility is due to water breaking its hydrogen bonds with gas molecules, which is not the primary reason for decreased solubility.
Conclude the evaluation: Based on the understanding of gas solubility and temperature, the statement is false because the decrease in solubility is mainly due to increased kinetic energy, not the breaking of hydrogen bonds.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Gas Solubility in Liquids
The solubility of gases in liquids is influenced by temperature and pressure. Generally, as temperature increases, the kinetic energy of gas molecules also increases, leading to a decrease in solubility. This is because gas molecules are more likely to escape from the liquid phase into the gas phase at higher temperatures.
Recommended video:
Guided course
01:44
Gas Solubility Example
Hydrogen Bonding
Hydrogen bonding is a type of intermolecular force that occurs when hydrogen is covalently bonded to highly electronegative atoms like oxygen or nitrogen. In the context of water, these bonds create a structured network that can affect how gases interact with water. However, the statement incorrectly attributes the decrease in gas solubility to the breaking of hydrogen bonds with gas molecules.
Recommended video:
Guided course
01:22Hydrogenation Reactions
Henry's Law
Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This principle helps explain why gas solubility decreases with increasing temperature, as higher temperatures reduce the gas's tendency to remain dissolved, regardless of the interactions with water molecules.
Recommended video:
Guided course
01:40Henry's Law Calculations
Related Practice
Textbook Question
Indicate whether each statement is true or false: (c) As you cool a saturated solution from high temperature to low temperature, solids start to crystallize out of solution if you achieve a supersaturated solution.
Textbook Question
Indicate whether each statement is true or false: (d) If you take a saturated solution and raise its temperature, you can (usually) add more solute and make the solution even more concentrated.
Textbook Question
(a) Calculate the mass percentage of Na2SO4 in a solution containing 10.6 g of Na2SO4 in 483 g of water.