/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 39 Describe factors that affect the... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 14: Problem 39

Describe factors that affect the formation of solutions.

Short Answer

Expert verified
The formation of solutions is influenced by the properties of the solute and solvent, temperature, and pressure. Generally, "like dissolves like," meaning polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes. The solubility of most solid solutes increases with temperature, but may decrease if the dissolution process is exothermic. Pressure greatly affects the solubility of a gas in a liquid, with solubility increasing as pressure increases, according to Henry's law. For solids and liquids, pressure has a negligible effect on solubility compared to temperature and solute-solvent properties.

Step by step solution

01

Identify the solute and solvent

The solute is the substance that is to be dissolved, while the solvent is the substance in which the solute is dissolved. Sometimes the distinction is not clear, and in such cases, we can generally consider the substance present in larger quantity as the solvent.
02

Consider the properties of solute and solvent

The formation of a solution largely depends on the properties of both the solute and the solvent. According to the phrase "like dissolves like," polar solvents tend to dissolve polar solutes, and nonpolar solvents tend to dissolve nonpolar solutes. This is because solvents and solutes with similar molecular structures and intermolecular forces are more likely to mix together.
03

Analyze the role of temperature

The solubility of a substance generally increases with an increase in temperature. For most solid solutes, solubility increases as the temperature of the solvent increases, because higher temperatures provide the energy needed to break the bonds between solute particles and solvent particles. However, in some cases, the solubility of a solute could decrease with increasing temperature if the dissolution process is exothermic (releases heat).
04

Consider the effect of pressure on solubility

The solubility of a gas in a liquid is greatly affected by pressure. According to Henry's law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. As we increase the pressure, the solubility of the gas in the liquid also increases. For solids and liquids, the effect of pressure on solubility is insignificant compared to the effects of temperature and the properties of solutes and solvents. In summary, the factors that affect the formation of solutions are the properties of the solute and solvent, temperature, and pressure. Understanding these factors helps in predicting whether a solute will dissolve in a particular solvent and under specific conditions.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Solubility
Solubility refers to the ability of a solute to dissolve in a solvent to form a homogeneous solution at a given temperature and pressure. It's a fundamental property that determines how much of a solute can be dissolved in a solvent. Solubility is expressed in terms of the maximum concentration of solute that can be dissolved. Different substances show varying levels of solubility. Factors influencing solubility include:
  • The nature of the solute and solvent: "Like dissolves like," meaning polar substances typically dissolve best in polar solvents, and nonpolar substances in nonpolar solvents.
  • Interactions and bonds: The more similar the intermolecular forces are between solute and solvent, the more likely they are to form a solution.
Temperature Effects on Solubility
Temperature has a significant impact on the solubility of substances. For many solid solutes, increasing the temperature elevates their solubility in a solvent. This is because heat provides energy for breaking intermolecular bonds, allowing more solute particles to interact with the solvent.
However, this rule doesn't apply in all cases. Some solutes have exothermic dissolution processes, where increasing the temperature can actually reduce solubility as heat hinders the dissolution process.
Understanding how temperature affects solubility enables better predictions of solution behavior under different conditions and helps in applications where temperature control is critical.
Pressure Effects on Solubility
Pressure primarily affects the solubility of gases in liquids. According to Henry's Law, the solubility of a gas increases with an increase in pressure. This is because more gas molecules are "pushed" into the solution, enhancing their interaction with the solvent.
For liquids and solids, pressure changes rarely have a noticeable effect on solubility due to the incompressible nature of these phases. Therefore, in practical scenarios, pressure adjustments are mostly considered when dealing with gaseous solutes. Consider the case of carbonated beverages: higher pressure keeps more carbon dioxide dissolved in the liquid, maintaining the fizz.
Properties of Solute and Solvent
The intrinsic properties of solutes and solvents play a crucial role in the formation of solutions. These properties include polarity, molecular size, and structure.
  • Polarity: The concept of "like dissolves like" highlights the interplay of polar and nonpolar substances. Polar solutes generally dissolve in polar solvents, and the same rule applies to nonpolar pairs.
  • Molecular size: Smaller molecules often dissolve more easily, due to their ability to interact more readily with the solvent molecules.
  • Molecular structure: Structural compatibility between solute and solvent can result in better dissolution, leading to stable and uniform solutions.
Knowing these properties can guide the selection of the appropriate solvent for dissolving a given solute successfully.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

What volume of a 3.00\(M \mathrm{KI}\) stock solution would you use to make 0.300 \(\mathrm{L}\) of a 1.25 \(\mathrm{M} \mathrm{Kl}\) solution?

Describe different types of colloids.

How many milliliters of 3.0\(M\) phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) can be made from 95 \(\mathrm{mL}\) of a 5.0 \(\mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) solution?

What is the molality of a solution that contain 75.3 \(\mathrm{g}\) of \(\mathrm{KCl}\) dissolved in 95.0 \(\mathrm{g}\) of water?

Soft Drinks The partial pressure of \(\mathrm{CO}_{2}\) inside a bottle of soft drink is 4.0 \(\mathrm{atm}\) at \(25^{\circ} \mathrm{C}\) . The solubility of \(\mathrm{CO}_{2}\) is 0.12 \(\mathrm{mol} / \mathrm{L}\) . When the bottle is opened, the partial pressure drops to \(3.0 \times 10^{-4} \mathrm{atm} .\) What is the solubility of \(\mathrm{CO}_{2}\) in the open drink? Express your answer in grams per liter.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.