Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 11: Problem 29

Adding a solute to a solvent extends the liquid phase over a larger temperature range. Explain this statement.

Short Answer

Expert verified
When a solute is added to a solvent, it disrupts the natural arrangement of the solvent molecules and forms intermolecular interactions. This leads to a depression of the freezing point and an elevation of the boiling point of the solution. Consequently, the temperature range over which the solution exists as a liquid is extended. This effect of the solute on the phase diagram is what the statement "adding a solute to a solvent extends the liquid phase over a larger temperature range" refers to.

Step by step solution

01

Understanding Phase Changes

In order to explain this statement, it is important to understand the concept of phase changes. A substance, such as a solvent, exists in different phases (solid, liquid, and gas) depending on the temperature. The phase change occurs when a substance changes from one phase to another, such as from solid to liquid or liquid to gas. The temperature at which a phase change occurs is called the phase change temperature.
02

Solute-Solvent Interactions

When a solute is added to a solvent, it disrupts the natural arrangement of the solvent molecules. This disruption occurs because the solute forms intermolecular interactions, such as hydrogen bonds, dipole-dipole interactions, and van der Waals forces, with the solvent molecules. These interactions will affect the energy required for the solvent molecules to escape or overcome the forces holding them together.
03

Effect on Melting Point and Freezing Point

The presence of a solute typically leads to a depression of the freezing point (melting point) and an elevation of the boiling point. This occurs because the solute molecules disrupt the normal arrangement of the solvent molecules. Consequently, it requires more energy to overcome these interactions and move the molecules further apart in the phase change from solid to liquid (freezing point depression) and less energy for the liquid to solid phase change (melting point elevation).
04

Effect on Boiling Point

Similarly, the presence of a solute in a solvent can raise the boiling point of the solution. This is because the solute-solvent interactions force the solvent molecules to use more energy to overcome these additional intermolecular forces and move further apart in the phase change from liquid to gas. As a result, the boiling point of the solution will be higher than that of the pure solvent.
05

Extending the Liquid Phase Temperature Range

Now, recalling the concept of liquid phase extension: when a solute is added to a solvent, the freezing point is depressed, and the boiling point is elevated. Consequently, the temperature range over which the solution exists as a liquid is extended. So, the statement "adding a solute to a solvent extends the liquid phase over a larger temperature range" refers to this effect of the solute on the phase diagram and the subsequent broadening of the liquid phase temperature range.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

The lattice energy* of Nal is \(-686 \mathrm{kJ} / \mathrm{mol}\) , and the enthalpy of hydration is \(-694 \mathrm{kJ} / \mathrm{mol}\) . Calculate the enthalpy of solution per mole of solid Nal. Describe the process to which this enthalpy change applies.

Which of the following statements is(are) true? Correct the false statements. a. The vapor pressure of a solution is directly related to the mole fraction of solute. b. When a solute is added to water, the water in solution has a lower vapor pressure than that of pure ice at \(0^{\circ} \mathrm{C} .\) c. Colligative properties depend only on the identity of the solute and not on the number of solute particles present. d. When sugar is added to water, the boiling point of the solution increases above \(100^{\circ} \mathrm{C}\) because sugar has a higher boiling point than water.

A \(4.7 \times 10^{-2}\) mg sample of a protein is dissolved in water to make 0.25 \(\mathrm{mL}\) of solution. The osmotic pressure of the solution is 0.56 torr at \(25^{\circ} \mathrm{C}\) . What is the molar mass of the protein?

n lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would proceed using the given information. a. 2.0 \(\mathrm{mKCl}\) in water (density of $\mathrm{H}_{2} \mathrm{O}=1.00 \mathrm{g} / \mathrm{cm}^{3} )$ b. 15\(\% \mathrm{NaOH}\) by mass in water $\left(d=1.00 \mathrm{g} / \mathrm{cm}^{3}\right)$ c. 25\(\% \mathrm{NaOH}\) by mass in $\mathrm{CH}_{3} \mathrm{OH}\left(d=0.79 \mathrm{g} / \mathrm{cm}^{3}\right)$ d. 0.10 mole fraction of \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) in water \(\left(d=1.00 \mathrm{g} / \mathrm{cm}^{3}\right)\)

An extremely important application of dialysis is the use of artificial kidney machines to purify blood. Explain how dialysis can be used to purify blood.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic 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.

Sign-up for free