/*! 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 32 Explain why pressure affects the... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Problem 32

Explain why pressure affects the solubility of \(\mathrm{O}_{2}\) in water, but not the solubility of \(\mathrm{NaCl}\) in water.

Short Answer

Expert verified
In summary, pressure affects the solubility of \(\mathrm{O}_{2}\) in water because, according to Henry's Law, the solubility of a gas is directly proportional to its partial pressure. As pressure increases, more gas molecules are forced into the liquid, increasing solubility. However, pressure does not significantly affect the solubility of a solid like \(\mathrm{NaCl}\) in water, since the dissolution process relies more on temperature and the properties of the solute and solvent, rather than pressure.

Step by step solution

01

Understanding solubility

Solubility is the ability of a substance to dissolve in a solvent. In this situation, the substances are \(\mathrm{O}_{2}\) (gas) and \(\mathrm{NaCl}\) (salt), and the solvent is water. The solubility of a substance depends on various factors, including temperature, pressure, and the nature of the substance and solvent.
02

How pressure affects the solubility of gases

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. This means that when the pressure of a gas above the liquid increases, the gas molecules are pushed more forcefully into the liquid, causing more gas to dissolve. In the case of \(\mathrm{O}_{2}\) in water, an increase in pressure will lead to higher solubility as more oxygen molecules are forced into the liquid.
03

How pressure affects the solubility of solids

The solubility of a solid in a liquid, such as \(\mathrm{NaCl}\) in water, is not significantly affected by pressure. This is because the dissolution process of a solid in a liquid involves breaking the solid's crystal lattice, which is not dependent on pressure. The solubility of a solid is mainly influenced by temperature and the nature of the solute and solvent.
04

Conclusion

To sum up, pressure affects the solubility of \(\mathrm{O}_{2}\) in water because the solubility of a gas is directly proportional to the partial pressure of the gas, as explained by Henry's Law. However, pressure does not significantly influence the solubility of a solid like \(\mathrm{NaCl}\) in water, as the dissolution process of a solid is mainly dependent on temperature and the nature of the substances involved, rather than pressure.

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!

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

(a) What is the mass percentage of iodine \(\left(\mathrm{I}_{2}\right)\) in a solution containing \(0.035 \mathrm{~mol} \mathrm{I}_{2}\) in \(115 \mathrm{~g}\) of \(\mathrm{CCl}_{4} ?\) (b) Seawater contains \(0.0079 \mathrm{~g} \mathrm{Sr}^{2+}\) per kilogram of water. What is the concentration of \(\mathrm{Sr}^{2+}\) measured in ppm?

By referring to Figure 13.17, determine whether the addition of \(40.0 \mathrm{~g}\) of each of the following ionic solids to \(100 \mathrm{~g}\) of water at \(40^{\circ} \mathrm{C}\) will lead to a saturated solution: (a) \(\mathrm{NaNO}_{3}\), (b) \(\mathrm{KCl}\), (c) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) (d) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\)

Oil and water are immiscible. What does this mean? Explain in terms of the structural features of their respective molecules and the forces between them.

Indicate the principal type of solute-solvent interaction in each of the following solutions, and rank the solutions from weakest to strongest solute- solvent interaction: (a) \(\mathrm{KCl}\) in water, (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\), (c) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water.

Consider a series of carboxylic acids whose general formula is \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{n} \mathrm{COOH}\). How would you expect the solubility of these compounds in water and in hexane to change as \(n\) increases? Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

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.