/*! 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 6 Describe the factors that affect... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Problem 6

Describe the factors that affect the solubility of a solid in a liquid. What does it mean to say that two liquids are miscible?

Short Answer

Expert verified
Factors affecting solubility of a solid in a liquid include temperature, pressure, and nature of solvent and solute, with most solids becoming more soluble with increasing temperature. 'Miscibility' refers to the ability of two liquids to mix in all proportions to form a homogeneous solution, typically following the 'like dissolves like' principle in which polar liquids are miscible with polar liquids, and non-polar ones with non-polar ones.

Step by step solution

01

Factors Affecting Solubility

There are majorly three factors that influence the solubility of a solid in a liquid: Temperature, Pressure, and Nature of Solvent and Solute. In most cases, solubility of a solid in a liquid increases with rise in temperature. Pressure has little effect on the solubility of a solid in a liquid but it does have an impact in the case of gases. Lastly, whether a solid will dissolve or not in a liquid often depends on the nature of the solvent and the solute. Like dissolves Like鈥� is a general rule, it means polar solvents dissolve polar solutes, and non-polar solvents dissolve non-polar solutes.
02

Understanding Miscibility

Miscibility is a term used to describe the property of liquids to mix in all proportions, forming a homogeneous solution. The concept is also 'Like dissolves like'. Polar liquids are miscible with polar liquids, and non-polar liquids are miscible with non-polar liquids. For example: Water (polar) and ethanol (polar) are miscible.

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

Calculate the molality of each of the following aqueous solutions: (a) \(2.50 \mathrm{M} \mathrm{NaCl}\) solution (density of solution \(=1.08 \mathrm{~g} / \mathrm{mL}\) ), (b) 48.2 percent by mass KBr solution.

For dilute aqueous solutions in which the density of the solution is roughly equal to that of the pure solvent, the molarity of the solution is equal to its molality. Show that this statement is correct for a \(0.010 \mathrm{M}\) urea \(\left.\left[\mathrm{(NH}_{2}\right)_{2} \mathrm{CO}\right]\) solution.

Outline the steps required for conversion among molarity, molality, and percent by mass.

Which of these two aqueous solutions has (a) the higher boiling point, (b) the higher freezing point, and (c) the lower vapor pressure: \(0.35 \mathrm{~m} \mathrm{CaCl}_{2}\) or \(0.90 \mathrm{~m}\) urea? State your reasons.

Why is naphthalene \(\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\) more soluble than \(\mathrm{CsF}\) in benzene?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Kinetics

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.