/*! 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 1 Which of the following will affe... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 16: Problem 1

Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes.

Short Answer

Expert verified
Out of the given options, only option c (The temperature changes) will affect the total amount of solute that can dissolve in a given amount of solvent, as the solubility of most solid solutes increases with increasing temperature, whereas the solubility of gas solutes decreases with increasing temperature. Options a and b may speed up the dissolution process but do not change the solubility limit.

Step by step solution

01

Option a: The solution is stirred.

Stirring a solution can speed up the dissolution process, as it helps distribute the solute particles evenly throughout the solvent. However, stirring does not affect the total amount of solute that can ultimately dissolve in the solvent. The solubility limit of the solute remains constant.
02

Option b: The solute is ground to fine particles before dissolving.

Grinding the solute into fine particles increases the surface area of the solute that comes into contact with the solvent. This can speed up the dissolution process, but it does not change the total amount of solute that can dissolve in the solvent. The solubility limit remains the same.
03

Option c: The temperature changes.

Changing the temperature of the solvent can affect the total amount of solute that can dissolve in it. For most solid solutes, their solubility increases with increasing temperature. For gas solutes, however, their solubility decreases with increasing temperature. Therefore, the temperature change can directly affect the total amount of solute that can dissolve in a given amount of solvent. In conclusion, out of the given options, only option c (The temperature changes) will affect the total amount of solute that can dissolve in a given amount of solvent.

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

Write equations for the stepwise formation of each of the following complex ions. a. \(\mathrm{CoF}_{6}^{3-}\) b. \(\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\)

Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties. a. \(\mathrm{Ag}_{3} \mathrm{PO}_{4}, K_{\mathrm{sp}}=1.8 \times 10^{-18}\) b. \(\mathrm{CaCO}_{3}, K_{\mathrm{sp}}=8.7 \times 10^{-9}\) c. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}, K_{\mathrm{sp}}=1.1 \times 10^{-18}\left(\mathrm{Hg}_{2}^{2+}\right.\) is the cation in solution.)

The solubility of \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) in a \(0.20 \mathrm{M} \mathrm{KIO}_{3}\) solution is \(4.4 \times\) \(10^{-8} \mathrm{~mol} / \mathrm{L}\). Calculate \(K_{\mathrm{sp}}\) for \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\).

For each of the following pairs of solids, determine which solid has the smallest molar solubility. a. \(\mathrm{CaF}_{2}(s), K_{\mathrm{sp}}=4.0 \times 10^{-11}\), or \(\mathrm{BaF}_{2}(s), K_{\mathrm{sp}}=2.4 \times 10^{-5}\) b. \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s), K_{\infty}=1.3 \times 10^{-32}\), or \(\mathrm{FePO}_{4}(s), K_{\mathrm{sp}}=1.0 \times 10^{-22}\)

Calculate the molar solubility of \(\mathrm{Co}(\mathrm{OH})_{3}, K_{\mathrm{sp}}=2.5 \times 10^{-43}\).
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

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.