3.091SC | Fall 2010 | Undergraduate

Introduction to Solid State Chemistry

Aqueous Solutions

25. Introduction to Aqueous Solutions

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Session Overview

Modules Aqueous Solutions
Concepts solute, solvent, solution, solubility rules, solubility product
Keywords water, mixture, colloid, ionic compound, van der Waals force, Madelung constant, suspension, dispersion, molarity, crystallization, miscibility, precipitation, equilibrium constant, saturation, conductivity, common ion effect, homogenization, Arrhenius
Chemical Substances carbon tetrachloride (CCl4), potassium permanganate (KMgO4), silver chloride (AgCl)
Applications water desalinization, glass manufacturing, bulk metallic glass


Before starting this session, you should be familiar with:

Learning Objectives

After completing this session, you should be able to:

  • Define what makes an “aqueous solution.”
  • Explain the behavior of ionic compounds in water.
  • Calculate molarity of a solution.
  • Predict the solubility of different combinations of solutes and solvents, given the chemical properties of those compounds.
  • Explain the dynamics of solutions using the concepts of equilibrium constant, solubility product, and common ion effect.


Book Chapters Topics
[Saylor] 13.1, “Factors Affecting Solution Formation.” Forming a solution; roles of enthalpy and entropy
[Saylor] 13.2, “Solubility and Molecular Structure.” Factors affecting solubility; molecular interactions in liquids; solutions of solids; solubility of ionic substances
[Saylor] 13.3, “Units of Concentration.” Molarity and mole fraction as measures of concentration
[Saylor] 17.1, “Determining the Solubility of Ionic Compounds.” Solubility product Ksp, ion product, common ion effect
[Saylor] 17.4, “Solubility and pH.” Acid-base equilibriua effects on solubility; basic, acidic, and amphoteric oxides; using pH for selective precipation

Lecture Video


Lecture Slides (PDF - 1.3MB)

Lecture Summary

This session surveys the chemistry of aqueous solutions, in which ionic compounds are dissolved in liquid water as a solvent. The rule “like dissolves like” means that a solute tends to dissolve best in a solvent with similar chemical structure. Molarity is defined as a measure of solubility, and conventions for classifying substances as soluble and insoluble are presented. The session also defines and examines the importance of equilibrium constant K and solubility product Ksp, and the common ion effect.

The class ends with a discussion of the properties of amorphous glasses, including recent advances in fabrication and product manufacturing using bulk metallic glasses.


Problems (PDF)

Solutions (PDF)

Textbook Problems

[saylor] Sections Conceptual Numerical
[Saylor] 17.1, “Determining the Solubility of Ionic Compounds.” 1, 6 2, 3, 10, 18, 21

For Further Study

Supplemental Readings

Chang, Kenneth. “The Nature of Glass Remains Anything but Clear.” The New York Times, July 29, 2008.


Svante Arrhenius1903 Nobel Prize in Chemistry

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Course Info

As Taught In
Fall 2010
Learning Resource Types
Course Introduction
Exams with Solutions
Lecture Notes
Lecture Videos
Problem Sets with Solutions
Recitation Videos
Problem Sets
Exam Materials