Chemical Equations
Home Table of Contents Preliminary Information Introduction Homogeneous Mixtures Solubility Limits Electrolytes Chemical Equations Precipitation Reactions Heat of Solution Colligative Properties Wrap Up

 

Dissolution Reactions
Molecular Changes
Identifying Acids,Bases and Salts
Writing Ionic Equations

Chemical Equations for Solutions

Now that you are familiar with the differences between electrolytes and nonelectrolytes, and also between strong and weak electrolytes, let's consider how to symbolize the process by which these solutions are formed. After that we will describe what kinds of atomic or molecular changes are taking place. Then we will take a look at how to use your understanding of the process to identify acids, bases and salts from their formulas and the ions that are formed when they go into solution.

First let's deal with symbolizing this process by writing chemical equations for dissolution reactions. You have already learned to write equations for chemical reactions and we'll be doing the same type of thing here. However, we'll be using the following additional symbols.

We use (s) to mean solid,
(l) for liquid,
(g) for gas,
and (aq) for aqueous, which means that the material is dissolved in water.

These symbols are written after the formula for each chemical to show what state or phase the material is in. For example when water melts it changes from solid to liquid. To show this in an equation we would write: H2O(s) rtarrow.gif (850 bytes) H2O(l).

With that background, move on to each of the page in this section. (Links are above in the left margin.)

 

Top of Page

Back to Course Homepage

Clackamas Community College E-mail instructor: Eden Francis
Physical Science
19600 South Molalla Avenue
Oregon City, OR 97045
(503) 594-3352
FAX (503)-650-6657

TDD (503) 650-6649

Distance Learning questions

Clackamas Community College
1998, 2003 Clackamas Community College, Hal Bender