1. Reactions in Aqueous Solutions
Section 8.3
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2. Vocab to know: Soluble – dissolves (goes away) in solution
Precipitate – does not dissolve in solution, forms a chunky solid in the solution
Spectator Ions – ions that are soluble in solution and do not form a precipitate

3. Solubility Rules
Ions that are soluble and do NOT form a precipitate in the reaction
Group 1 metals are soluble
Nitrates and acetates are soluble

4. Which compound is the precipitate?
AgNO3 + NaCl  AgCl + NaNO3
Na+ is a group 1 metal, so it is soluble
Nitrates (NO3-) are also soluble
The solubility rules do not say anything about silver or chloride, so this will form the precipitate!

5. Complete Ionic Equations
Shows the dissolves particles as free ions in the solution
Example:
AgNO3 + NaCl  AgCl + NaNO3
Ag+ + NO Na+ +Cl-  AgCl + Na+ + NO3-
Complete Ionic Reaction

6. Net Ionic Equations Shows only the ions that actual cause a reaction
Cross out the “Spectator Ions”
Example:
Ag+ + NO Na+ +Cl-  AgCl + Na+ + NO3-
Ag+ + Cl-  AgCl
Net Ionic Reaction

7. After reading Section 8.3, you should know:
How to apply the solubility rules to determine which compound will form a precipitate
How to write a complete and net ionic equation