1. Solubility and Net Ionic Equations

2. Solubility
Solubility of a compound determines if the compound will dissolve in water or not.
If a compound is soluble, it will dissolve.
If a compound is insoluble, it will not dissolve.
If a compound dissolves, it is called aqueous.
If not, it is a solid precipitate.
Compounds can either be solid (s), liquid (l), gas (g), or aqueous (aq).

3. Determining solubility
Look at the solubility chart on the back of your periodic table.
First locate the anion. Determine whether it is soluble or not.
Look for any exceptions. Remember, family 1 includes lithium, sodium, potassium, etc.
If it is soluble, then it is aqueous (aq).
If it is insoluble, then it is a solid (s).

4. Example Al(NO3)3 + K3PO4 → AlPO4 + 3KNO3 aq aq s aq Now you try one
Cu(C2H3O2)2 + Na2CO3 →
aq aq s aq
CuCO3 + 2NaC2H3O2

5. Total Ionic Equation
Shows what individual ions are doing in a chemical reaction.
Steps
1 – Write a balanced formula equation
2 – Determine the solubility of each reactant and product
3 – Write the TIE
If a compound is aqueous, break it into ions
Be sure to show charge
If the compound is a solid, leave it alone

6. Example: Write a TIE
Silver Nitrate + Potassium Chloride 

7. “Spectator Ions”
Ions that you cancel out because they aren’t actually involved in the reaction.

8. Net Ionic Equations
A net ionic equation shows only the ions that are actually reacting in a reaction.
Take the Total Ionic Equation, and cancel out ions that appear on both sides of the arrow (spectators)

9. Example: NIE

10. Try this one
Ammonium phosphate + Aluminum chloride 

11. Try this one
Potassium nitrate + Lithium acetate 

12. What do we do if everything cancels out?
NO REACTION!