1. Warm-Up: Double Displacement and Solubility Use your solubility table to predict which of the following solutions would produce a precipitate when mixed with a solution of copper (I) nitrate – Sodium hydroxide – Sodium sulfate – Potassium iodide

2. Reactions in Solutions LG: I understand the concept of dissociation and can use this to write total and net ionic equations

3. Dissociation Equations Many ionic compounds are highly soluble and dissociate into ions in aqueous solution Example: CuNO 3(s)  C U + (aq) + NO 3 - (aq) In aqueous double displacement reaction, we must consider the dissociation of 2 ionic compounds Example: CuNO 3(s) + KCl (s) 

4. Total Ionic Equations Total Ionic Equations provide a theoretical explanation for the results observed in a double displacement reaction

5. Net Ionic Equations In chemical reactions we do not normally show substances that do not change in any way Aqueous ions that remain in solution during a reaction are called spectators Writing chemical equations without the spectators, provides the net ionic equation.

6. In the previous example, which ions are spectators? How would you write the net ionic equation?

7. Consider the Following… Write a net ionic equation for the following reaction: aluminum nitrate + sodium phosphate  aluminum phosphate + sodium nitrate Where do we start?

8. Creating a NET ionic equation: 1.Write a balanced chemical equation 2.Use solubility rules to determine whether a precipitate will form 3.Write the total ionic equation by showing all soluble compounds as ions 4.Cancel the identical ions 5.Write the net ionic equation

9. Homework Pg. 428 # 1, 3, 4, 6, 8 GO HABS GO!