1. Net ionic equations Na + Al 3+ S 2– 2Ca 2+ PO 4 3– 3Cl –

2. Solution Chemistry When mixing 2 aqueous solutions there are 2 possible outcomes: 1. 2.

3. Double Displacement Reactions Can Be Recognized in 3 Ways: –The formation of a precipitate –The formation of a gas –The formation of water

4. Not all ionic compounds dissolve! Instead of doing experiments all the time to see which ones will dissolve, we use The solubility rules.

5. Solubility Rules 1.All nitrates (NO 3 - ) are soluble. 2.All ammonium (NH 4 + ) or alkali (Li +, Na +, K +, Rb +, Cs +, Fr + ) compounds are soluble. 3.All carbonates (CO 3 2- ), phosphates (PO 4 3 - ) and hydroxides (OH - ) are insoluble except with the cations in Rule #2. 4. All chlorides (Cl - ), bromides (Br - ), and iodides (I - ), are soluble except with Ag +, Pb 2+, or Hg +. 5. All sulphates (SO 4 2- ) are soluble except with Ca 2+, Sr 2+, Ba 2+, Ra 2+, Pb 2+,

6. Which of the following are soluble in water? a.SrSO 4 b.NaNO 3 c.PbCl 2 Not soluble soluble Not soluble

7. Precipitation Reactions When a solid doesn’t dissolve it is called insoluble. A solid that forms when two solutions are mixed is called a precipitate. By definition: -soluble = 1g / 100mL of water - slightly soluble = 0.1g-1g/100mL H 2 O - insoluble = 0.1g / 100mL H 2 O

8. Predict the products of the following reaction: (if no solid precipitate is formed, there is no reaction) Pb(NO 3 ) 2 (aq) + KI (aq)  Pb(NO 3 ) 2 (aq) + 2KI (aq)  PbI 2 (s) + 2KNO 3 (aq) We know it is a solid precipitate because it is insoluble according to the solubility rules. Total Ionic Equation (shows all ions involved) Pb 2+ (aq) + NO 3 - (aq) + K + (aq) + 2I - (aq)  PbI 2(s) + K + (aq) + NO 3 - (aq)

9. A picture of the reaction: Pb 2+ NO 3 - Because K + and NO 3 - remain dissolved, they are called spectator ions and are not included in the net ionic equation. Net Ionic Equation Pb 2+ (aq) + 2I - (aq)  PbI 2 (s) NO 3 - K+K+ I-I- K+K+ PbI 2(s)

10. Net Ionic Equation Write the balanced chemical and net ionic equation for: Na 2 CO 3 (aq) + CaCl 2 (aq)  Step 1: Write the balanced chemical equation Na 2 CO 3 (aq) + CaCl 2 (aq)  CaCO 3 (s) + 2NaCl (aq) Step 2: Remove the spectator ions (those that are soluble). Ca 2+ (aq) + CO 3 2- (aq)  CaCO 3 (s) Insoluble precipitate

11. Write the total and net ionic equation for when sodium chloride reacts with silver nitrate Step 1: Write the chemical equation and indicate whether or not a precipitate is formed. NaCl (aq) + AgNO 3(aq)  NaNO 3(aq) + AgCl (s) Step 2: Write the chemical equation with the soluble ionic compounds in their dissociated ions. (Make sure all charges are indicated and the reaction is balanced.) Na + (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq)  AgCl (s) + Na + (aq) + NO 3 - (aq)

12. Step 3: Identify any spectator ions (ions which are the same in the reactants and products) and eliminate them. Na + (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq)  AgCl (s) + Na + (aq) + NO 3 - (aq) Step 4: Rewrite the total ionic equation without the spectator ions to get the net ionic equation. Ensure the reaction is balanced. Cl - (aq) + Ag + (aq)  AgCl (s)

13. Homework Pg 335 #1,2 Pg 339 #4 Pg 343 # 5,6