1. Reactions in Aqueous Solution

2. Aqueous Solutions Most chemical reactions involve substances dissolved in water –Solvent – Most plentiful substance in the solution. In an aqueous solution, this is water. –Solute – substances dissolved.

3. Ionic Compounds disassociate into ions when in solution. Polar Molecules do not disassociate. Acids – substances that disassociate to form hydrogen ions.

4. Precipitates Double replacement reactions occur in an aqueous solution to produce a precipitate. However, not all substances that form will come out of solution.

5. Ionic Equations Slightly different from chemical equations, ionic equations show ions in solutions. –Complete ionic equation – ionic equation that shows all the particles as they realistically exist.

6. –Certain ions remain disassociated, and do not participate in the reaction. These are known as spectator ions. –Net Ionic Equation – displays only those ions that participate in the reaction.

7. Example Write a balanced chemical equation, complete ionic equation, and a net ionic equation for the reaction of sodium hydroxide with copper (II) chloride, which produces a precipitate of copper (II) hydroxide.

8. Reactions that Form Water When an acid reacts with a base (substance containing hydroxide), the reaction forms water, and a salt (usually dissolved).

9. Example Write a balanced chemical equation, complete ionic equation and net ionic equation for the neutralization of hydrobromic acid by sodium hydroxide.

10. Reactions the form Gases Precipitates are not the only product from double replacement reactions.

11. Example Hydriodic acid and lithium sulfide, react to produce hydrogen sulfide gas. Write a balanced chemical equation, complete ionic equation and net ionic equation for the reaction.

12. Multiple Reactions Many times the products of one reaction will immediately react with other substances (spectator ions, unused reactant, etc.)

13. Multiple Reactions can be combined and shown as one chemical reaction. In this procedure, any substance found on both sides of the participating reactions are crossed out.

14. Example Hydrochloric acid will react with sodium hydrogen carbonate to produce Carbonic acid and sodium chloride(aq). The carbonic acid then decomposes into water and carbon dioxide. Represent the process as one balanced chemical equation. Show the net ionic reaction as well.