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Reactions in Aqueous Solutions Section 8.3 Pages 225-230.

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Presentation on theme: "Reactions in Aqueous Solutions Section 8.3 Pages 225-230."— Presentation transcript:

1 Reactions in Aqueous Solutions Section 8.3 Pages

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? AgNO 3 + NaCl AgCl + NaNO 3 Na + is a group 1 metal, so it is soluble Nitrates (NO 3 - ) 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: AgNO 3 + NaCl AgCl + NaNO 3 Ag + + NO Na + +Cl - AgCl + Na + + NO 3 - 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 + + NO 3 - 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


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