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Reactions in Aqueous Solutions

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Presentation on theme: "Reactions in Aqueous Solutions"— 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?
AgNO3 + NaCl  AgCl + NaNO3 Na+ is a group 1 metal, so it is soluble Nitrates (NO3-) 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: AgNO3 + NaCl  AgCl + NaNO3 Ag+ + NO Na+ +Cl-  AgCl + Na+ + NO3- 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+ + NO3- 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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