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