Chemistry 1441 1st Edition Lecture 12 Outline of Last Lecture I Molarity and Solution Stoichiometry II Electrolytes III Precipitation Reactions Outline of Current Lecture I Solubility Rules II Acid Base Reactions III Solution Stoiciometry Current Lecture I Solubility Rules Soluble Ionic Compounds a b c d e Those containing alkali metals Those containing ammonium Those containing nitrate bicarbonate and chlorate Those containing halide except Ag Hg2 and Pb2 Those containing sulfates except Ag Hg2 Pb2 Ca2 Sr2 and Ba2 Insoluble Ionic Compounds a Those containing carbonate phosphate chromate and sulfide except alkali metals or ammonium b Those containing hydroxide except alkali metals or Ba2 II Acid Base Reactions Acids have a sour taste cause color changes in plant dyes and react with certain metals such as Li Na K Ba Ca Mg and Al Bases have a bitter taste feel slippery cause color changes in plant dyes and can conduct electricity Example hydrochloric acid sodium hydroxide molecular eqn HCl aq NaOH aq H2O l NaCl aq total ionic eqn H aq Cl aq Na aq OH aq H2O l Na aq Cl aq net ionic eqn H aq OH aq H2O l III Solution Stoichiometry M mol L m M L Example What volume of 0 100 M MgCl2 solution is required to precipitate all of the silver from 10 0 mL of 0 0500 M AgNO3 2AgNo3 aq MgCl2 aq 2AgCl s Mg NO3 2 aq 10 0mL 010L 0100 0500 5 00 10 4 mol AgNO3 5 00 10 4 mol AgNO3 1 mol MgCl2 2 mol AgNO3 2 5 10 4 mol MgCl2 L mol M 2 5 10 4mol 100M 2 50 10 3LMgCl2