Reactions Between Ions in Solution • Objectives – To mix ionic solutions and observe possible reactants – To predict formulas of products – To write net ionic equations for reactants Results • Data • Create Data Table for the different combinations of reactants • Indicate whether or not precipitate formed • Create Table of Possible Precipitates by cations • Create Table of Possible Precipitates by anions Background • Ionic Compounds dissociate in water • They separate into anion and cation • When reacting aqueous solutions of ionic compounds, the IONS are reacting • Double displacement • The Solubility Rules are used to determine/ predict the products and whether or not a solid forms Compounds and Equations • Compounds used in lab: – – – – – – – AgNO3 FeCl3 KI Na2SO4 Ba(NO3)2 NaOH Co(NO3)2 Compounds and Equations • Molecular Equation – 3AgNO3(aq) + FeCl3 (aq) ---> 3AgCl (s) + Fe(NO3)3 (aq) • Complete Ionic Equation – 3Ag+ (aq) + 3NO3- (aq) + Fe 3+ (aq) + 3Cl- (aq) ---> 3AgCl(s) + Fe 3+ (aq) + 3NO3- (aq) • Net Ionic Equation – 3Ag+ (aq) + 3Cl- (aq) ---> 3AgCl (s) – NO3- and Fe 3+ are spectator ions Conclusions • Conclusion Questions: – 1. Which products were precipitates from the chemical reactions carried out in lab? Write net ionic equations for 2 of the precipitate reactions. Which solubility rules apply to the 2 reactions? – 2. How would you describe spectator ions? List at least 3 spectator ion products from the chemical reactions carried out in lab. • Summary – Besides the usual information, discuss what happens to ionic compounds in aqueous solutions and how products of the double displacement/ precipitation reactions can be predicted. Use example from your results.