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.