1. Ionic Equations and Acid-Base Reactions

2. The complete ionic equation
A complete ionic equation shows
all aqueous ionic compounds separated into their ions
Molec. eq’n: Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
Comp. ionic eq’n:
Net ionic eq’n:

3. The net ionic equation A net ionic equations shows only
the compounds directly participating in the reaction
Comp. ionic:
Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2I-(aq)  PbI2(s) + 2K+(aq) + 2NO3-(aq)
Net ionic:

4. One more together
Write the net ionic equation for the following reaction:
BaCl2(aq) + Na2SO4(aq)  BaSO4 + 2NaCl(aq)

5. Try this one on your own
What is the net ionic equation for the following reaction?
(NH4)2SO4(aq) + CaCl2(aq)  2NH4Cl(aq) + CaSO4(s)

6. Acids and bases Acids produce ___ ions when dissolved in water
Bases produce ___ ions when dissolved in water H+
Cl- H+ Cl-
H Cl-
Na+
Na+ OH- Na+
OH- OH-

7. Strong Acids and Strong Bases
dissolve completely into their ions in water
______ is created when a strong acid reacts with a strong base

8. Chemical Reactions
Double Displacement
Precipitation
Acid-Base
Form solid
Form water

9. Determine the net ionic equation
HNO3(aq) + KOH(aq)  H2O(l) + KNO3(aq)
hydrochloric acid plus sodium hydroxide 

10. Determine the molecular and net ionic equations

11. Most salts of Na+, K+, and NH4+
Soluble
Slightly Soluble
Insoluble
Most NO3- Salts
Most salts of Na+, K+, and NH4+
Most chloride salts (Cl-) and iodide and bromide salts
AgCl, PbCl2, Hg2Cl2,Those containing Ag+, Hg22+, Pb2+
Most sulfate (SO42-) salts
BaSO4, PbSO4, CaSO4
NaOH and KOH
Most hydroxide (OH-) compounds. Ba(OH)2 and Ca(OH)2 moderately soluble
Most sulfide (S2-) carbonate (CO32-) and phosphate (PO43-) salts
 Note: the terms insoluble and slightly soluble really mean the same thing, since such a tiny amount dissolves that it is not possible to detect it with the naked eye.