1. Complete Ionic Equation Net Ionic Equations

2. Electrolytes from Conductivity Test
Electrolytes are substances whose aqueous solution is a conductor of electricity
All electrolyte have ions dissolved in water
Conductor of electricity?
Pure water: No! No ions are present
Table salt (NaCl) solution: Yes! Na+ & Cl- 2

3. Dissociation
Dissociation: When ionic compounds dissolve in water, the anions and cations are separated from each other - however not all ionic compounds are soluble in water!
When compounds containing polyatomic ions dissociate, the polyatomic group stays together as one ion

4. Electrolytes
Strong electrolytes: all the electrolyte molecules or formula units are separated into ions. Table salt (NaCl)
Non-electrolytes: none of the molecules are separated into ions. Table sugar (C12H22O11), all gases (CO2), water.
Weak electrolytes: a small percentage of the molecules are separated into ions. Acetic acid (Vinegar, CH3COOH), ammonia in water (NH3). 4

5. Strong Electrolytes Salts = water soluble ionic compounds
NaCl, NH4C2H3O2, Ba(NO3)2, FeBr3, CuSO4
Strong Acids = completely dissociate to form H+ ions in water solution.
HCl, HBr, HI, HNO3, H2SO4, HClO4
Strong Bases = water soluble metal hydroxides (OH-)
Metal hydroxide of ALL GIA metals such as NaOH, KOH, etc.
Lower GIIA hydroxides: Ca(OH)2), Sr(OH)2, Ba(OH)2 5

6. Dissociation
Potassium iodide dissociates in water into potassium cations and iodide anions
KI(aq)  K+(aq) + I-(aq)
Copper(II) sulfate dissociates in water into copper(II) cations and sulfate anions
CuSO4(aq)  Cu2+(aq) + SO42-(aq) K+ I- K I
SO4
SO42- Cu
Cu2+

7. Dissociation involving Polyatomic Ions
Ammonium phosphate dissociates in water into ammonium cations and phosphate anions
(NH4)3PO4(aq)  3 NH4+(aq) + PO43-(aq)
PO4
PO43-
NH4
NH4
NH4+
NH4
NH4+
NH4+

8. Ionic Equations Molecular equations uses Chemical formulas
2 KOH(aq) + Mg(NO3)2(aq) ® 2 KNO3(aq) + Mg(OH)2(s)
Ionic equations describe the material’s structure when dissolved.
ONLY aqueous strong electrolytes are written as ions
soluble salts, strong acids, strong bases
ALL OTHER compounds, Gases, Solids (such as insoluble substances), Liquids are written in molecular form
2K+(aq) + 2OH−(aq) + Mg2+(aq) + 2NO3−(aq) ® 2K+(aq) + 2NO3−(aq) + Mg(OH)2(s) 8 8

9. Net Ionic Equations
Ions that are both reactants and products are called spectator ions
2K+(aq) + 2OH−(aq) + Mg2+(aq) + 2NO3−(aq) ® 2K+(aq) + 2NO3−(aq) + Mg(OH)2(s)
Net ionic equation: An ionic equation in which the spectator ions are removed
2 OH−(aq) + Mg2+(aq) ® Mg(OH)2(s) 9 9

10. Example: Acid-Base neutralization
NOTE: ONLY soluble salts, strong acids, and strong bases forms ions
2HNO3(aq) + Ca(OH)2(s) ® 2H2O(l) + Ca(NO3)2(aq)
Types? ________ _____ _____ ________
Ionic equation:
Spectator ions?
net ionic equation: 10

11. Example: Gas-forming ionic equation
ONLY soluble salts, strong acids, and strong bases forms ions
Na2CO3(aq) + 2HCl(aq) ® 2NaCl(aq) + CO2(g) + H2O(l)
Types? ________ ________ ________ ____ ____
Ionic equation:
Spectator ions?
net ionic equation: 11

12. Precipitation Reaction as ionic equation
ONLY __________, ___________, and ___________ forms ions!!!
K2CO3(aq) + 2 AgNO3(aq) ® 2 KNO3(aq) + Ag2CO3(s)
Types? ________ ________ _______ ___________
Ionic equation:
Spectator ions?
net ionic equation: 12

13. More Practice – Write the ionic and net ionic equation
K2SO3(aq) + 2HBr(aq) ® H2O(l) + SO2(g) + 2 KBr(aq)
CO2(g) + 2KOH(aq) ® K2CO3(aq) + H2O(l)
Ba(OH)2(aq) + H2SO4(aq) ® 2H2O(l) + BaSO4(s)
2LiOH(aq) + CuSO4(aq) ® Cu(OH)2(s) + Li2SO4(aq) 13

14. More Practice – Convert and Complete, then Write the ionic and net ionic equation
chloric acid + ammonium sulfite 
silver acetate + iron(III) bromide 
zinc hydroxide + sulfuric acid 
lithium sulfite + manganese(II) chloride  14

15. Weak Electrolytes Does NOT dissociate
Weak acids (acetic acid, nitrous acid, hydrofluoric acid, etc), Weak base (ammonium hydroxide, etc), Insoluble salts largely remain undissociated in water
HC2H3O2(aq)  H+(aq) + C2H3O2-(aq)
NH4OH(aq)  NH4+(aq) + OH-(aq)
PbCl2(s) CaCO3(s) BaSO4(s)
Pure gas, liquid, or solid exists as non-dissolved states
CO2(g), H2S(g), H2O(l), Al(s), Hg(s) 15

16. Write the ionic and net ionic equation involving weak or non-electrolyte(s)
Na2CO3(aq) + 2 HC2H3O2(aq) ® 2 NaC2H3O2(aq) + CO2(g) + H2O(l)
sol. salt weak acid sol. salt nonelectrolyte
2Na+(aq) + CO32−(aq) + 2HC2H3O2(aq)
® 2Na+(aq) + 2C2H3O2−(aq) + CO2(g) + H2O(l)
NIE: CO32−(aq) + 2HC2H3O2(aq) ® 2C2H3O2−(aq) + CO2(g) + H2O(l) 16

17. Write the ionic and net ionic equation involving weak or non-electrolyte(s)
NH4OH(aq) + HC2H3O2(aq) ® NH4C2H3O2(aq) + H2O(l)
weak base weak acid sol. salt nonelectrolyte
NH4OH(aq) + HC2H3O2 (aq)
® C2H3O2−(aq) + NH4+(aq) + H2O(l)
NIE: no spectator ions, same as Complete Ionic Equations 17

18. Practice – Write the ionic and net ionic equation
K2CO3(aq) + 2HC2H3O2(aq) ® H2O(l) + CO2(g) + 2KC2H3O2(aq)
2HI(aq) + BaSO3(s) ® BaI2(aq) + H2O(l) + SO2(g)
BaBr2(aq) + 2AgNO3(aq) ® 2AgBr(s) + Ba(NO3)2(aq)
2 NH4OH(aq) + CuSO4(aq) ® Cu(OH)2(s) + (NH4)2SO4(aq) 18

19. More Practice – Convert and Complete, then Write the ionic and net ionic equation
sulfuric acid + ammonium hydroxide 
aluminum acetate + ammonium hydroxide 
iron(II) sulfite + acetic acid 
scandium(III) hydroxide + acetic acid  19

20. More Practice: Write and Balance the Ionic and Net Ionic Equation in aqueous solution from Word Equation
hydrobromic acid + zinc metal  zinc bromide + hydrogen gas
chlorine gas + water  hydrochloric acid + hypochlorous acid (as a weak acid)
copper + iron(III) nitrate  iron(II) nitrate + copper(II) nitrate
acetic acid + magnesium metal  magnesium acetate + hydrogen gas 20

21. Example–Ionic and net ionic equation
NOTE: ONLY soluble salts, strong acids, and strong bases forms ions
2HNO3(aq) + Ca(OH)2(s) ® 2 H2O(l) + Ca(NO3)2(aq)
Forms Ions? ______ _____ _____ ________
Ionic equation:
Spectator ions?
NIE: 2H+(aq) + Ca(OH)2(s) ® 2 H2O(l) + Ca2+(aq) 21

22. Practice –ionic equation
ONLY soluble salts, strong acids, and strong bases forms ions
Na2CO3(aq) + 2 HCl(aq) ® 2 NaCl(aq) + CO2(g) + H2O(l)
sol. salt sol.acid sol. salt nonelectrolyte
2Na+(aq) + CO32−(aq) + 2H+(aq) + 2Cl−(aq)
® 2Na+(aq) + 2Cl−(aq) + CO2(g) + H2O(l)
NIE: CO32−(aq) + 2 H+(aq) ® CO2(g) + H2O(l) 22

23. Practice – Write the ionic and net ionic equation
K2CO3(aq) + 2 AgNO3(aq) ® 2 KNO3(aq) + Ag2CO3(s)
sol. salt sol.salt sol. salt insoluble salt
2K+(aq) + CO32−(aq) + 2Ag+(aq) + 2NO3−(aq)
® 2K+(aq) + 2NO3−(aq) + Ag2CO3(s)
NIE: 2 Ag+(aq) + CO32−(aq) ® Ag2CO3(s) 23

24. Write the ionic and net ionic equation involving weak or non-electrolyte(s)
Na2CO3(aq) + 2 HC2H3O2(aq) ® 2 NaC2H3O2(aq) + CO2(g) + H2O(l)
sol. salt weak acid sol. salt nonelectrolyte
2Na+(aq) + CO32−(aq) + 2HC2H3O2(aq)
® 2Na+(aq) + 2C2H3O2−(aq) + CO2(g) + H2O(l)
NIE: CO32−(aq) + 2HC2H3O2(aq) ® 2C2H3O2−(aq) + CO2(g) + H2O(l) 24

25. Write the ionic and net ionic equation involving weak or non-electrolyte(s)
NH4OH(aq) + HC2H3O2(aq) ® NH4C2H3O2(aq) + H2O(l)
weak base weak acid sol. salt nonelectrolyte
NH4OH(aq) + HC2H3O2 (aq)
® C2H3O2−(aq) + NH4+(aq) + H2O(l)
NIE: no spectator ions, same as Complete Ionic Equations 25