Chapter 10-3
 Many reactions occur in water- that is, in
aqueous solution
 When dissolved in water, many ionic
compounds “dissociate”, or separate, into
cations and anions. These compounds
are soluble in water.
 Refer
to the solubility list
 Compounds NOT soluble can be a solid
(precipitate), liquid, or gas
Net Ionic Equations
 Occurs in a double replacement reaction

AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq)
1. Write the full balanced equation
2. Next, write it as an ionic equation by
splitting the compounds into their ions:
Ag1+ + NO31- + Na1+ + Cl1- 
AgCl + Na1+ + NO31Note that the AgCl did not ionize, because it is a “precipitate”
Net Ionic Equations
3. SIMPLFY by crossing out ions not
directly involved (called spectator ions)
Ag1+ (aq) + Cl1- (aq)  AgCl (s)
This is called the net ionic equation
 Some reactions will form water
HBr(aq) + NaOH(aq)  H2O(l) + NaBr (aq)
 Some reactions will form gas
2HI(aq) + Li2S(aq)  H2S(g) + 2LiI (aq)
Practice Problems
Write the Chemical, Complete Ionic, and Net ionic
equations
1. Aqueous solutions of potassium iodide and silver
nitrate are mixed, forming the precipitate silver
iodide.
2. Aqueous solutions of aluminum chloride and sodium
hydroxide are mixed, forming the precipitate
aluminum hydroxide.
3. Sulfuric acid and aqueous potassium hydroxide forms
water.
4. Hydrobromic acid reacts with aqueous ammonium
carbonate to produce a gas.