Precipitate - an insoluble solid formed by a reaction in solution.
Consider the following molecular equation:
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
The net ionic equation of the above molecular equation is:
Ag+(aq) + Cl-(aq) → AgCl(s)
In order to know which ions will combine to form precipitates, we have the solubility rules
Solubility Rules
- All salts containing NH4+ and group IA cations (Li+, Na+, K+, Rb+, Cs+, ) are soluble.
- All salts containing NO3-, C2H3O2-, HClO3-, and ClO4- are soluble.
- All salts containing Cl-, Br-, and I- are soluble, except those with Ag+, Hg22+, and Pb2+
- All salts containing SO42- are soluble, except PbSO4, BaSO4, HgSO4, CaSO4, and AgSO4.
- Most salts containing O2-, OH-, PO43-, CO32-, and S2- are insoluble, except those containing NH4+ and group IA cations.
Determine the net ionic equation for the following reaction:
Ba(NO3)2 + Na2SO4 → BaSO4 + 2NaNO3
Rule number 4 tells us that BaSO4 is insoluble. So we can write the complete ionic equation as
Ba2+(aq)+2 NO3-(aq) +2 Na+(aq)+SO42-(aq) → BaSO4(s)+2 Na+(aq)+NO3-(aq)
Removing the spectator ions leaves us with the net ionic equation:
Ba2+(aq) + SO42-(aq) → BaSO4(s)
Homework from Chemisty, The Central Science, 10th Ed.
4.19, 4.21, 4.23, 4.25, 4.27, 4.39, 4.41, 4.43, 4.45, 4.47, 4.49, 4.51, 4.53, 4.55, 4.57
