1. Salts containing Group I elements are soluble (Li+, Na+,
K+, Cs+, Rb+). Exceptions to this rule are rare. Salts
containing the ammonium
ion (NH4+) are also soluble.
2. Salts containing nitrate ion (NO3-) are generally soluble.
3. Salts containing Cl -, Br -, I - are generally soluble.
Important exceptions to this rule are halide
salts of Ag+, Pb2+, and (Hg2)2+. Thus,
AgCl,
PbBr2, and Hg2Cl2 are all insoluble.
4. Most silver salts are insoluble. AgNO3 and
Ag(C2H3O2) are common soluble salts of silver; virtually
anything else is insoluble.
5. Most sulfate salts are soluble. Important exceptions to this rule include BaSO4,
PbSO4, Ag2SO4 and SrSO4 .
6. Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble.
Hydroxide salts of Group II elements (Ca,
Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al3+ are
insoluble. Thus, Fe(OH)3, Al(OH)3, Co(OH)2 are not
soluble.
7. Most sulfides of transition metals are highly insoluble. Thus, CdS, FeS, ZnS,
Ag2S are all insoluble. Arsenic, antimony, bismuth, and lead
sulfides are also insoluble.
8. Carbonates are frequently insoluble. Group II carbonates (Ca, Sr, and Ba) are insoluble. Some
other insoluble carbonates include FeCO3 and
PbCO3.
9. Chromates are frequently insoluble. Examples: PbCrO4, BaCrO4
10. Phosphates are frequently insoluble. Examples:
Ca3(PO4)2, Ag3PO4
11. Fluorides are frequently insoluble. Examples: BaF2, MgF2
PbF2.
This offering of solubility rules is in the public domain and may be copied without restriction. The
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