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The general chemistry book that I'm using to supplement Kaplan's Blue Book is McMurry and Fay's Chemistry (4th ed.). This book states the solubility rules as follows:
A compound is probably soluble if it contains either (or both) of the following criteria:
1) contains one of the following cations:
- group 1A cations: Li+, Na+, K+, Rb+, Cs+
- ammonium cation: NH4+
2) contains one of the following anions:
- Halide: Cl-, Cr-, I- not paired with Ag+, Hg22+, or Pb2+
- Nitrate (NO3-), perchlorate (ClO4-), acetate (CH3CO2-), and sulfates (SO42-) not paired with Ba2+, Hg22+, Pb2+, Ca2+, or Sr+
If a compound does not contains one of the previous ions, then it is probably not soluble.
How accurate is this information?
A compound is probably soluble if it contains either (or both) of the following criteria:
1) contains one of the following cations:
- group 1A cations: Li+, Na+, K+, Rb+, Cs+
- ammonium cation: NH4+
2) contains one of the following anions:
- Halide: Cl-, Cr-, I- not paired with Ag+, Hg22+, or Pb2+
- Nitrate (NO3-), perchlorate (ClO4-), acetate (CH3CO2-), and sulfates (SO42-) not paired with Ba2+, Hg22+, Pb2+, Ca2+, or Sr+
If a compound does not contains one of the previous ions, then it is probably not soluble.
How accurate is this information?