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solubility rules

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single replacement reactions
two types
Metal atom +metal ion

halogen molecule + halide ion
Cl2 + 2I --> 2Cl + I2
precipitation (double replacement) reaction
if two salts are reacting then it is likely a precipitation reaction
the precipitate will be the insoluble salt
there can be two precipitates
salts
ionic compounds that are neither acids or bases
in general MX where M is a metal and X is an anion such as Cl-, SO4 -, PO4 3-
bases
soluble metal hydroxides
(NaOH and KOH being the most common by far)
soluble carbonates (Na2CO3 and K2CO3 being the most common)
aqueous ammonia NH3 +
Generally insoluble
CO3 2-, PO4 3-, S 2-, SO3 2-, C2O4 2-, CrO4 2-
insoluble except alkali metals Li +, Na +, K +, Rb +, Cs+ and NH4 +
Generally insoluble
O 2-, OH -
insoluble except alkali metals Li +, Na +, K +, Rb +, Cs+
and NH4 +, Ca 2+, Sr 2+, Ba 2+
Generally soluble
SO4 2-
EXCEPT
Ca 2+, Sr 2+, Ba 2+, Pb 2+
Generally soluble
F-
EXCEPT
Ca 2+, Sr 2+, Ba 2+, Pb 2+, Mg 2+
Generally soluble
Cl-, Br-, I-
EXCEPT
Ag+, Pb 2+, Hg2 2+
always soluble
alkali metals
Li +, Na +, K +, Rb +, Cs+
NH4-, NO3-, ClO3-, ClO4-, C2H3O2-
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