a. Solubility Rules:
II.
III.
IV.
V.
VI.
VII.
Most nitrate (NO3-) salts are soluble.
Most salts containing the alkali metal ions (Li+, Na+, K+, Cs+, Rb+) and the ammonium ion
(NH4+) are soluble.
Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts
containing the ions Ag+, Pb2+, and Hg22+.
Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, Hg2SO4, and CaSO4.
Most hydroxides are only slightly soluble. The important soluble hydroxides are NaOH
and KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble.
Most sulfide (S2-), carbonate (CO32-), chromate (CrO42-), and phosphate (PO43-) salts are
only slightly soluble, except for those containing the cations in Rule II.
1. Based on the above solubility rules identify the below salts as soluble or of low
solubility:
a.
b.
c.
d.
e.
f.
Na2SO4
K2S
AgI
Barium hydroxide
Calcium phosphate
Ammonium chloride
2. For the above solutes, write a balanced equation of their dissociation in water. (Note
that soluble salts completely dissociate in water where salts of low solubility partially
dissociate in water)
3. In the beaker below represent the dissociation of 5 particles of K2S.
K+
S2 -