By: Darcy, Matthew and Yosuke
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Solubility is a result of an interaction between
polar water molecules and the ions which
make up a product. Two forces determine the
extent to which solution will occur.
Compounds with small charges tend to be
soluble
Compounds with large charges tend to be
insoluble
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As the charge is increased, the force holding
those ions together becomes stronger.
H20 molecules and the ions of the solid,
tends to bring ions into the solution.
Considering this the compound would be
highly soluble in water.
Between oppositely charged ions. This keeps
the ions in a solid state, making it insoluble.
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Ionic compounds with group 1 metallic or ammonium
cations, NH4+, form soluble compounds no matter
what the anion is.
Ionic compounds with acetate or nitrate ions it
forms soluble compounds no matter what the cation
is.
Compounds with chloride, bromide or iodide ions
are water-soluble except when paired with silver or
lead(II) ions.
Compounds with sulfate are water-soluble except
with barium or lead(II) ions.
Compounds with carbonate, phosphate or hydroxide
ions, are insoluble in water except with group 1
metallic ions or ammonium ions, larger charges.
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With what cations form soluble compounds
no matter what the anion is?
With what anions form soluble compounds
no matter what the cation is?
What are the exceptions to not make a
compound soluble when chloride, iodide or
bromide ions are involved.
Compounds with what are water-soluble
except when paired with barium or lead(II)
ions?