Solubility Rules for Ionic Compounds

Flashcards detailing the solubility of specific ions and the exceptions that change their solubility status.

Chromate ($CrO_4^{2-}$)

An ion that forms insoluble compounds except when combined with Group 1 ions or ammonium ($NH_4^+$).

Carbonate ($CO_3^{2-}$)

An ion that forms insoluble compounds except when combined with Group 1 ions or ammonium ($NH_4^+$).

Phosphate ($PO_4^{3-}$)

An ion that forms insoluble compounds except when combined with Group 1 ions or ammonium ($NH_4^+$).

Sulfide ($S^{2-}$)

An ion that forms insoluble compounds except when combined with Group 1 ions, $Ca^{2+}$, $Mg^{2+}$, or ammonium ($NH_4^+$).

Hydroxide ($OH^-$)

An ion that forms insoluble compounds except when combined with Group 1 ions, $Ca^{2+}$, $Ba^{2+}$, $Sr^{2+}$, or ammonium ($NH_4^+$).

Group 1 ions

soluble

Ammonium ($NH_4^+$)

soluble

Nitrate ($NO_3^-$)

soluble

Acetate ($C_2H_3O_2^-$ or $CH_3COO^-$)

soluble

Hydrogen carbonate ($HCO_3^-$)

soluble

Chlorate ($ClO_3^-$)

soluble

Halides ($Cl^-$, $Br^-$, $I^-$)

Ions that form soluble compounds except when combined with $Ag^+$, $Pb^{2+}$, or $Hg_2^{2+}$.

Sulfates ($SO_4^{2-}$)

Ions that form soluble compounds except when combined with $Ag^+$, $Ca^{2+}$, $Sr^{2+}$, $Ba^{2+}$, or $Pb^{2+}$.