Question

Werecertainionstypicallyalwayssolubleoralwaysinsoluble?Howcouldyoutell?Includespecificexamples.

Answer 1

Solutes and solvents with similar IMF’s tend to be more soluble in one another than those with vastly different IMF’s

Ionic >> H-Bonding > Polar > Non-Polar

The further apart the solute and solvent in terms of IMF's, the less soluble the pair will be.

Note that Ionic Compounds in Aqueous Solution have special rules

Solubility Rules for Ionic Compounds in Aqueous Solutions

A. Always Soluble Ions (these ions never ppt)

Nitrate: NO3^- Perchlorate: ClO4^- Ammonium: NH4⁺ Group 1 ions: Li+ , Na+ , K+ , Rb+ , Cs+

B.Insoluble Ions (these ions form insoluble compounds with other ions except with “Always Soluble Ions”)

Lead: Pb2⁺ Carbonate: CO3^2- Sulfide: S^2- Phosphate: PO4^3- Chromate: CrO4^2-

C. Generally Soluble Ions (these form soluble compounds with most ions unless with Insoluble Ions or special ions)

Halides: Cl^- , Br^- , I^- (insoluble with Ag⁺ , Pb²⁺)

Sulfate: SO4^2- (insoluble with Ba2⁺, Ca²⁺, Sr²⁺, Pb²⁺)

Hydroxide: OH^- only soluble with Group I or II ions (insoluble with other metal ions)