the ionic product << Ksp..

Here you go--

Rule 1. All compounds of Group IA elements (the alkali metals) are soluble.

For example, NaNO3, KCl, and LiOH are all soluble compounds. This means that an aqueous solution of KCl really contains the predominant species K+ and Cl- and, because KCl is soluble, no KCl is present as a solid compound.

Rule 2. All ammonium salts (salts of NH₄⁺) are soluble.

For example, NH4OH is a soluble compound. Molecules of NH4OH completely dissociate to give ions of NH4+ and OH- in aqueous solution.

Rule 3. All nitrate (NO₃^-), chlorate (ClO₃^-), perchlorate (ClO₄^-), and acetate (CH₃COO^- or C₂H₃O₂^-, sometimes abbreviated as Oac^-) salts are soluble.

For example, KNO3 would be classified as completely soluble by rules 1 and 3, and thus KNO3 could be expected to dissociate completely in aqueous solution into K+ and NO3- ions.

Rule 4.All chloride (Cl^-), bromide (Br^-), and iodide (I^-) salts are soluble except for those of Ag⁺, Pb²⁺, and Hg₂²⁺.

For example, AgCl is a classic insoluble chloride salt, with a Ksp value of 1.8 ´ 10-10.

Rule 5. All sulfate ( SO₄⁼) compounds are soluble except those of Ba²⁺, Sr²⁺, Ca²⁺, Pb²⁺, Hg₂²⁺, and Hg²⁺, Ca²⁺ and Ag⁺ sulfates are only moderately soluble.

For example, BaSO4 is insoluble (only soluble to a very small extent). Na2SO4 is completely soluble.

Rule 6. All hydroxide (OH^-) compounds are insoluble except those of Group I-A (alkali metals) and Ba²⁺, Ca²⁺, and Sr²⁺.

For example, Mg(OH)2 is insoluble (Ksp =7.1 ´ 10-12); NaOH and Ba(OH)2 are soluble, completely dissociating in aqueous solution: NaOH => Na+ + OH-, Ba(OH)2(s) => Ba2+ + 2OH-

Rule 7. All sulfide (S⁼) compounds are insoluble except those of Groups I-A and II-A (alkali metals and alkali earths).

For example, Na2S is soluble, MnS is insoluble.

Rule 8. All sulfites (SO₃⁼), carbonates (CO₃⁼), chromates (CrO₄⁼), and phosphates (PO₄⁼) are insoluble except for those of NH₄⁺ and Group I-A (alkali metals).

For example, calcite, CaCO3(s) <=> Ca2+ + CO3=, Ksp=4.5 ´ 10-9