A basic knowledge of which compounds are soluble in aqueous solutions is essential for predicting whether a given reaction might involve formation of a precipitate (aka a solid). The solubility rules are essential in remembering if a compound can be dissolved in water or not. Here are the rules:
Rule 1. All compounds of Group IA elements (the alkali metals) are soluble.
Rule 2. All ammonium salts (salts of NH4+) are soluble.
Rule 3. All nitrate (NO3-), chlorate (ClO3-), perchlorate (ClO4-), and acetate (CH3COO- or C2H3O2-, sometimes abbreviated as Oac-) salts are soluble.
Rule 4. All chloride (Cl-), bromide (Br-), and iodide (I-) salts are soluble except for those of Ag+, Pb2+, and Hg22+.
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.
Rule 6. All hydroxide (OH-) compounds are insoluble except those of Group I-A (alkali metals) and Ba2+, Ca2+, and Sr2+.
Rule 7. All sulfide (S2-) compounds are insoluble except those of Groups I-A and II-A (alkali metals and alkali earths).
Rule 8. All sulfites (SO3=), carbonates (CO3=), chromates (CrO4=), and phosphates (PO43-) are insoluble except for those of NH4+ and Group I-A (alkali metals)(see rules 1 and 2).
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