Solubility Rules PDF

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This is a summary of the solubility rules for chemicals...

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Solubility Rules In principle, all ionic compounds dissolve in water to some extent, though this may be very slight. For practical purposes, we consider a compound to be insoluble if the maximum amount that can dissolve is less than about 0.01 mole per liter. To predict the solubility of different ionic compounds, we can use a set of approximate solubility rules as follows. I.

Compounds that are always soluble: – Those that contain alkali metal cations (Li+, Na+, K+, Rb+, Cs+) or the ammonium ion (NH4+). – Those that contain the anions nitrate (NO3 G), perchlorate (ClO4 G), or acetate (C2H3O2 G).

II. Compounds that are usually soluble: – Those that contain chloride, bromide, or iodide ions. Exceptions: salts containing Pb2+, Ag+, or Hg22+ are insoluble. – Those that contain sulfate (SO4 2G). Exceptions: salts containing Sr2+, Ba2+, Pb2+, Hg2 2+. CaSO4 is slightly soluble. III. Compounds that are mostly insoluble: – Those that contain sulfide (S2G). Exceptions: salts containing NH4 + or the grou p I and II cations are soluble. – Those that contain hydroxide (OHG). Exceptions: salts containing NH4 + or the group I and II cations (except Be2+ and Mg2+) are soluble. – Those that contain carbonate (CO3 2G) or phosphate (PO43G). Exceptions: salts containing NH4+ or the group I cations are soluble.

These rules are taken from “General Chemistry Principles and Modern Applications 8'th Ed.,” Petrucci, Harwood, and Herring, Prentice Hall, Upper Saddle River, NJ 2002....