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Sulfate

Many examples of ionic sulfates are known, and many of these are highly soluble in water. Exceptions include calcium sulfate, strontium sulfate, and barium sulfate, which are poorly soluble. The barium derivative is useful in the gravimetric analysis of sulfate: one adds a solution of, perhaps, barium chloride to a solution containing sulfate ions. The appearance of a white precipitate, which is barium sulfate, indicates that sulfate anions are present.

The sulfate ion can act as a ligand attaching either by one oxygen (monodentate) or by two oxygens as either a chelate or a bridge.[1] An example is the neutral metal complex PtSO4P(C6H5)32 where the sulfate ion is acting as a bidentate ligand. The metal-oxygen bonds in sulfate complexes can have significant covalent character

- Sodium Sulfate
- Iron Sulfate
- Iron Sulphate
- Zinc Sulfate
- Magnesium Sulfate
- Manganese Sulfate
- Barium Sulfate
- Ammonium Sulfate
- Copper Sulfate
- Ferrous Sulfate
- Basic Chromium Sulfate
- Tin Sulfate
- Calcium Sulfate
- Ferric Sulfate
- Potassium Sulfate
- Lithium Sulfate
- Aluminium Sulfate


  Copper Sulfate

Copper(II) sulfate is the chemical compound with the formula CuSO4. This salt exists as a series of compounds that differ in their degree of hydration. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. This hydrated copper sulfate occurs in nature as the mineral called chalcanthite. Archaic names for copper(II) sulfate are "blue vitriol" and "blue stone"




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