Sulfate

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In inorganic chemistry, a sulfate (IUPAC-recommended spelling; also sulphate in British English) is a salt of sulfuric acid.

Chemical properties

The sulfate ion is a polyatomic anion with the empirical formula SO₄²⁻ and a molecular mass of 96.06 daltons; it consists of one central sulfur atom surrounded by four identical oxygen atoms in a tetrahedral arrangement. The sulfate ion carries a negative two formal charge and is the conjugate base of the hydrogensulfate ion, HSO₄⁻, which is the conjugate base of H₂SO₄, sulfuric acid.

A sulfate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic compound. Almost all sulfates are soluble in water at standard temperature and pressure. Exceptions include calcium, strontium and barium sulfates.

Uses

Sulfates, also known as sulfur oxides, are important in both the chemical industry and biological systems:

• The Lead-acid battery typically uses sulfuric acid.
• Organisms living near deep sea thermal vents depend on sulfates for energy in lieu of the sun.
• Copper sulfate is a common algaecide.
• Magnesium sulfate, commonly known as Epsom salts, is used in therapeutic baths.

Oxoanion Sulfides

• SO₅²⁻ persulfate ion
• SO₄²⁻ sulfate ion
• SO₃²⁻ sulfite ion
• SO₂²⁻ hyposulfite ion

Sulfates occur as microscopic particles (aerosols) resulting from fossil fuel and biomass combustion. They increase the acidity of the atmosphere and form acid rain. There is a negative radiative forcing from aerosols because, while in the atmosphere, they reflect incoming solar radiation. This is an increase in albedo.ca:Sulfat da:Sulfat de:Sulfate es:Sulfato fr:Sulfate it:Solfati lv:Sulfāti nl:Sulfaat pl:Siarczan pt:Sulfato sr:Сулфат sv:Sulfat