'''Sulfate''' is the IUPAC name for the SO
42- ion, consisting of a central
sulfur atom single
bonded to four
tetrahedrally oriented
oxygen atoms. This
anion has a net negative two
electric charge.
Almost all ionic
compounds with sulfate anions are soluble in
water at standard temperature and pressure (the exceptions include CaSO
4, SrSO
4, and BaSO
4).
The
acid of the sulfate ion is H
2SO
4, called
sulfuric acid.
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.
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.
Category:Oxyanions
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