Bicarbonate

In inorganic chemistry, a bicarbonate (IUPAC-recommended nomenclature: hydrogencarbonate) is an intermediate form in the deprotonation of carbonic acid.

Chemical properties

The bicarbonate ion is a polyatomic anion with the empirical formula H C O₃⁻ and a molecular mass of 61.02 daltons; it consists of one central carbon atom surrounded by three identical oxygen atoms in a trigonal planar arrangement, with a hydrogen atom attached to one of the oxygens. The bicarbonate ion carries a negative one formal charge and is the conjugate base of carbonic acid, H₂CO₃; it is the conjugate acid of CO₃²⁻, the carbonate ion.

A bicarbonate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic compound. Many bicarbonates are soluble in water at standard temperature and pressure.

Uses

The most common salt of the bicarbonate ion is sodium bicarbonate, NaHCO₃, which is used as baking soda. When exposed to an acid such as acetic acid (vinegar), bicarbonates release carbon dioxide. This is used to cause bread to rise in baking and to propel toy rockets.

The bicarbonate/carbonate ionic system is also a buffer in blood.

This chemical is also found in the blood. It is a crucial component of the acid/base system of the body (maintaining homeostasis). 86%-90% of CO₂ in the body is converted into H₂CO₃ which also can turn into its basic form HCO₃⁻, a polyprotic acid.

Occasionally bicarbonates are referred to as acid carbonates.

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Chemical properties

Uses

See also