Bicarbonate



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In carbonic acid.

Bicarbonate serves a crucial biochemical role in the physiological pH buffering system.[1]

Chemical properties

 

The bicarbonate ion (hydrogen carbonate) is an anion with the equilibrium reactions.

CO32- +2 H2O ⇋ HCO31- + H2O + OH1- ⇋ H2CO3 +2 OH1-

H2CO3 +2 H2O ⇋ HCO31- + H3O1+ + H2O ⇋ CO32- +2 H3O1+

A bicarbonate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic water quality.

Biochemical role

Bicarbonate is a vital component of the carbonic acid (H2CO3), which can quickly turn into bicarbonate (HCO3-).

With carbonic acid as the alkalosis.)

Other uses

The most common salt of the bicarbonate ion is carbon dioxide. This is used as a leavening agent in baking.

The flow of bicarbonate ions from rocks weathered by the carbonic acid in rainwater is an important part of the carbon cycle.

Bicarbonate also serves in the digestive system. It raises the internal pH of the stomach, after highly acidic digestive juices have finished in their digestion of food.

Diagnostics

In diagnostic medicine, the blood value of bicarbonate is one of several indicators of the state of acid-base physiology in the body.

The parameter Standard bicarbonate concentration (SBCe) is the bicarbonate concentration in the blood at a Celsius.[2]

Bicarbonate compounds

References

  1. ^ a b c http://www.biology.arizona.edu/biochemistry/problem_sets/medph/intro.html
    Biology.arizona.edu - October 2006. Clinical correlates of pH levels: bicarbonate as a buffer.
  2. ^ Acid Base Balance (page 3)

See also

v • d • e
Inorganic compounds containing carbon
Common oxides: Carbides
 
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