Editing Bicarbonate (section)

==Chemical properties==
The bicarbonate ion (hydrogencarbonate ion) is an [[anion]] with the [[empirical formula]] {{chem2|HCO3-}} and a molecular mass of 61.01 [[atomic mass unit|daltons]]; it consists of one central carbon [[atom]] surrounded by three oxygen atoms in a [[trigonal planar]] arrangement, with a hydrogen atom attached to one of the oxygens. It is [[isoelectronic]] with [[nitric acid]] {{chem2|HNO3}}. The bicarbonate ion carries a negative one [[formal charge]] and is an [[Amphoterism#Amphiprotic molecules|amphiprotic]] species which has both acidic and basic properties. It is both the [[conjugate acid|conjugate base]] of [[carbonic acid]] {{chem2|H2CO3}}; and the [[conjugate acid]] of {{chem2|CO3(2−)}}, the [[carbonate]] ion, as shown by these [[chemical equilibrium|equilibrium]] reactions:
:{{chem2|CO3(2−) + 2 H2O <-> HCO3 + H2O + HO− <-> H2CO3 + 2 HO−}}
:{{chem2|H2CO3 + 2 H2O <-> HCO3- + H3O+ + H2O <-> CO3(2−) + 2 H3O+}}

A bicarbonate salt forms when a [[cation|positively charged ion]] attaches to the negatively charged oxygen atoms of the ion, forming an [[ionic compound]]. Many bicarbonates are [[solubility|soluble]] in [[aqueous solution|water]] at [[standard temperature and pressure]]; in particular, sodium bicarbonate contributes to [[total dissolved solids]], a common parameter for assessing [[water quality]].<ref>{{cite book|last1=Geor|first1=Raymond J.|last2=Coenen|first2=Manfred|last3=Harris|first3=Pat|title=Equine Applied and Clinical Nutrition: Health, Welfare and Performance|date=31 January 2013|publisher=Elsevier Health Sciences|isbn=978-0-7020-5418-1|page=90|language=en|quote=The most common indicator of water quality is the concentration of total dissolved solids (TDS)}}</ref>