Editing Alkalinity (section)

== Detailed description ==
Alkalinity measures the ability of a solution to neutralize [[acid]]s to the [[equivalence point]] of carbonate or bicarbonate, defined as pH 4.5 for many oceanographic/limnological studies.<ref>{{Cite journal|last=Dickson|first=A.G.|date=June 1981|title=An exact definition of total alkalinity and a procedure for the estimation of alkalinity and total inorganic carbon from titration data|url=https://linkinghub.elsevier.com/retrieve/pii/0198014981901217|journal=Deep Sea Research Part A. Oceanographic Research Papers|language=en|volume=28|issue=6|pages=609–623|doi=10.1016/0198-0149(81)90121-7|bibcode=1981DSRA...28..609D |url-access=subscription}}</ref> The alkalinity is equal to the [[stoichiometric]] sum of the [[base (chemistry)|base]]s in solution.  In most Earth surface waters [[carbonate alkalinity]] tends to make up most of the total alkalinity due to the common occurrence and dissolution of [[carbonate]] rocks and other geological [[weathering]] processes that produce carbonate anions. Other common natural components that can contribute to alkalinity include [[borate]], [[hydroxide]], [[phosphate]], [[silicate]], dissolved [[ammonia]], and the [[conjugate acid|conjugate bases]] of [[organic acids]] (e.g., [[acetate]]). Solutions produced in a laboratory may contain a virtually limitless number of species that contribute to alkalinity. Alkalinity is frequently given as molar equivalents per liter of solution or per kilogram of solvent. In commercial (e.g. the swimming pool industry) and regulatory contexts, alkalinity might also be given in parts per million of equivalent calcium carbonate (ppm CaCO<sub>3</sub>){{Citation needed|date=April 2023}}. Alkalinity is sometimes incorrectly used interchangeably with [[Base (chemistry)|basicity]].   For example, the addition of CO<sub>2</sub> lowers the pH of a solution, thus reducing  basicity while alkalinity remains unchanged ([[#Addition of CO2|see example below]]).

A variety of [[Titration|titrants]], endpoints, and [[PH indicator|indicators]] are specified for various alkalinity measurement methods.  [[Hydrochloric acid|Hydrochloric]] and [[Sulfuric acid|sulfuric]] acids are common acid titrants, while [[Phenolphthalein|phenolpthalein]], [[methyl red]], and [[bromocresol green]] are common indicators.<ref>{{Citation |title=2320 alkalinity |date=2017-08-27 |url=https://www.standardmethods.org/doi/10.2105/SMWW.2882.023 |series=Standard Methods for the Examination of Water and Wastewater |publisher=American Public Health Association |doi=10.2105/smww.2882.023 |doi-broken-date=1 November 2024 |isbn=9780875532998 |access-date=2022-12-01}}</ref>