Editing Brine (section)

==Uses==
===Iodine and bromine mining===
[[Iodine]], essential for human health, is obtained on a commercial scale from iodide-rich brines.  The purification begins by converting iodide to hydroiodic acid, which is then oxidized to iodine using chlorine.  The iodine is then separated by evaporation or adsorption.<ref>{{cite book |doi=10.1002/14356007.a14_381.pub2 |chapter=Iodine and Iodine Compounds |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2015 |last1=Lyday |first1=Phyllis A. |last2=Kaiho |first2=Tatsuo |pages=1–13 |isbn=978-3-527-30673-2 }}</ref>  Bromine is also obtained from brines.  Akin to the production of iodine, the process exploits the easy oxidation of [[bromide]] into [[bromine]], again using chlorine as the oxidant.  The product bromine can be selectively collected by exploiting its volatility.<ref>{{cite book |doi=10.1002/14356007.a04_391 |chapter=Bromine |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2000 |last1=Mills |first1=Jack F. |isbn=3-527-30673-0 }}</ref>

===Lithium and magnesium mining===
Major deposits of [[lithium]] are in the form of brines.<ref>{{cite book |doi=10.1002/14356007.a15_393.pub2 |chapter=Lithium and Lithium Compounds |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2014 |last1=Wietelmann |first1=Ulrich |last2=Steinbild |first2=Martin |pages=1–38 |isbn=978-3-527-30385-4 }}</ref>  Magnesium is also produced in part from waste brine from various sources, such as potash production.  Crude magnesium oxides and chlorides mixtures are converted into magnesium metal by [[electrolysis]].<ref>{{cite book |doi=10.1002/14356007.a15_559 |chapter=Magnesium |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2003 |last1=Amundsen |first1=Ketil |last2=Aune |first2=Terje Kr. |last3=Bakke |first3=Per |last4=Eklund |first4=Hans R. |last5=Haagensen |first5=Johanna Ö. |last6=Nicolas |first6=Carlos |last7=Rosenkilde |first7=Christian |last8=Van Den Bremt |first8=Sia |last9=Wallevik |first9=Oddmund |isbn=978-3-527-30385-4 }}</ref>

===Chlorine production===
{{main|Chlorine production}}
Elemental chlorine can be produced by [[electrolysis]] of brine ([[NaCl]] solution). This process also produces [[sodium hydroxide]] (NaOH) and [[hydrogen]] gas (H<sub>2</sub>). The reaction equations are as follows:

* Cathode: {{chem2|2 H+ + 2 e- -> H2 ↑}}
* Anode: {{chem2|2 Cl- -> Cl2 ↑ + 2 e-}}
* Overall process: {{chem2|2 NaCl + 2 H2O -> Cl2 + H2 + 2 NaOH}}

===Refrigerating fluid===<!--[[Brine (refrigerant)]] redirects here-->
Brine (primarily cheap brines based on [[calcium chloride]] and [[sodium chloride]]<ref name="Cool-Info">{{cite web |title=Secondary Refrigerant Systems |url=http://www.cool-info.co.uk/brines_steam/secondary_refrigerants/sec_refrig01.html |access-date=17 July 2017 |work=Cool-Info.com}}</ref>) is used as a secondary [[fluid]] in large refrigeration installations to transport [[thermal energy]]. It is used because the addition of salt to water lowers the freezing temperature of the solution, significantly enhancing its heat transport efficiency at low cost. The lowest freezing point obtainable for NaCl brine (called its [[eutectic]] point) is {{convert|−21.1|C}} at the concentration of 23.3% NaCl by weight.<ref name="Cool-Info" />

Because of their corrosive properties, salt-based brines have been replaced by organic liquids such as [[ethylene glycol]].<ref>{{cite web |url= http://www.accent-refrigeration.com/tips/design-tips/calcium-chloride-versus-glycol |title= Calcium Chloride versus Glycol |work= accent-refrigeration.com |access-date=17 July 2017}}</ref>

Sodium chloride brine spray is used on some fishing vessels to freeze fish.<ref name=fish>{{cite book |url= http://seafood.oregonstate.edu/.pdf%20Links/Planning-for-Seafood-Freezing.pdf |title= Planning for Seafood Freezing |first1= Edward |last1= Kolbe |first2= Donald |last2= Kramer |series= Alaska Sea Grant College Program [[Oregon State University]] |date= 2007 |isbn= 978-1566121194 |access-date= 17 July 2017 |archive-url= https://web.archive.org/web/20170712134414/http://seafood.oregonstate.edu/.pdf%20Links/Planning-for-Seafood-Freezing.pdf |archive-date= 12 July 2017 |url-status= dead }}</ref> The brine temperature is generally {{convert|-5|F|C}}. Air blast freezing temperatures are {{convert|-31|F|C}} or lower. Given the higher temperature of brine, the system efficiency over air blast freezing can be higher. High-value fish usually are frozen at much lower temperatures, below the practical temperature limit for brine.

===Water softening and purification===
Brine is used for regeneration of [[ion-exchange resin]]s.<ref>{{Cite book| title=The NALCO Water Handbook |editor-last=Kemmer |editor-first=Frank N. |publisher=McGraw-Hill |year=1979 |pages=12–7; 12–25}}</ref> After treatment, ion-exchange resin beads saturated with [[calcium]] and [[magnesium]] ions from the treated water, are regenerated by soaking in brine containing 6–12% NaCl. The [[sodium]] ions from brine replace the calcium and magnesium ions on the beads.<ref>{{cite web|url=http://www.bbc.co.uk/schools/gcsebitesize/science/triple_aqa/water/hard_soft_water/revision/4/ |title= Hard and soft water |website=GCSE Bitesize |publisher=BBC}}</ref><ref name="SenGupta2016">{{cite book|author=Arup K. SenGupta|title=Ion Exchange and Solvent Extraction: A Series of Advances|url=https://books.google.com/books?id=hf4sYJfDYm8C&pg=PA125|date= 2016|publisher=CRC Press|isbn=978-1-4398-5540-9|pages=125–}}</ref>

===Culinary===
{{main|Brining}}
Brine is a common agent in food processing and cooking. Brining is used to [[Food preservation|preserve]] or [[seasoning|season]] the food. Brining can be applied to [[vegetable]]s, [[cheese]]s, [[fruit]] and some fish in a process known as [[pickling]]. [[Meat]] and [[fish]] are typically [[steeping|steeped]] in brine for shorter periods of time, as a form of [[marination]], enhancing its [[meat tenderness|tenderness]] and [[Flavoring|flavor]], or to enhance shelf period.

===De-icing===
In lower temperatures, a brine solution can be used to [[De-icing|de-ice]] or reduce freezing temperatures on roads.<ref>{{cite web|url=http://www.usroads.com/journals/rmj/9702/rm970202.htm|title=Prewetting with Salt Brine for More Effective Roadway Deicing|website=www.usroads.com|access-date=2012-01-14|archive-url=https://web.archive.org/web/20150107172008/http://www.usroads.com/journals/rmj/9702/rm970202.htm|archive-date=2015-01-07|url-status=dead}}</ref>

===Quenching===
[[Quenching]] is a heat-treatment process when forging metals such as steel. A brine solution, along with oil and other substances, is commonly used to harden steel. When brine is used, there is an enhanced uniformity of the cooling process and heat transfer.<ref>3.	Luís H. Pizetta Zordão, Vinícius A. Oliveira, George E. Totten, Lauralice C.F. Canale, "Quenching power of aqueous salt solution", ''International Journal of Heat and Mass Transfer'', Volume 140, 2019, pp. 807–818.</ref>