View source for Sodium bicarbonate

{{short description|Chemical compound}}
{{distinguish|Sodium carbonate}}
{{For|the leavening agent of which baking soda is a common ingredient|Baking powder}}<!--following templates on the same line to prevent blank paragraphs:-->{{cs1 config|name-list-style=vanc}}{{Use dmy dates|date=January 2021}}
{{Chembox
| Watchedfields  = changed
| verifiedrevid  = 476996774
| Name           = 
| ImageFile      = SodiumBicarbonate.svg
| ImageClass     = skin-invert-image
| ImageSize      = 121
| ImageFileL1    = Sodium-3D.png
| ImageNameL1    = Ball and stick model of a sodium cation
| ImageFileR1    = Bicarbonate-ion-3D-balls.png
| ImageNameR1    = Ball and stick.







 model of a bicarbonate anion
| ImageFile2     = Sodium-bicarbonate-xtal-2x2x2-3D-bs-17.png
| ImageClass2    = bg-transparent
| ImageCaption2  = [[Crystal structure]]
| ImageFileL3    = Sodium-bicarbonate-xtal-Na-coord-3D-bs-17.png
| ImageClassL3   = bg-transparent
| ImageCaptionL3 = Na<sup>+</sup> [[Coordination geometry|coordination]]
| ImageFileR3    = Sodium-bicarbonate-xtal-HCO3-coord-3D-bs-17.png
| ImageClassR3   = bg-transparent
| ImageSizeR3    = 150px
| ImageCaptionR3 = HCO<sub>3</sub><sup>−</sup> coordination
| IUPACName      = sodium hydrogencarbonate
| OtherNames     = Baking soda, bicarb (laboratory slang), bicarbonate of soda, [[nahcolite]], natrium hydrogen carbonate, natron
| SystematicName = 
| Section1       = {{Chembox Identifiers
 | IUPHAR_ligand = 4507
 | CASNo = 144-55-8
 | CASNo_Ref = {{cascite|correct|CAS}}
 | PubChem = 516892
 | ChemSpiderID = 8609
 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
 | UNII = 8MDF5V39QO
 | UNII_Ref = {{fdacite|correct|FDA}}
 | EINECS = 205-633-8
 | DrugBank_Ref = {{drugbankcite|correct|drugbank}}
 | DrugBank = DB01390
 | KEGG_Ref = {{keggcite|correct|kegg}}
 | KEGG = C12603
 | MeSHName = Sodium+bicarbonate
 | ChEBI_Ref = {{ebicite|correct|EBI}}
 | ChEBI = 32139
 | ChEMBL = 1353
 | ChEMBL_Ref = {{ebicite|correct|EBI}}
 | RTECS = VZ0950000
 | Beilstein = 4153970
 | SMILES = [Na+].OC([O-])=O
 | StdInChI = 1S/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1
 | StdInChI_Ref = {{stdinchicite|correct|chemspider}}
 | InChI = 1/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1
 | StdInChIKey = UIIMBOGNXHQVGW-UHFFFAOYSA-M
 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
 | InChIKey = UIIMBOGNXHQVGW-REWHXWOFAQ
 }}
| Section2       = {{Chembox Properties
 | Formula = {{chem|Na|HCO|3}} {{cascite|correct|CAS}}<!--correct in PubChem: how do I cite that here?-->
 | MolarMass = 84.0066 g mol<sup>−1</sup>
 | Appearance = White crystals
 | Odor = Odorless
 | Density = {{unbulleted list
  | 2.20 g/cm<sup>3</sup><ref name=crc>Haynes, p. 4.90</ref>
  }}
| BoilingPtC = <!-- 851, conflicting sources, corresponds to MeltingPtC of sodium carbonate. See talk page September 2013. -->
| MeltingPtC = 
| MeltingPt_notes = (Decomposes to [[sodium carbonate]] starting at 50&nbsp;°C<ref name="crc"/><ref>{{cite journal |doi=10.1007/s10973-006-8182-1 |title=Thermal behaviour of diclofenac, diclofenac sodium and sodium bicarbonate compositions |journal=Journal of Thermal Analysis and Calorimetry |volume=90 |issue=3 |pages=903–907 |year=2007| vauthors = Pasquali I, Bettini R, Giordano F |s2cid=95695262 }}</ref>)
| Solubility = {{unbulleted list
 | 69 g/L (0&nbsp;°C)<ref name=crc3>Haynes, p. 5.194</ref><ref name=UNEP>{{cite web|publisher=[[United Nations Environment Programme]]|url=http://www.chem.unep.ch/irptc/sids/oecdsids/Sodium%20bicarbonate.pdf|title=Sodium Bicarbonate|url-status=dead|archive-url=https://web.archive.org/web/20110516015331/http://www.chem.unep.ch/irptc/sids/oecdsids/Sodium%20bicarbonate.pdf|archive-date=16 May 2011}}</ref>
 | 96 g/L (20&nbsp;°C)<ref name=crc3/><ref name=UNEP/>
 | 165 g/L (60&nbsp;°C)<ref name=crc3/><ref name=UNEP/>
 }}
| SolubleOther = 0.02 wt% acetone, 2.13 wt% methanol @22&nbsp;°C.,<ref>{{cite journal | title = Solubilities of Sodium Carbonate and Sodium Bicarbonate in Acetone-Water and Methanol-Water Mixtures | journal = J. Chem. Eng. Data | year = 1966 | volume = 11 | issue = 3 | pages = 323–324 | doi = 10.1021/je60030a009| vauthors = Ellingboe JL, Runnels JH }}</ref> insoluble in [[ethanol]]{{cn|date=June 2025}}
| LogP = −0.82
| pKa = {{unbulleted list
 | 6.34<ref name=crc4>Haynes, p. 7.23</ref>
 | 6.351 (carbonic acid)<ref name=crc4/>
 }}
| RefractIndex = nα = 1.377 nβ = 1.501 nγ = 1.583
 }}
| Section3       = {{Chembox Structure
 | CrystalStruct = Monoclinic
 }}
| Section6       = {{Chembox Pharmacology
 | ATCCode_prefix = B05
 | ATCCode_suffix = CB04
 | ATC_Supplemental = {{ATC|B05|XA02}}, {{ATCvet|G04|BQ01}}
 | AdminRoutes = Intravenous, oral
 }}
| Section4       = 
| Section5       = {{Chembox Thermochemistry
 | DeltaHf = −950.8 kJ/mol<ref name=crc2>Haynes, p. 5.19</ref>
 | DeltaGf = −851.0 kJ/mol<ref name=crc2/>
 | Entropy =  101.7 J/mol K<ref name=crc2/>
 | HeatCapacity = 87.6 J/mol K<ref name=crc2/>
 }}
| Section7       = {{Chembox Hazards
 | ExternalSDS = [https://web.archive.org/web/20090306164850/http://siri.org/msds/f2/bdm/bdmjw.html External MSDS]
 | MainHazards = Causes serious eye irritation
 | NFPA-H = 2
 | NFPA-F = 0
 | NFPA-R = 1
 | LD50 = 4220 mg/kg (rat, oral)<ref>{{cite journal | last=Griffith | first=John F. | title=Interlaboratory variations in the determination of acute oral LD50 | journal=Toxicology and Applied Pharmacology | volume=6 | issue=6 | date=1964 | doi=10.1016/0041-008X(64)90124-3 | pages=726–730| pmid=14235840 }}</ref>
 | FlashPt = Incombustible
 }}
| Section8       = {{Chembox Related
 | OtherAnions = [[Sodium carbonate]]
 | OtherCations = {{unbulleted list
  | [[Ammonium bicarbonate]]
  | [[Potassium bicarbonate]]
  }}
 | OtherCompounds = {{unbulleted list
  | [[Sodium bisulfate]]
  | [[Sodium hydrogen phosphate]]
  }}
 }}
}}
[[File:Cupcake2020.jpg|thumb|Cupcakes baked with baking soda as a raising agent]]
'''Sodium bicarbonate''' ([[IUPAC name]]: '''sodium hydrogencarbonate'''<ref>{{Citation
 |url         = http://old.iupac.org/publications/books/rbook/Red_Book_2005.pdf
 |title       = Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005
 |publisher   = IUPAC
 |page        = 137
 |url-status     = live
 |archive-url  = https://web.archive.org/web/20170518230415/http://old.iupac.org/publications/books/rbook/Red_Book_2005.pdf
 |archive-date = 2017-05-18
}}</ref>), commonly known as '''baking soda''' or '''bicarbonate of soda''' (or simply "'''bicarb'''", especially in the UK), or '''salaratus''', is a [[chemical compound]] with the formula '''NaHCO<sub>3</sub>'''. It is a [[salt (chemistry)|salt]] composed of a [[sodium]] [[cation]] ([[Sodium|Na<sup>+</sup>]]) and a [[bicarbonate]] [[anion]] ({{chem2|HCO3-}}). Sodium bicarbonate is a white solid that is [[crystal]]line but often appears as a fine powder. It has a slightly salty, [[alkaline]] taste resembling that of [[sodium carbonate]] ("washing soda"). The natural mineral form is [[nahcolite]], although it is more commonly found as a component of the mineral [[trona]].<ref name=":4">{{Cite journal |last1=Gärtner |first1=Robert S. |last2=Witkamp |first2=Geert-Jan |date=August 2007 |title=Mixed solvent reactive recrystallization of trona (sodium sesqui-carbonate) into soda (sodium carbonate anhydrate) |url=https://linkinghub.elsevier.com/retrieve/pii/S0304386X07000758 |journal=Hydrometallurgy |language=en |volume=88 |issue=1–4 |pages=75–91 |doi=10.1016/j.hydromet.2007.03.006|bibcode=2007HydMe..88...75G |url-access=subscription }}</ref>

As it has long been known and widely used, the salt has many different names such as baking soda, bread soda, cooking soda, brewing soda and bicarbonate of soda and can often be found near [[baking powder]] in stores. The term ''baking soda'' is more common in the United States, while ''bicarbonate of soda'' is more common in Australia, the United Kingdom, and New Zealand.<ref>{{Cite web |title=Baking powder, baking soda or bicarbonate of soda? |url=https://www.readersdigest.com.au/recipes/bicarb-soda-versus-baking-powder |access-date=2024-06-02 |website=Reader's Digest Australia |language=en-US}}</ref> Abbreviated colloquial forms such as ''sodium bicarb'','' bicarb soda'', ''bicarbonate'', and ''bicarb'' are common.<ref>{{cite web|last=PubChem|title=Sodium bicarbonate|url=https://pubchem.ncbi.nlm.nih.gov/compound/516892|access-date=2021-01-25|website=pubchem.ncbi.nlm.nih.gov|language=en}}</ref>

The prefix ''bi-'' in "bicarbonate" comes from an outdated naming system predating molecular knowledge. It is based on the observation that there is twice as much carbonate ({{chem2|CO3(2-)}}) per sodium in sodium bicarbonate (NaHCO<sub>3</sub>) as there is in sodium carbonate (Na<sub>2</sub>CO<sub>3</sub>).<ref>{{cite journal|last=Wollaston|first=WH|date=January 1814|title=I. A Synoptic scale of chemical equivalents|url=https://royalsocietypublishing.org/doi/10.1098/rstl.1814.0001|journal=Philosophical Transactions of the Royal Society of London|volume=104|pages=1–22|doi=10.1098/rstl.1814.0001|s2cid=96774986|url-access=subscription}}</ref> The modern chemical formulas of these compounds now express their precise chemical compositions which were unknown when the name ''bi-carbonate of potash'' was coined (see also: [[bicarbonate]]).

==Uses==

===Cooking===

{{Main|Leavening agent}}{{Cookbook|Baking Soda}}
In cooking, baking soda is primarily used in [[baking]] as a [[leavening agent]]. When it reacts with acid or is heated, carbon dioxide is released, which causes expansion of the batter and forms the characteristic texture and grain in cakes, [[quick bread]]s, [[soda bread]], and other baked and fried foods. When an acid is used, the [[acid–base reaction]] can be generically represented as follows:<ref>{{cite book | veditors = Bent AJ | title=The Technology of Cake Making | edition=6 | year=1997 | page=102 | publisher=Springer | isbn=9780751403497 | url=https://books.google.com/books?id=OTy8aIWxHhQC&pg=PA102 | access-date=12 August 2009}}</ref>

:NaHCO<sub>3</sub> + H<sup>+</sup> → Na<sup>+</sup> + CO<sub>2</sub> + H<sub>2</sub>O

Acidic materials that induce this reaction include [[Monohydrogen phosphate|hydrogen phosphates]], [[cream of tartar]], [[lemon]] juice, [[yogurt]], [[buttermilk]], [[Cocoa solids|cocoa]], and [[vinegar]]. Baking soda may be used together with [[sourdough]], which is acidic, making a lighter product with a less acidic taste.<ref>{{cite web|last=Cascio|first=Julie|title=Sourdough|url=https://www.uaf.edu/files/ces/publications-db/catalog/hec/FNH-00061.pdf|url-status=dead|archive-url=https://web.archive.org/web/20160327162100/https://www.uaf.edu/files/ces/publications-db/catalog/hec/FNH-00061.pdf|archive-date=27 March 2016|access-date=2 May 2017|publisher=University of Alaska Fairbanks [[Alaska Cooperative Extension Service|Cooperative Extension Service]]|id=FNH-00061}}</ref> Since the reaction occurs slowly at room temperature, mixtures (cake batter, etc.) can be allowed to stand without rising until they are heated in the oven.{{citation needed|date=March 2020}}

Heat can also by itself cause sodium bicarbonate to act as a raising agent in baking because of [[thermal decomposition]], releasing carbon dioxide at temperatures above {{convert|80|C|F|-1}}, as follows:<ref>{{cite news|url=http://foodreference.about.com/od/Ingredients_Basics/a/What-Is-Baking-Soda.htm|title=The Many Practical Uses of Baking Soda in the Kitchen|newspaper=About.com Food|access-date=22 January 2017|archive-date=2 February 2017|archive-url=https://web.archive.org/web/20170202011456/http://foodreference.about.com/od/Ingredients_Basics/a/What-Is-Baking-Soda.htm|url-status=dead}}</ref><!-- note that The Technology of Cake Making says something different, that effectively the reaction is actually 4 NaHCO<sub>3</sub> → Na<sub>2</sub>CO<sub>3</sub>·2 NaHCO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O so that only one quarter of the available CO<sub>2</sub> is released. -->

: 2 NaHCO<sub>3</sub> → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O + CO<sub>2</sub>

When used this way on its own, without the presence of an acidic component (whether in the batter or by the use of a baking powder containing acid), only half the available CO<sub>2</sub> is released (one CO<sub>2</sub> molecule is formed for every two equivalents of NaHCO<sub>3</sub>). Additionally, in the absence of acid, thermal decomposition of sodium bicarbonate also produces [[sodium carbonate]], which is strongly alkaline and gives the baked product a bitter, soapy taste and a yellow color.

==== Baking powder ====
{{main|Baking powder}}
[[Baking powder]], also sold for cooking, contains around 30% of bicarbonate, and various acidic ingredients that are activated by the addition of water, without the need for additional acids in the cooking medium.<ref>{{cite web|url=http://nzic.org.nz/ChemProcesses/food/6D.pdf|title= The Chemistry of Baking | vauthors = Czernohorsky JH, Hooker R |publisher=New Zealand Institute of Chemistry|access-date=22 January 2017|archive-url=https://web.archive.org/web/20161127151812/http://nzic.org.nz/ChemProcesses/food/6D.pdf|archive-date=27 November 2016|url-status=dead}}</ref><ref>{{cite news|url=http://www.finecooking.com/item/12173/baking-soda-and-baking-powder|title=Baking Soda and Baking Powder|website=FineCooking.com|language=en|access-date=22 January 2017|archive-date=2 February 2017|archive-url=https://web.archive.org/web/20170202020545/http://www.finecooking.com/item/12173/baking-soda-and-baking-powder|url-status=dead}}</ref><ref>{{cite web |url=http://www.armandhammer.com/FAQ/BakingSoda.aspx |title=Baking Soda FAQs |website=Arm & Hammer Multi-Brand |publisher=Church & Dwight Company |access-date=20 July 2017 |at=What is the difference baking soda and baking powder?|url-status=dead |archive-url=https://web.archive.org/web/20170627082018/http://www.armandhammer.com/FAQ/bakingsoda.aspx |archive-date=27 June 2017 }}</ref> Many forms of baking powder contain sodium bicarbonate combined with [[calcium acid phosphate]], [[sodium aluminium phosphate]], or [[cream of tartar]].<ref>{{cite web|title=Glossary Ingredients|url=http://www.cooking.com/recipes-and-more/glossary.aspx?GlossName=Baking+powder|url-status=dead|archive-url=https://web.archive.org/web/20080915045426/http://www.cooking.com/recipes-and-more/glossary.aspx?GlossName=Baking+powder|archive-date=15 September 2008|publisher=Cooking.com}}</ref> Baking soda is alkaline; the acid used in baking powder avoids a metallic taste when the chemical change during baking creates sodium carbonate.<ref>{{cite web|date=2016-07-11|title=Sodium Bicarbonate|url=http://brpadhikarychemicals.com/high-density-polyethylene-hdpe/|access-date=2021-01-25|website=BRP Adhikary|language=en}}</ref>

===Food additive===
It is often used in conjunction with other [[bottled water]] [[food additive]]s to add taste.<ref>{{Cite magazine|url=https://time.com/3029191/bottled-water-ingredients-nutrition-health/|title=Why Your Bottled Water Contains Four Different Ingredients|first=Becca|last=Stanek|date=24 July 2014|magazine=TIME}}</ref> Its [[European Union]] [[E number]] is E500.<ref>{{cite web|title=Approved additives and E numbers|url=https://www.food.gov.uk/business-guidance/approved-additives-and-e-numbers|access-date=7 December 2020|website=Food Standards Agency|language=en}}</ref>

===Pyrotechnics===
Sodium bicarbonate is one of the main components of the common [[Black snake (firework)|"black snake" firework]]. The effect is caused by the [[thermal decomposition]], which produces carbon dioxide gas to produce a long snake-like ash as a combustion product of the other main component, [[sucrose]].<ref name="MEL Science">{{cite web |title=Sugar snake |url=https://melscience.com/US-en/experiments/sugar-snake/ |website=MEL Science |publisher=MEL Science 2015–2019 |accessdate=28 October 2019 |archive-url=https://web.archive.org/web/20191006112734/https://melscience.com/US-en/experiments/sugar-snake/ |archive-date=6 October 2019 |url-status=live}}</ref> Sodium bicarbonate also delays combustion reactions through the release of carbon dioxide and water, both of which are flame retardants, when heated.

===Mild disinfectant===
It has weak [[disinfectant]] properties<ref name=Malik>{{cite journal | vauthors = Malik YS, Goyal SM | title = Virucidal efficacy of sodium bicarbonate on a food contact surface against feline calicivirus, a norovirus surrogate | journal = International Journal of Food Microbiology | volume = 109 | issue = 1–2 | pages = 160–3 | date = May 2006 | pmid = 16540196 | doi = 10.1016/j.ijfoodmicro.2005.08.033 }}</ref><ref>{{cite journal | vauthors = Rutala WA, Barbee SL, Aguiar NC, Sobsey MD, Weber DJ | title = Antimicrobial activity of home disinfectants and natural products against potential human pathogens | journal = Infection Control and Hospital Epidemiology | volume = 21 | issue = 1 | pages = 33–8 | date = January 2000 | pmid = 10656352 | doi = 10.1086/501694 | s2cid = 34461187 }}</ref> and it may be an effective [[fungicide]] against some organisms.<ref name=Zamani>{{cite journal | vauthors = Zamani M, Sharifi Tehrani A, Ali Abadi AA | title = Evaluation of antifungal activity of carbonate and bicarbonate salts alone or in combination with biocontrol agents in control of citrus green mold | journal = Communications in Agricultural and Applied Biological Sciences | volume = 72 | issue = 4 | pages = 773–7 | year = 2007 | pmid = 18396809 }}</ref>

===Fire extinguisher===
Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire, as heating of sodium bicarbonate releases carbon dioxide.<ref name=arm>{{cite web|url=http://www.armhammer.com/basics/magic|title=Arm & Hammer Baking Soda – Basics – The Magic of Arm & Hammer Baking Soda|website=armandhammer.com|archive-url=https://web.archive.org/web/20090831133032/http://www.armhammer.com/basics/magic|archive-date=31 August 2009|url-status=dead|access-date=30 July 2009}}</ref> However, it should not be applied to fires in [[deep fryer]]s; the sudden release of gas may cause the grease to splatter.<ref name=arm/> Sodium bicarbonate is used in BC [[Fire extinguishers#Dry chemical|dry chemical]] [[fire extinguishers]] as an alternative to the more corrosive [[monoammonium phosphate]] in ABC extinguishers. The alkaline nature of sodium bicarbonate makes it the only dry chemical agent, besides [[Purple-K]], that was used in large-scale fire suppression systems installed in commercial kitchens.<ref name=":0">{{cite web |last=Voelkert |first=J. Craig |date=2015 |title=Fire and Fire Extinguishment - A Brief Guide to Fire Chemistry and Extinguishment Theory for fire Equipment Service Technicians |url=https://www.amerex-fire.com/upl/downloads/educational-documents/fire-and-fire-extinguishment-99cd88b2.pdf |archive-url=https://web.archive.org/web/20240531221055/https://www.amerex-fire.com/upl/downloads/educational-documents/fire-and-fire-extinguishment-99cd88b2.pdf |archive-date=2024-05-31 |access-date=22 Sep 2023 |pages=14–15}}</ref>

Sodium bicarbonate has several fire-extinguishing mechanisms that act simultaneously. It decomposes into water and carbon dioxide when heated, an [[Endothermic process|endothermic reaction]] that deprives the fire of heat. In addition, it forms intermediates that can scavenge the [[Radical (chemistry)|free radicals]] which are responsible for the [[Combustion#Reaction mechanism|propagation of fire]].<ref name=":1">{{Cite journal |last1=Liu |first1=Yang |last2=Zhang |first2=Yansong |last3=Meng |first3=Xiangbao |last4=Yan |first4=Ke |last5=Wang |first5=Zheng |last6=Liu |first6=Jiqing |last7=Wang |first7=Zhifeng |last8=Yang |first8=Panpan |last9=Dai |first9=Wenjiao |last10=Li |first10=Fang |date=April 2022 |title=Research on flame propagation and explosion overpressure of oil shale dust explosion suppression by NaHCO3 |url=https://linkinghub.elsevier.com/retrieve/pii/S0016236121026417 |journal=Fuel |language=en |volume=314 |article-number=122778 |doi=10.1016/j.fuel.2021.122778|bibcode=2022Fuel..31422778L |url-access=subscription }}</ref> With [[fire classification|grease fires]] specifically, it also has a mild [[saponification]] effect, producing a soapy foam that can help smother the fire.<ref name=":0" />

===Neutralization of acids ===
Sodium bicarbonate reacts spontaneously with acids, releasing CO<sub>2</sub> gas as a reaction product. It is commonly used to neutralize unwanted acid solutions or acid spills in chemical laboratories.<ref>{{cite web | title = Prepare for Emergencies from Uncontrolled Hazards | url = https://www.acs.org/content/acs/en/chemical-safety/basics/prepare-for-emergencies.html | publisher = American Chemical Society }}</ref> It is not appropriate to use sodium bicarbonate to neutralize base<ref>{{cite web | title = Laboratory Safety | first = Deanna | last = Hurum | work = Civil Engineering | publisher = Northwestern University | url = http://faculty.washington.edu/korshin/Class-486/AEESP-safety-notes.pdf }}</ref> even though it is [[amphoterism|amphoteric]], reacting with both acids and bases.<ref name=":3">{{Cite journal |last=Davidson |first=David |date=November 1955 |title=Amphoteric molecules, ions and salts |url=https://pubs.acs.org/doi/abs/10.1021/ed032p550 |journal=Journal of Chemical Education |language=en |volume=32 |issue=11 |pages=550 |doi=10.1021/ed032p550 |bibcode=1955JChEd..32..550D |issn=0021-9584|url-access=subscription }}</ref>

===Sports supplement===
Sodium bicarbonate is taken as a sports supplement to improve muscular endurance.<ref>{{cite journal|vauthors = Grgic J, Rodriguez RF, Garofolini A, Saunders B, Bishop DJ, Schoenfeld BJ, Pedisic Z|title = Effects of Sodium Bicarbonate Supplementation on Muscular Strength and Endurance: A Systematic Review and Meta-analysis | journal = Sports Medicine | volume = 50 | issue = 7 | pages = 1361–1375 | date = July 2020 | pmid = 32096113 | doi = 10.1007/s40279-020-01275-y |s2cid = 211254185 |url = https://vuir.vu.edu.au/40625/ }}</ref> Studies conducted mostly in males have shown that sodium bicarbonate is most effective in enhancing performance in short-term, high-intensity activities.<ref name="pmid34794476">{{cite journal | vauthors=Grgic J, Grgic I, Pedisic Z| title=Effects of sodium bicarbonate supplementation on exercise performance: an umbrella review | journal=[[BioMed Central#BMC Series|Journal of the International Society of Sports Nutrition]] | volume=18 | issue=1 | article-number=71 | year=2021 | doi = 10.1186/s12970-021-00469-7 | pmc=8600864 | pmid=34794476 | doi-access=free }}</ref>

===Agriculture===
Sodium bicarbonate can prevent the growth of fungi when applied on leaves, although it will not kill the fungus. Excessive amounts of sodium bicarbonate can cause discolouration of fruits (two percent solution) and [[chlorosis]] (one percent solution).<ref>{{cite web|title=Horticulture myths|url=http://www.uvm.edu/pss/ppp/articles/myths.html|url-status=live|archive-url=https://web.archive.org/web/20190807145520/http://www.uvm.edu/pss/ppp/articles/myths.html|archive-date=7 August 2019|access-date=18 October 2021|website=University of Vermont Extension Department of Plant and Soil Science}}</ref> Sodium bicarbonate is also commonly used as a free choice dietary supplement in sheep to help prevent bloat.

===Medical uses and health===
{{see also|Intravenous sodium bicarbonate}}
Sodium bicarbonate mixed with water can be used as an [[antacid]] to treat [[acid indigestion]] and [[heartburn]].<ref>{{cite web|publisher=Jackson Siegelbaum Gastroenterology|url=http://gicare.com/medication/sodium-bicarbonate/|title=Sodium Bicarbonate|year=1998|access-date=4 October 2016|archive-url= https://web.archive.org/web/20161005124933/http://gicare.com/medication/sodium-bicarbonate/ |archive-date=5 October 2016 |url-status=dead}}</ref><ref>{{cite web |title=Sodium Bicarbonate (Oral Route, Intravenous Route, Subcutaneous Route) Side Effects - Mayo Clinic |url=https://www.mayoclinic.org/drugs-supplements/sodium-bicarbonate-oral-route-intravenous-route-subcutaneous-route/side-effects/drg-20065950?p=1 |access-date=2023-05-05 |website=www.mayoclinic.org}}</ref> Its reaction with [[stomach acid]] produces [[sodium chloride|salt]], water, and [[carbon dioxide]]:
:NaHCO<sub>3</sub> + HCl → NaCl + H<sub>2</sub>O + CO<sub>2</sub>(g)

A mixture of sodium bicarbonate and [[polyethylene glycol]] dissolved in water and taken orally, is an effective [[gastrointestinal lavage]] preparation and [[laxative]] prior to gastrointestinal surgery, [[gastroscopy]], etc.{{citation needed|date=March 2020}}

[[Intravenous sodium bicarbonate]] in an aqueous solution is sometimes used for cases of [[acidosis]], or when insufficient sodium or bicarbonate ions are in the blood.<ref>{{cite web|publisher=Better Health Channel |url= http://www.betterhealth.vic.gov.au/bhcv2/bhcmed.nsf/pages/pucsodbi/$File/pucsodbi.pdf |title=Sodium Bicarbonate Intravenous Infusion |work=Consumer Medicine Information|date=13 July 2004|url-status=dead |archive-url= https://web.archive.org/web/20080822111454/http://www.betterhealth.vic.gov.au/bhcv2/bhcmed.nsf/pages/pucsodbi/$File/pucsodbi.pdf |archive-date=22 August 2008}}</ref> In cases of respiratory acidosis, the infused bicarbonate ion drives the carbonic acid/bicarbonate buffer of plasma to the left, and thus raises the pH{{Citation needed|date=July 2025}}. For this reason, sodium bicarbonate is used in medically supervised [[cardiopulmonary resuscitation]] {{Citation needed|date=July 2025}} <!-- Bicarb is no longer used in CPR as there is no data to support significant improvement in blood pH -->. Infusion of bicarbonate is indicated only when the blood [[pH]] is markedly low (&lt;&nbsp;7.1–7.0).<ref>{{cite web|publisher=emedicine|url=http://emedicine.medscape.com/article/301574-treatment|title=Respiratory Acidosis: Treatment & Medication|date=26 March 2020}}</ref>

HCO<sub>3</sub><sup>−</sup> is used for treatment of [[hyperkalemia]], as it will drive K<sup>+</sup> back into cells during periods of acidosis.<ref>{{cite book| last = Dart | first = Richard C. |title=Medical Toxicology|url=https://books.google.com/books?id=BfdighlyGiwC&pg=PA910|year=2004|publisher=Lippincott Williams & Wilkins|isbn=978-0-7817-2845-4|pages=910–}}</ref>{{Irrelevant citation|reason=Source covers bicarb overdose, not its mechanism of action in hyperkalemia|date=July 2025}} Since sodium bicarbonate can cause [[alkalosis]], it is sometimes used to treat aspirin overdoses. Aspirin requires an acidic environment for proper absorption, and a basic environment will diminish aspirin absorption in cases of overdose.<ref>{{cite book|title=Cloth Diapers|url=https://books.google.com/books?id=Nz4J9oSJT4IC&pg=PA46|publisher=Donald C. Cooper PhD|pages=46–}}</ref> Sodium bicarbonate has also been used in the treatment of [[tricyclic antidepressant overdose]].<ref name="pmid9142034">{{update inline|date=March 2014}}{{cite journal | vauthors = Knudsen K, Abrahamsson J | title = Epinephrine and sodium bicarbonate independently and additively increase survival in experimental amitriptyline poisoning | journal = Critical Care Medicine | volume = 25 | issue = 4 | pages = 669–74 | date = April 1997 | pmid = 9142034 | doi = 10.1097/00003246-199704000-00019 }}</ref> It can also be applied topically as a paste, with three parts baking soda to one part water, to relieve some kinds of insect bites and stings (as well as accompanying swelling).<ref>{{cite web|publisher=Mayo Clinic|url=http://www.mayoclinic.com/health/first-aid-insect-bites/fa00046|title=Insect bites and stings: First aid|date=15 January 2008}}</ref><!-- The preceding two paragraphs are copied straight from "cloth diapers" -->

Some alternative practitioners, such as [[Tullio Simoncini]], have promoted baking soda as a cancer cure, which the American Cancer Society has warned against due to both its unproven effectiveness and potential danger in use.<ref>{{cite web|url=http://www.cancer.org/treatment/treatmentsandsideeffects/complementaryandalternativemedicine/herbsvitaminsandminerals/sodium-bicarbonate |title=Sodium Bicarbonate |publisher=[[American Cancer Society]] |access-date=19 February 2013 |date=28 November 2008 |url-status=unfit |archive-url=https://web.archive.org/web/20130219044718/http://www.cancer.org/treatment/treatmentsandsideeffects/complementaryandalternativemedicine/herbsvitaminsandminerals/sodium-bicarbonate |archive-date=19 February 2013 }}</ref> [[Edzard Ernst]] has called the promotion of sodium bicarbonate as a cancer cure "one of the more sickening alternative cancer scams I have seen for a long time".<ref name=sick>{{cite web | first = Edzard | last = Ernst |title=This must be the most sickening cancer scam I have seen for a while |date=3 February 2017 |url=https://edzardernst.com/2017/02/this-must-be-the-most-sickening-cancer-scam-i-have-seen-for-a-while/ }}</ref>

Sodium bicarbonate can be added to [[local anaesthetics]], to speed up the onset of their effects and make their injection less painful.<ref>{{cite web|last1=Edgcombe|first1= H|last2= Hocking |first2= G|url=http://www.frca.co.uk/article.aspx?articleid=100505|date=6 October 2006|website=Anaesthesia UK |title= Local Anaesthetic Pharmacology|publisher=|archive-date=22 December 2015 |archive-url= https://web.archive.org/web/20151222085359/http://www.frca.co.uk/article.aspx?articleid=100505|url-status=dead}}</ref> It is also a component of [[Moffett's solution]], used in [[Nose|nasal]] surgery.<ref>{{cite journal |last1=Benjamin |first1=E. |last2=Wong |first2=D.K.K. |last3=Choa |first3=D. |date=2004 |title='Moffett's' solution: a review of the evidence and scientific basis for the topical preparation of the nose |journal=Clinical Otolaryngology and Allied Sciences |volume=29 |issue=6 |pages=582–587 |doi= 10.1111/j.1365-2273.2004.00894.x |pmid=15533141 |doi-access=free }}</ref>

It has been proposed that acidic diets weaken bones.<ref>{{cite web |url=https://www.newscientist.com/article/mg17223214-900-hard-cheese/ |title=Hard cheese |work=[[New Scientist]]|date=15 December 2001| last = Fox | first = Douglas |access-date= 20 July 2017}}</ref> One systematic meta-analysis of the research shows no such effect.<ref>{{cite journal | pmc=3114717 | year=2011 | last1=Fenton | first1=T. R. | last2=Tough | first2=S. C. | last3=Lyon | first3=A. W. | last4=Eliasziw | first4=M. | last5=Hanley | first5=D. A. | title=Causal assessment of dietary acid load and bone disease: A systematic review & meta-analysis applying Hill's epidemiologic criteria for causality | journal=Nutrition Journal | volume=10 | article-number=41 | doi=10.1186/1475-2891-10-41 |doi-access=free | pmid=21529374 }}</ref> Another also finds that there is no evidence that alkaline diets improve bone health, but suggests that there "may be some value" to alkaline diets for other reasons.<ref>{{cite journal |doi=10.1155/2012/727630 |doi-access=free|title=The Alkaline Diet: Is There Evidence That an Alkaline pH Diet Benefits Health? |year=2012 |last1=Schwalfenberg |first1=Gerry K. |journal=Journal of Environmental and Public Health |volume=2012 |pages=1–7 |pmid=22013455 |pmc=3195546 }}</ref>

[[Antacid]] (such as baking soda) solutions have been prepared and used by protesters to alleviate the effects of exposure to [[tear gas]] during protests.{{Failed verification|date=October 2017}}<ref>{{cite web|url=http://www.starhawk.org/activism/trainer-resources/teargas.html|title=Medical information from Prague 2000|url-status=dead|archive-url=https://web.archive.org/web/20141018221605/http://www.starhawk.org/activism/trainer-resources/teargas.html|archive-date=18 October 2014}}</ref>

Similarly to its use in baking, sodium bicarbonate is used together with a mild acid such as [[tartaric acid]] as the excipient in effervescent tablets: when such a tablet is dropped in a glass of water, the carbonate leaves the reaction medium as carbon dioxide gas (HCO<sub>3</sub><sup>−</sup> + H<sup>+</sup> → H<sub>2</sub>O + CO<sub>2</sub>↑ or, more precisely, HCO<sub>3</sub><sup>−</sup> + H<sub>3</sub>O<sup>+</sup> → 2&nbsp;H<sub>2</sub>O + CO<sub>2</sub>↑). This makes the tablet disintegrate, leaving the medication suspended and/or dissolved in the water together with the resulting salt (in this example, [[sodium tartrate]]).<ref>{{cite journal |last1=Shirsand |first1=S. B. |last2=Suresh |first2=Sarasija |last3=Jodhana |first3=L. S. |last4=Swamy |first4=P. V. |title=Formulation Design and Optimization of Fast Disintegrating Lorazepam Tablets by Effervescent Method |journal=Indian Journal of Pharmaceutical Sciences |date=2010 |volume=72 |issue=4 |pages=431–436 |doi=10.4103/0250-474X.73911 |pmid=21218052 |issn=0250-474X |pmc=3013557 |doi-access=free }}</ref>

====Personal hygiene====
Sodium bicarbonate is also used as an ingredient in some mouthwashes. It has anticaries and abrasive properties.<ref>{{cite web |url=https://www.duo.uio.no/bitstream/handle/10852/33076/Storehagen_Ose_Midha.pdf?sequence=1 |title=Dentifrices and mouthwashes ingredients and their use | last1 = Storehagen | first1 = Silje | last2 = Ose | first2 = Nanna | last3 = Midha | first3 = Shilpi |work=Institutt for klinisk odontologi |publisher=Universitetet i Oslo}}</ref> It works as a mechanical cleanser on the teeth and gums, neutralizes the production of acid in the mouth, and also acts as an [[antiseptic]] to help prevent infections.<ref>{{cite patent | inventor = Barth J | title = Oral Product | country= US | number = 4132770A | fdate = 1977 | gdate = 1979 }}</ref><ref>{{cite journal | vauthors = Iqbal K, Asmat M, Jawed S, Mushtaque A, Mohsin F, Hanif S, Sheikh N | display-authors = 6 | title = Role of different ingredients of tooth pastes and mouthwashes in oral health. | journal = Journal of Pakistan Dental Association | date = July 2011 | volume = 20 | issue = 3 | pages = 163–70 | url = http://applications.emro.who.int/imemrf/J_Pak_Dent_Assoc/J_Pak_Dent_Assoc_2011_20_3_163_170.pdf }}</ref> Sodium bicarbonate in combination with other ingredients can be used to make a dry or wet [[deodorant]].<ref>{{cite journal|last=Lamb|first=John Henderson |title=Sodium Bicarbonate: An Excellent Deodorant|journal=The Journal of Investigative Dermatology|date=1946|volume=7|issue=3|pages=131–133|doi=10.1038/jid.1946.13|doi-access=free}}</ref><ref>{{cite web|title=Bicarb soda: natural body deodorant|date=10 March 2009|url=http://sustainableecho.com/bicarb-soda-natural-body-deodorant/|publisher=sustainableecho.com}}</ref> Sodium bicarbonate may be used as a [[Buffer solution|buffering agent]], combined with table salt, when creating a solution for [[nasal irrigation]].<ref>{{cite book | last = Metson | first = Ralph B. | date = 2005 | title = The Harvard Medical School Guide to Healing Your Sinues | publisher = McGraw Hill | page = 68 | isbn = 9780071444699 }}</ref>

It is used in eye hygiene to treat [[blepharitis]]. This is done by adding a teaspoon of sodium bicarbonate to cool water that was recently boiled followed by gentle scrubbing of the eyelash base with a cotton swab dipped in the solution.<ref>{{cite web|url=https://www.ouh.nhs.uk/patient-guide/leaflets/files/101028blepharitis.pdf|title=Blepharitis : Information for patients leaflet|website=Ouh.nhs.uk|access-date=28 February 2022|archive-date=26 March 2023|archive-url=https://web.archive.org/web/20230326025203/https://www.ouh.nhs.uk/patient-guide/leaflets/files/101028blepharitis.pdf|url-status=dead}}</ref><ref>{{cite web|url=http://patient.info/health/blepharitis-leaflet|title=Blepharitis. Treatment and Causes. Eyelid inflammation {{!}} Patient|website=Patient|language=en-GB|access-date=31 May 2016|archive-date=5 December 2015|archive-url=https://web.archive.org/web/20151205071928/http://patient.info/health/blepharitis-leaflet|url-status=dead}}</ref>

====Veterinary uses====
Sodium bicarbonate is used as a cattle feed supplement, in particular as a [[buffering agent]] for the [[rumen]].<ref>{{cite journal | title = Use of sodium bicarbonate, offered free choice or blended into the ration, to reduce the risk of ruminal acidosis in cattle | journal = Canadian Journal of Animal Science | volume = 86 | issue = 3 | pages = 429–437 | year = 2006 | last1 = Paton | first1 = Laura J. | last2 = Beauchemin | first2 = Karen A. | last3 = Veira | first3 = Douglas M. | last4 = von Keyserlingk | first4 = Marina A. G. | doi = 10.4141/A06-014 | doi-access = free }}</ref>

===Cleaning agent===
Sodium bicarbonate is used in a process to remove paint and corrosion called [[sodablasting]]. As a blasting medium, sodium bicarbonate is used to remove surface contamination from softer and less resilient [[substrate (materials science)|substrate]]s such as aluminium, copper, or timber that could be damaged by silica sand abrasive media.<ref>{{cite web|url=https://www.popularmechanics.com/home/tools/reviews/a9280/blast-away-grime-with-baking-soda-15773126/|publisher=Popular Mechanics|title=Blast Away Grime With Baking Soda|access-date=2 August 2020|date=5 August 2013}}</ref>

A manufacturer recommends a paste made from baking soda with minimal water as a gentle scouring powder.<ref name="arm" /> Such a paste can be useful in removing surface rust because the rust forms a water-soluble compound when in a concentrated alkaline solution.<ref name="InorgChem">{{cite book | title = Inorganic Chemistry, 3rd Edition | chapter = Chapter 22: ''d''-block metal chemistry: the first row elements | last1 = Housecroft | first1 = Catherine E. | last2 = Sharpe | first2 = Alan G. | publisher = Pearson | year = 2008 | isbn = 978-0-13-175553-6 | page = 716 }}</ref> Cold water should be used since hot-water solutions can corrode steel.<ref>{{cite web|title=Science Lab.com|url=http://www.sciencelab.com/msds.php?msdsId=9927263|url-status=dead|archive-url=https://web.archive.org/web/20120905154417/http://www.sciencelab.com/msds.php?msdsId=9927263|archive-date=5 September 2012|website=MSDS- Sodium carbonate|publisher=sciencelab.com}}</ref> Sodium bicarbonate attacks the thin protective oxide layer that forms on aluminium, making it unsuitable for cleaning this metal.<ref name="PhilMus">{{cite web|url=http://www.philamuseum.org/booklets/7_44_85_1.html?page=2|title=Finishing Techniques in Metalwork|publisher=Philadelphia Museum of Art}}</ref>

A solution of baking soda in warm water will remove the [[tarnish]] from silver when the silver is in contact with a piece of [[aluminium foil]].<ref name="PhilMus" /><ref>{{cite web|title=Put a Shine on It|url=http://scifun.chem.wisc.edu/homeexpts/TARNISH.html|url-status=dead|archive-url=https://archive.today/20120731071117/http://scifun.chem.wisc.edu/homeexpts/TARNISH.html|archive-date=31 July 2012|access-date=6 March 2011|publisher=scifun.chem.wisc.edu}}</ref>

Baking soda is commonly added to washing machines as a replacement for water softener and to remove odors from clothes. When diluted with warm water, it is also almost as effective in removing heavy tea and coffee stains from cups as [[sodium hydroxide]].{{Cn|date=June 2025}}

During the [[Manhattan Project]] to develop the [[Nuclear weapon|nuclear bomb]] in the early 1940s, the [[Toxicity|chemical toxicity]] of [[uranium]] was an issue. [[Uranium oxide]]s were found to stick very well to [[cotton cloth]] and did not wash out with [[soap]] or [[laundry detergent]]. However, the uranium would wash out with a 2% solution of sodium bicarbonate. Clothing can become contaminated with toxic dust of [[depleted uranium]] (DU), which is very dense, hence it is used for counterweights in a civilian context and in armour-piercing projectiles. DU is not removed by normal laundering; washing with about {{convert|6|oz|g}} of baking soda in 2 gallons (7.5 L) of [[water]] will help wash it out.<ref name=Orcutt>{{cite web| vauthors = Orcutt JA |url=http://myweb.brooklyn.liu.edu/lawrence/duproject/duhealth.htm|work=Pharmacology and Toxicology of Uranium Compounds|publisher=McGraw-Hill|access-date=21 March 2012|title=Depleted Uranium and Health: Facts and Helpful Suggestions|url-status=dead|archive-url=https://web.archive.org/web/20130117213341/http://myweb.brooklyn.liu.edu/lawrence/duproject/duhealth.htm|archive-date=17 January 2013}}</ref>

===Odor control===
It is often claimed that baking soda is an effective odor remover<ref>{{cite news|url=http://cravedujour.com/kitchen-odor-eliminating-candles-products-tricks/#xxTICWbUEW5oLJeh.99|last=Raymond|first=Jessica|title=Kitchen Odor Eliminating Candles, Products, and Tricks|date=10 June 2016|work=cravedujour.com|access-date=29 June 2016|archive-date=7 August 2020|archive-url=https://web.archive.org/web/20200807080836/http://cravedujour.com/kitchen-odor-eliminating-candles-products-tricks/#xxTICWbUEW5oLJeh.99|url-status=usurped}}</ref>{{Better source needed|date=August 2020|comment=This is a random Wordpress blog}} and recommended that an open box be kept in the refrigerator to absorb odor.<ref>
Vicki Lansky, Martha Campbell, ''Baking Soda: Over 500 Fabulous, Fun, and Frugal Uses You've Probably Never Thought Of'', 2009, {{isbn|1931863733}}, p. 28</ref> This idea was promoted by the leading U.S. brand of baking soda, [[Arm & Hammer]], in an advertising campaign starting in 1972.<ref>"A trusted solution for more than 170 years. Pure and simple.", Arm & Hammer [https://www.armandhammer.com/en-ca/about-us "About Us"] page</ref> Though this campaign is considered a classic of marketing, leading within a year to more than half of American refrigerators containing a box of baking soda,<ref>Keith Sawyer, ''Group Genius: The Creative Power of Collaboration'', 2017, {{isbn|0465093582}}, [https://books.google.com/books?id=v42PDQAAQBAJ&dq=%22baking+soda%22+marketing+1972+hammer&pg=PT114 "keep food tasting fresh"]</ref><ref>Clayton M. Christensen, Scott Cook, Taddy Hall, ''Marketing Malpractice: The Cause and the Cure'', ''[[Harvard Business Review]]'', December 2005, [https://hbr.org/2005/12/marketing-malpractice-the-cause-and-the-cure]</ref> there is little evidence that it is effective in this application.<ref>"Myth #100: An Open Box of Baking Soda in the Fridge absorbs Odors", Bruce Weinstein, Mark Scarbrough, ''Lobsters Scream When You Boil Them; And 100 Other Myths About Food and Cooking'', 2011, {{isbn|1439195382}}, p. 312</ref><ref>{{cite web|url=http://www.cooksillustrated.com/how_tos/5510-baking-soda-as-odor-absorber|title=Baking Soda as Odor Absorber &#124; Cook's Illustrated|website=Cooksillustrated.com|access-date=28 February 2022}}</ref> However, baking soda may be effective in absorbing musty smells in books.<ref>{{cite journal|title=Book Repair for BookThinkers: How To Remove Odors From Books| last = Altman | first = Gail |date=22 May 2006|issue=69|journal=The BookThinker|url=http://www.bookthink.com/0069/69alt.htm}}</ref>

=== Education ===
An educational science experiment known as the "Baking Soda and Vinegar Volcano" uses the acid-base reaction with [[vinegar]] acid to mimic a volcanic eruption. The rapid production of CO<sub>2</sub> causes the liquid to foam up and overflow its container. Other ingredients such as dish soap and food coloring can be added to enhance the visual effect.<ref>{{Cite web |title=7 Baking Soda & Vinegar STEM Activities & Experiments {{!}} ARM & HAMMER |url=https://www.armandhammer.com/en/articles/fun-and-easy-stem-activities-with-baking-soda-and-vinegar#soda_volcano |access-date=2024-11-27 |website=www.armandhammer.com |language=en}}</ref> If this reaction is performed inside of a closed vessel (such as a bottle) with no way for gas to escape, it can cause an [[explosion]] if the pressure is high enough.

==Chemistry==
[[File:Hydrogenuhličitan sodný.jpg|thumb|Sodium bicarbonate]]
Sodium bicarbonate is an [[amphoteric]] compound.<ref name=":3" /> Aqueous solutions are mildly [[alkaline]] due to the formation of [[carbonic acid]] and [[hydroxide]] ion:<ref name=":3" />

:HCO{{su| b=3 |p=−}} + H<sub>2</sub>O → {{chem|H|2|CO|3}} + OH<sup>−</sup>

Sodium bicarbonate can sometimes be used as a mild [[Neutralization (chemistry)|neutralization]] agent and a safer alternative to strong bases like [[sodium hydroxide]].<ref name=":2">{{Cite journal |last1=Papuga |first1=Aleksandra |last2=Polańczyk |first2=Andrzej |date=2023-12-06 |title=Analysis of the latest guidelines for the neutralization of selected acids, including recommendations for emergency responders |url=https://zeszytynaukowe-sgsp.pl/gicid/01.3001.0054.1220 |journal=Zeszyty Naukowe SGSP |volume=1 |issue=88 |pages=75–95 |doi=10.5604/01.3001.0054.1220 |issn=0239-5223|doi-access=free }}</ref> Reaction of sodium bicarbonate and an [[acid]] produces a salt and carbonic acid, which readily decomposes to carbon dioxide and water:<ref name=":2" />

:NaHCO<sub>3</sub> + HCl → NaCl + H<sub>2</sub>O + CO<sub>2</sub>
:H<sub>2</sub>CO<sub>3</sub> → H<sub>2</sub>O + CO<sub>2</sub>(g)

Sodium bicarbonate reacts with [[acetic acid]] (found in vinegar), producing [[sodium acetate]], water, and [[carbon dioxide]]:

:NaHCO<sub>3</sub> + CH<sub>3</sub>COOH → CH<sub>3</sub>COONa + H<sub>2</sub>O + CO<sub>2</sub>(g)

Sodium bicarbonate reacts with [[base (chemistry)|bases]] such as [[sodium hydroxide]] to form carbonates:

:NaHCO<sub>3</sub> + NaOH → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O

===Thermal decomposition===
At temperatures from {{convert|80|–|100|C|F}}, sodium bicarbonate gradually decomposes into [[sodium carbonate]], water, and carbon dioxide. The conversion is faster at {{convert|200|°C}}:<ref name=frostburg>{{cite web|publisher=General Chemistry Online|title=Decomposition of Carbonates|url=http://antoine.frostburg.edu/chem/senese/101/inorganic/faq/carbonate-decomposition.shtml|access-date=16 March 2010|archive-url=https://web.archive.org/web/19991002045519/http://antoine.frostburg.edu/chem/senese/101/inorganic/faq/carbonate-decomposition.shtml|archive-date=2 October 1999|url-status=dead}}</ref>

: 2 NaHCO<sub>3</sub> → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O + CO<sub>2</sub>

Most bicarbonates undergo this [[dehydration reaction]]. Further heating converts the carbonate into the [[sodium oxide|oxide]] (above {{convert|850|°C|°F|disp=x|/}}):<ref name=frostburg />

: Na<sub>2</sub>CO<sub>3</sub> → Na<sub>2</sub>O + CO<sub>2</sub>

The generation of carbon dioxide and water partially explain the fire-extinguishing properties of NaHCO<sub>3</sub>,<ref name=":0" /> although other factors like [[Endothermic process|heat absorption]] and radical [[Scavenger (chemistry)|scavenging]] are more significant.<ref name=":1" />

== Natural occurrence ==
In nature, sodium bicarbonate occurs almost exclusively as either [[nahcolite]] or [[trona]]. Trona is more common, as nahcolite is more soluble in water and the [[chemical equilibrium]] between the two minerals favors trona.<ref name=":4" /> Significant nahcolite deposits are in the United States, Botswana and Kenya, Uganda, Turkey, and Mexico.<ref>{{Cite web |date=2012 |title=Nahcolite |url=https://www.britannica.com/science/nahcolite |access-date=2024-06-02 |website=[[Encyclopedia Britannica]] |language=en}}</ref> The biggest trona deposits are in the [[Green River (Colorado River tributary)|Green River]] basin in Wyoming.<ref>{{Cite book |last=Bolen |first=Wallace P. |url=https://pubs.usgs.gov/periodicals/mcs2024/mcs2024-soda-ash.pdf |title=Soda ash |date=January 2024 |publisher=[[U.S. Geological Survey]] |archive-url=https://web.archive.org/web/20240304184031/https://pubs.usgs.gov/periodicals/mcs2024/mcs2024-soda-ash.pdf |archive-date=2024-03-04}}</ref>

Nahcolite is sometimes found as a component of [[oil shale]].<ref name=":5">{{Cite book |last1=Johnson |first1=Ronald C. |title=An Assessment of In-Place Oil Shale Resources in the Green River Formation, Piceance Basin, Colorado |last2=Mercier |first2=Tracey J. |last3=Brownfield |first3=Michael E. |last4=Pantea |first4=Michael P. |last5=Self |publisher=[[U.S. Geological Survey]] |year=2020}}</ref>

==Stability and shelf life==
If kept cool ([[room temperature]]) and dry (an airtight container is recommended to keep out moist air), sodium bicarbonate can be kept without a significant amount of decomposition for at least two or three years.<ref>{{cite web|last=PubChem|title=Sodium bicarbonate|url=https://pubchem.ncbi.nlm.nih.gov/compound/516892|access-date=2021-05-16|website=pubchem.ncbi.nlm.nih.gov|language=en}}</ref><ref>{{cite web|date=31 January 2019|title=Sodium bicarbonate (S300) batch numbering and shelf life statement – Solvay Chemicals, Inc.|url=https://www.solvay.com/sites/g/files/srpend221/files/2019-06/SOLVAIR®%20S300%20BICAR%20Batch%20Numbering%20and%20Shelf%20Life%20Statement%20-%20Green%20River%20-%20US.pdf}}</ref><ref>{{cite web|date=1 April 2015|title=Re: Shelf Life – Sodium Bicarbonate (all grades) – Tronox Alkali Corporation|url=https://alkali.genesisenergy.com/wp-content/uploads/sites/24/2015/05/Shelf-Life-Sodium-Bicarbonate-1.pdf}}</ref><ref>{{cite web|title=Does Baking Soda Go Bad? How to Know If It's Still Good|url=https://www.thespruceeats.com/how-to-tell-if-baking-soda-is-still-good-1388327|access-date=2021-05-16|website=The Spruce Eats|language=en}}</ref>

==History==
The word ''natron'' has been in use in many languages throughout [[Modern history|modern times]] (in the forms of ''anatron'', ''natrum'' and ''natron'') and originated (like [[Spanish language|Spanish]], [[French language|French]] and [[English language|English]] ''natron'' as well as '[[sodium]]') via Arabic ''naṭrūn'' (or ''anatrūn''; cf. the Lower Egyptian "Natrontal" [[Wadi El Natrun]], where a mixture of [[sodium carbonate]] and sodium hydrogen carbonate for the dehydration of [[Mummy|mummies]] was used<ref>Renate Gerner: ''Instruments and substances used in mummification.'' In: Renate Gerner, Rosemarie Drenkhahn (ed.): ''Mumie und Computer. A multidisciplinary research project in Hanover. Special exhibition of the Kestner Museum Hanover from September 26, 1991 to January 19, 1992.'' Kestner Museum, Hanover 1991, {{ISBN|3-924029-17-2}}, p. 28 f.</ref>) from Greek ''nítron (νίτρον)'' (Herodotus; Attic ''lítron (λίτρον)''), which can be traced back to ancient Egyptian ''ntr''. The Greek ''nítron'' (soda, saltpeter) was also used in Latin ''(sal) nitrum'' and in German ''Salniter'' (the source of ''Nitrogen'', ''Nitrat'' etc.).<ref>Franz Dornseiff: "The Greek words in German." Walter de Gruyter & Co, Berlin 1950, p. 44.</ref><ref>[[Friedrich Kluge]], Alfred Götze (Philologist): ''[[Etymological Dictionary of the German Language]]. '' 20th edition, ed. by Walther Mitzka, De Gruyter, Berlin / New York 1967; Reprint (“21st unchanged edition”) ibid 1975, {{ISBN|3-11-005709-3}}, p. 504.</ref> The word ''saleratus'', from [[Latin language|Latin]] ''sal æratus'' (meaning "aerated salt"), was widely used in the 19th century for both sodium bicarbonate and [[potassium bicarbonate]].<ref>{{cite web |title=Definition of SALERATUS |url=https://www.merriam-webster.com/dictionary/saleratus |access-date=6 December 2020 |website=www.merriam-webster.com |language=en}}</ref>

In 1791, French chemist [[Nicolas Leblanc]] produced sodium carbonate (also known as soda ash). Pharmacist [[Valentin Rose (pharmacologist)|Valentin Rose the Younger]] is credited with the discovery of sodium bicarbonate in 1801 in Berlin. In 1846, two American bakers, [[John Dwight (manufacturer)|John Dwight]] and [[Austin Church]], established the first factory in the United States to produce baking soda from sodium carbonate and [[carbon dioxide]].<ref>{{cite web|publisher=Church & Dwight Co.|title=Company History|url=http://www.churchdwight.com/Company/corp_history.asp|archive-url=https://web.archive.org/web/20111016003546/http://www.churchdwight.com/Company/corp_history.asp|archive-date=16 October 2011|url-status=dead}}</ref>

''Saleratus'', potassium or sodium bicarbonate, is mentioned in the novel ''[[Captains Courageous]]'' by [[Rudyard Kipling]] as being used extensively in the 1800s in commercial fishing to prevent freshly caught fish from spoiling.<ref>{{cite book| last = Kipling | first = Rudyard |title=[[Captains Courageous]]| page= 25|year=1897}}</ref>

In 1919, [[Lee Slater Overman|US Senator Lee Overman]] declared that bicarbonate of soda could cure the [[Spanish flu]]. In the midst of the debate on 26 January 1919, he interrupted the discussion to announce the discovery of a cure. "I want to say, for the benefit of those who are making this investigation," he reported, "that I was told by a judge of a superior court in the mountain country of North Carolina they have discovered a remedy for this disease." The purported cure implied a critique of modern science and an appreciation for the simple wisdom of simple people. "They say that common baking soda will cure the disease," he continued, "that they have cured it with it, that they have no deaths up there at all; they use common baking soda, which cures the disease."<ref>{{citation|last=Bristow|first=Nancy K.|title=American Pandemic: The Lost Worlds of the 1918 Influenza Epidemic|publisher=Oxford University Press|date=2012|page=178|isbn=978-0199811342}}</ref>

==Production==
Sodium bicarbonate is produced industrially from [[sodium carbonate]]:<ref name=Ullmann>{{cite encyclopedia|chapter=Sodium Carbonates| first = Christian | last = Thieme |encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|publisher=Wiley-VCH|location=Weinheim|year=2000|doi=10.1002/14356007.a24_299| isbn = 3527306730 }}</ref>
:Na<sub>2</sub>CO<sub>3</sub> +  CO<sub>2</sub>  +  H<sub>2</sub>O  →  2 NaHCO<sub>3</sub>
It is produced on the scale of about 100,000 tonnes/year (as of 2001) {{Dubious|Production figure|date=November 2020}}<ref>{{cite book | vauthors = Holleman AF, Wiberg E | date = 2001 | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | isbn = 0-12-352651-5 }}</ref> with a worldwide production capacity of 2.4&nbsp;million tonnes per year (as of 2002).<ref name="ESAPA">Page 45, section 3.6.2.1 of [https://web.archive.org/web/20080407001754/http://www.cefic.be/files/Publications/ESAPA_Soda_Ash_Process_BREF3.pdf "Process Best Practices Reference Document (BREF) for Soda Ash,"] report produced by the [http://www.cefic.be/templates/shwAssocDetails.asp?NID=473&HID=27&ID=60 European Soda Ash Producer's Association] {{Webarchive|url=https://web.archive.org/web/20061003115649/http://www.cefic.be/templates/shwAssocDetails.asp?NID=473&HID=27&ID=60 |date=3 October 2006 }}, March 2004.</ref> Commercial quantities of baking soda are also produced by a similar method: soda ash, mined in the form of the ore [[trona]], is dissolved in water and treated with carbon dioxide. Sodium bicarbonate precipitates as a solid from this solution.{{citation needed|date=March 2020}}

Regarding the [[Solvay process]], sodium bicarbonate is an intermediate in the reaction of [[sodium chloride]], [[ammonia]], and [[carbon dioxide]]. The product however shows low purity (75pc).{{citation needed|date=March 2020}}

: [[sodium chloride|NaCl]] + [[carbon dioxide|CO<sub>2</sub>]] + [[ammonia|NH<sub>3</sub>]] + [[water|H<sub>2</sub>O]] → NaHCO<sub>3</sub> + [[ammonium chloride|NH<sub>4</sub>Cl]]

Although of no practical value, NaHCO<sub>3</sub> may be obtained by the reaction of carbon dioxide with an [[aqueous solution]] of sodium hydroxide:{{citation needed|date=March 2020}}
:CO<sub>2</sub> + NaOH → NaHCO<sub>3</sub>

===Mining===
Naturally occurring deposits of [[nahcolite]] (NaHCO<sub>3</sub>) are found in the [[Eocene]]-age (55.8–33.9 Mya) [[Green River Formation]], [[Piceance Basin]] in [[Colorado]]. Nahcolite was deposited as beds during periods of high evaporation in the basin. It is commercially mined using common underground mining techniques such as bore, drum, and longwall mining in a fashion very similar to coal mining.{{citation needed|date=March 2020}}

It is also produced by solution mining, pumping heated water through nahcolite beds and crystallizing the dissolved nahcolite through a cooling crystallization process.

Since nahcolite is sometimes found in [[shale]], it can be produced as a co-product of [[shale oil extraction]], where it is recovered by solution mining.<ref name=":5" />

==In popular culture==

Sodium bicarbonate, as "bicarbonate of soda", was a frequent source of punch lines for [[Groucho Marx]] in [[Marx Brothers]] movies. In ''[[Duck Soup (1933 film)|Duck Soup]]'', Marx plays the leader of a nation at war. In one scene, he receives a message from the battlefield that his general is reporting a gas attack, and Groucho tells his aide: "Tell him to take a teaspoonful of bicarbonate of soda and a half a glass of water."<ref>{{cite web|url=https://www.imdb.com/title/tt0023969/trivia?tab=qt|title=Duck Soup (1933)|work=IMDb|access-date=4 August 2015}}</ref> In ''[[A Night at the Opera (film)|A Night at the Opera]]'', Groucho's character addresses the opening night crowd at an opera by saying of the lead tenor: "Signor Lassparri comes from a very famous family. His mother was a well-known bass singer. His father was the first man to stuff spaghetti with bicarbonate of soda, thus causing and curing indigestion at the same time."<ref>{{cite web|url=https://www.imdb.com/title/tt0026778/trivia?tab=qt&ref_=tt_trv_qu|title=A Night at the Opera (1935)|work=IMDb|access-date=4 August 2015}}</ref>

In the Joseph L. Mankewicz classic ''[[All About Eve]]'', the Max Fabian character ([[Gregory Ratoff]]) has an extended scene with Margo Channing ([[Bette Davis]]) in which, suffering from heartburn, he requests and then drinks bicarbonate of soda, eliciting a prominent burp. Channing promises to always keep a box of bicarb with Max's name on it.

== See also ==
{{div col|colwidth=30em}}
* [[Carbonic acid]]
* [[List of ineffective cancer treatments]]
* [[List of minerals]]
* [[Natron]]
* [[Potassium bicarbonate]]
* [[Trona]]
{{div col end}}

== References ==
{{reflist}}

==Bibliography==
{{refbegin}}
* {{cite book | editor-last = Haynes | editor-first = William M. | year = 2011 | title = CRC Handbook of Chemistry and Physics | edition = 92nd | publisher = [[CRC Press]] | isbn = 978-1439855119| title-link = CRC Handbook of Chemistry and Physics }}
{{refend}}

== External links ==
{{Commons category|Sodium bicarbonate}}
* [http://www.inchem.org/documents/icsc/icsc/eics1044.htm International Chemical Safety Card 1044]

{{Sodium compounds}}
{{hydrogen compounds}}
{{Carbonates}}
{{Antacids}}
{{Emergency medicine}}
{{Authority control}}

[[Category:Acid salts]]
[[Category:Antacids]]
[[Category:Bases (chemistry)]]
[[Category:Bicarbonates]]
[[Category:Chemical substances for emergency medicine]]
[[Category:Fire suppression agents]]
[[Category:Household chemicals]]
[[Category:Leavening agents]]
[[Category:Sodium compounds]]
[[Category:E-number additives]]
[[Category:Powders]]
[[Category:Food powders]]