Old page wikitext, before the edit (old_wikitext ) | '{{chembox
| Watchedfields = changed
| verifiedrevid = 311801095
| Name = Sodium Bicarbonate
| ImageFile = SodiumBicarbonate.svg
| ImageSize = 150px
| ImageFileL1 = Sodium-3D.png
| ImageSizeL1 = 80px
| ImageFileR1 = Bicarbonate-ion-3D-balls-B.png
| ImageSizeR1 = 120px
| ImageFile2 = Sodium bicarbonate.jpg
| IUPACName = Sodium hydrogen carbonate
| OtherNames = Sodium bicarbonate<br/>Bicarbonate of soda<br/>Baking soda<br/>Sodium hydrogencarbonate<br/>[[Nahcolite]]
| Section1 = {{Chembox Identifiers
| CASNo = 144-55-8
| CASNo_Ref = {{cascite}}
| PubChem = 516892
| ChemSpiderID = 8609
| RTECS = VZ0950000
}}
| Section2 = {{Chembox Properties
| Na=1|H=1|C=1|O=3
| Appearance = white crystalline solid
| Odor = odorless
| Density = 2.173 g/cm<sup>3</sup>
| Solubility = 7.8 g/100 mL (18 °C) <br /> 10 g/100 mL (20 °C)
| SolubleOther = insoluble in [[alcohol]], [[ether]]
| MeltingPt = decomp: 323.15 K (50 °C) - 543.15 K (270 °C)
| RefractIndex = 1.3344
| pKa = 10.3
}}
| Section7 = {{Chembox Hazards
| ExternalMSDS = [http://siri.org/msds/f2/bdm/bdmjw.html External MSDS]
| EUIndex = Not listed
| MainHazards =
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
| FlashPt = Non-flammable
| RPhrases =
| SPhrases =
| LD50 = 4220 mg/kg
}}
| Section8 = {{Chembox Related
| OtherAnions = [[Sodium carbonate]]
| OtherCations = [[Potassium bicarbonate]]<br/>[[Ammonium bicarbonate]]
| OtherCpds = [[Sodium bisulfate]]<br/>[[Sodium hydrogen phosphate]]
}}
}}
'''Sodium bicarbonate''' or '''sodium hydrogen carbonate''' is the [[chemical compound]] with the formula NaHCO<sub>3</sub>. 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 washing soda ([[sodium carbonate]]). It is a component of the mineral [[natron]] and is found dissolved in many [[mineral spring]]s. The natural mineral form is known as '''[[nahcolite]]'''. It is found in its dissolved form in [[bile]], where it serves to neutralize the acidity of the [[hydrochloric acid]] produced by the stomach, and is excreted into the duodenum of the small intestine via the bile duct. It is also produced artificially.
Since it has long been known and is widely used, the [[Salt (chemistry)|salt]] has many related names such as '''baking soda''', '''bread soda''', '''cooking soda''', '''bicarbonate of soda'''. Colloquially, its name is shortened to '''''sodium bicarb''''', '''''bicarb soda''''', or simply '''''bicarb'''''. 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]]. The term has now fallen out of common usage.
==History==
The [[ancient Egyptians]] used natural deposits of [[natron]], a mixture consisting mostly of [[sodium carbonate]] decahydrate and sodium bicarbonate. The natron was used as a cleansing agent like [[soap]].
In 1791, a French chemist, [[Nicolas Leblanc]], produced [[sodium carbonate]], also known as [[soda ash]]. In 1846 two New York bakers, John Dwight and Austin Church, established the first factory to develop 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}}
</ref>
==Production==
{{Main|Solvay process}}
NaHCO<sub>3</sub> is mainly prepared by the [[Solvay process]], which is the reaction of [[calcium carbonate]], [[sodium chloride]], [[ammonia]], and [[carbon dioxide]] in water. It is produced on the scale of about 100,000 ton/year (as of 2001).<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref>
NaHCO<sub>3</sub> may be obtained by the reaction of [[carbon dioxide]] with an aqueous solution of [[sodium hydroxide]]. The initial reaction produces [[sodium carbonate]]:
:CO<sub>2</sub> + 2 NaOH → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O
Further addition of [[carbon dioxide]] produces sodium bicarbonate, which at sufficiently high concentration will precipitate out of solution:
:Na<sub>2</sub>CO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O → 2 NaHCO<sub>3</sub>
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 method:
: Na<sub>2</sub>CO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O → 2 NaHCO<sub>3</sub>
==Mining==
Naturally occurring deposits of nahcolite (NaHCO<sub>3</sub>) are found in the [[Eocene]]-age (55.8 ± 0.2 - 33.9 ± 0.1 Ma) [[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 in-situ leach techniques involving dissolution of the nahcolite by heated water which is pumped through the nahcolite beds and reconstituted through a natural cooling crystallization process.
==Chemistry==
Sodium bicarbonate is an [[amphoteric]] compound. Aqueous solutions are mildly [[alkaline]] due to the formation of [[carbonic acid]] and [[hydroxide]] ion:
:HCO{{su|b=3|p=−}} + H<sub>2</sub>O → {{chem|H|2|CO|3}} + OH<sup>−</sup>
Sodium bicarbonate can be used as a wash to remove any acidic impurities from a "crude" liquid, producing a purer sample. Reaction of sodium bicarbonate and an [[acid]] to give a salt and carbonic acid, which readily decomposes to carbon dioxide and water:
:NaHCO<sub>3</sub> + HCl → NaCl + H<sub>2</sub>CO<sub>3</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]]) and presents a simple and showy demonstration of a [[chemical reaction]]. The products of the ensuing two-stage reaction are [[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)|base]]s such as [[sodium hydroxide]] to form [[carbonate]]s:
:NaHCO<sub>3</sub> + NaOH → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O
Sodium bicarbonate reacts with [[carboxyl group]]s in proteins to give a brisk effervescence from the formation of {{chem|CO|2}}. This reaction is used to test for the presence of carboxylic groups in protein.
===Thermal decomposition===
Above 70 °C, sodium bicarbonate gradually decomposes into [[sodium carbonate]], [[water]] and [[carbon dioxide]]. The conversion is fast at 200 °C:<ref> {{cite web | publisher = General Chemistry Online | title = Decomposition of Carbonates | url = http://antoine.frostburg.edu/chem/senese/101/inorganic/faq/carbonate-decomposition.shtml}} </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]] (at around 1000 °C):
: Na<sub>2</sub>CO<sub>3</sub> → Na<sub>2</sub>O + CO<sub>2</sub>
These conversions are relevant to the use of NaHCO<sub>3</sub> as a fire-suppression agent ("BC powder") in some dry powder [[fire extinguisher]]s.
==Applications==
===Cooking===
{{Main|Leavening agent}}
Sodium bicarbonate is primarily used in [[cooking]] ([[baking]]) where it reacts with other components to release carbon dioxide, that helps [[dough]] rise. The acidic compounds that induce this reaction include [[phosphates]], [[cream of tartar]], [[Lemon|lemon juice]], [[yogurt]], [[buttermilk]], [[Cocoa solids|cocoa]], [[vinegar]], etc. Sodium bicarbonate can be substituted for [[baking powder]] provided sufficient acid reagent is also added to the recipe.<ref>Radiation Cookery Book 45<sup>th</sup> Edition, Radiation Group Sales Ltd 1954</ref> Many forms of baking powder contain sodium bicarbonate combined with one or more acidic phosphates (especially good) or cream of tartar. It can also be used for softening peas (⅛ tsp. per pint of water and bring to boil for one hour)
Thermal decomposition causes sodium bicarbonate alone to act as a raising agent by releasing carbon dioxide at baking temperatures. The mixture for cakes using this method can be allowed to stand before baking without any premature release of carbon dioxide.
===Neutralization of acids and bases===
Many laboratories keep a bottle of sodium bicarbonate powder within easy reach, because sodium bicarbonate is [[amphoterism|amphoteric]], reacting with [[PH|acids and bases]]. Furthermore, as it is relatively innocuous in most situations, there is no harm in using excess sodium bicarbonate. Lastly, sodium bicarbonate powder may be used to smother a small fire.<ref name="arm"/>
A wide variety of applications follows from its neutralization properties, including reducing the spread of [[white phosphorus]] from incendiary bullets inside an afflicted soldier's wounds.<ref>{{cite web | publisher = GlobalSecurity.org | title = White Phosphorus | url = http://www.globalsecurity.org/military/systems/munitions/wp.htm | accessdate = 2007-09-26}}</ref> Sodium bicarbonate can be added as a simple solution for raising the pH balance of water (increasing total alkalinity) where high levels of chlorine (2-5 ppm) are present as in swimming pools and aquariums.<ref>{{cite web | publisher = Arm & Hammer Baking Soda | title = Outdoor Fun: Pool Care | url = http://www.armhammer.com/myfamily/tips/outdoors.asp | date = 2003 | accessdate = 2007-09-26}}</ref>
===Medical uses===
Sodium bicarbonate is used in an [[aqueous solution]] as an [[antacid]] taken orally to treat [[acid indigestion]] and [[heartburn]].<ref>{{cite web | publisher = Jackson Siegelbaum Gastroenterology | url = http://www.gicare.com/pated/sodium_bicarbonate.htm | title = Sodium Bicarbonate | date = 1998}}</ref> It may also be used in an oral form to treat chronic forms of metabolic acidosis such as [[chronic renal failure]] and [[renal tubular acidosis]]. Sodium bicarbonate may also be useful in urinary alkalinization for the treatment of [[aspirin overdose]] and [[uric acid]] renal stones.
An aqueous solution is sometimes administered [[intravenous]]ly for cases of [[acidosis]], or when there are insufficient sodium or bicarbonate ions 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 = 2004-07-13}}</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. It is for this reason that sodium bicarbonate is used in medically supervised [[cardiopulmonary resuscitation]]. Infusion of bicarbonate is indicated only when the blood pH is marked (<7.1-7.0) low.<ref>{{Cite web |publisher=emedicine |url=http://emedicine.medscape.com/article/301574-treatment |title=Respiratory Acidosis: Treatment & Medication}}</ref>
It is used as well for treatment of [[hyperkalemia]]. Since sodium bicarbonate can cause [[alkalosis]], it is sometimes used to treat aspirin overdoses. Aspirin requires an acidic environment for proper absorption, and the basic environment diminishes aspirin absorption in the case of an overdose. Sodium bicarbonate has also been used in the treatment of [[tricyclic antidepressant overdose]].<ref name="pmid9142034">{{cite journal |pmid=9142034 |year=1997 |month=Apr |author=Knudsen, K; Abrahamsson, J |title=Epinephrine and sodium bicarbonate independently and additively increase survival in experimental amitriptyline poisoning |volume=25 |issue=4 |pages=669–74 |issn=0090-3493 |journal=Critical care medicine |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 insect bites.<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 = 2008-01-15}}</ref>
Adverse reactions to the administration of sodium bicarbonate can include [[metabolic alkalosis]], [[edema]] due to sodium overload, [[congestive heart failure]], [[hyperosmolar syndrome]], hypervolemic [[hypernatremia]], and [[hypertension]] due to increased sodium. In patients who consume a high calcium or dairy-rich diet, [[calcium supplements]], or calcium-containing antacids such as [[calcium carbonate]] (e.g., Tums), the use of sodium bicarbonate can cause [[milk-alkali syndrome]], which can result in [[metastatic calcification]], [[kidney stones]], and [[kidney failure]].
Sodium bicarbonate is also used as an ingredient in some mouthwashes. It works as a mechanical cleanser on the teeth and gums, neutralizes the production of acid in the mouth and also as an [[antiseptic]] to help prevent infections occurring.
Sodium bicarbonate can be used to cover an allergic reaction of poison ivy, oak, or sumac to relieve some of the itching that is associated with it (an alternative to buying hydrocortisone cream).<ref>http://www.virtuowl.com/bicarb-lab/WhatisSodiumBicarbonateUsedFor.html</ref>
Sodium bicarbonate can be used as an exfoliant. Its particles are rounded and fine in texture, making it both effective and gentle on the skin. Using baking soda as an exfoliating scrub will remove dead skin cells, which can be discolored from hyperpigmentation and scarring.
===Personal hygiene===
A paste made from sodium bicarbonate and a 3% [[hydrogen peroxide]] solution can be used as an alternative to commercial non-fluoride [[toothpaste]]s, and sodium bicarbonate in combination with other ingredients can be used to make a dry or wet [[deodorant]]. Sodium bicarbonate is a common ingredient in alternative and natural brands of toothpaste and deodorant. It may also be used as a shampoo.<ref name = "Bouchard"> Four Green Steps, Mallory Bouchard (2010). http://www.fourgreensteps.com/infozone/featured-zone/a-green-and-healthy-beauty-secret-going-shampoo-free </ref>
===Soda loading===
Small amounts of sodium bicarbonate have been shown to be useful as a supplement for endurance athletes,<ref>{{cite news| url=http://women.timesonline.co.uk/tol/life_and_style/women/body_and_soul/article4539000.ece | work=The Times | location=London | title=Is bicarbonate of soda a performanceenhancing drug | first=Peta | last=Bee | date=2008-08-16 | accessdate=2010-05-23}}</ref> but overdose is a serious risk.<ref>http://www.umm.edu/ency/article/002749all.htm</ref>
===As a cleaning agent===
A paste from baking soda can be very effective when used in cleaning and scrubbing.<ref>{{cite web|url=http://www.armhammer.com/basics/magic/#3 |title=Arm & Hammer Baking Soda - Basics - The Magic Of Arm & Hammer Baking Soda |publisher=Armhammer.com |date= |accessdate=2009-07-30}}</ref> For cleaning aluminium objects, the use of sodium bicarbonate is discouraged as it attacks the thin unreactive protective oxide layer of this otherwise very reactive metal. A solution in warm water will remove the [[tarnish]] from [[silver]] when the silver is in contact with a piece of [[aluminium foil]].<ref>[http://www.instructables.com/id/EWU42JVP9EEV2ZBWZL/ instructables.com]</ref>
Baking soda is commonly added to the rinse cycles of washing machines (together with the detergent) as a replacement for softener and also to remove odors. Sodium bicarbonate is also effective in removing heavy tea and coffee stains from cups when diluted with warm water.
===Cattle feed supplement===
Sodium bicarbonate is sold as a [[cattle]] feed supplement, in particular as a [[buffering agent]] for the [[rumen]].
===Miscellaneous===
Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire.<ref name=arm>{{cite web|url=http://www.armhammer.com/basics/magic/#9 |title=Arm & Hammer Baking Soda - Basics - The Magic Of Arm & Hammer Baking Soda |publisher=Armhammer.com |date= |accessdate=2009-07-30}}</ref> However, it should not be applied to fires in [[deep fryer]]s as it 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 [[ammonium phosphate]] in ABC extinguishers. The alkali 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. Because it can act as an alkali, the agent has a mild [[saponification]] effect on hot grease, which forms a smothering soapy foam. Dry chemicals have since fallen out of favor for kitchen fires as they have no cooling effect compared to the extremely effective wet chemical agents specifically designed for such hazards.{{Citation needed|date=September 2007}}
Sodium bicarbonate is used in a process for cleaning paint called [[sodablasting]]. It can be administered to pools, spas, and garden ponds to raise [[pH]] levels.<ref>{{cite web|url=http://www.armhammer.com/basics/magic/#8 |title=Arm & Hammer Baking Soda - Basics - The Magic Of Arm & Hammer Baking Soda |publisher=Armhammer.com |date= |accessdate=2009-07-30}}</ref> It has [[disinfectant]] and [[antiseptic]] properties,<ref>{{cite journal |pmid=16540196 |year=2006 |month=May |author=Malik, Ys; Goyal, Sm |title=Virucidal efficacy of sodium bicarbonate on a food contact surface against feline calicivirus, a norovirus surrogate |volume=109 |issue=1-2 |pages=160–3 |issn=0168-1605 |doi=10.1016/j.ijfoodmicro.2005.08.033 |journal=International journal of food microbiology}}</ref> and it may be an effective [[fungicide]] against some organisms.<ref>{{cite journal |pmid=18396809 |year=2007 |month= |author=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 |volume=72 |issue=4 |pages=773–7 |issn=1379-1176 |journal=Communications in agricultural and applied biological sciences |url=http://toxnet.nlm.nih.gov/cgi-bin/sis/search/r?dbs+hsdb:@term+@rn+7440-09-7 |format=Free full text}}</ref>
Because it can be used to absorb odors, it is a tried-and-true method of used booksellers. The baking soda will absorb the musty smell, leaving the books less odorous.<ref>{{cite journal |title=Book Repair for BookThinkers: How To Remove Odors From Books |author=Gail Altman |date=2006-05-22 |issue=69 |work=The BookThinker |url=http://www.bookthink.com/0069/69alt.htm}}</ref>
== See also ==
* [[Carbonic acid]]
* [[Baking powder]]
* [[List of minerals]]
* [[Nahcolite]]
* [[Natron]]
* [[Natrona]] (disambiguation)
* [[Trona]]
==References==
{{reflist|2}}
==Further reading==
*{{cite journal |pmid=15126714 |year=2004 |month=May |author=Bishop, D; Edge, J; Davis, C; Goodman, C |title=Induced metabolic alkalosis affects muscle metabolism and repeated-sprint ability. |volume=36 |issue=5 |pages=807–13 |issn=0195-9131 |journal=Medicine and science in sports and exercise}}
==External links==
{{Commons category|Sodium bicarbonate}}
{{Cookbook|Baking soda}}
*[http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc10/icsc1044.htm International Chemical Safety Card 1044]
*[http://chemistry.about.com/cs/foodchemistry/f/blbaking.htm/ Differences between Baking Soda and Baking Powder]
{{Sodium compounds}}
{{Antacids}}
{{DEFAULTSORT:Sodium Bicarbonate}}
[[Category:Sodium compounds]]
[[Category:Bases]]
[[Category:Antacids]]
[[Category:Bicarbonates]]
[[Category:Acid salts]]
[[Category:Fire suppression agents]]
[[Category:Household chemicals]]
[[Category:Leavening agents]]
[[ar:بيكربونات الصوديوم]]
[[bs:Natrijum hidrogen karbonat]]
[[bg:Натриев бикарбонат]]
[[ca:Bicarbonat de sodi]]
[[cs:Hydrogenuhličitan sodný]]
[[da:Natron]]
[[de:Natriumhydrogencarbonat]]
[[et:Naatriumvesinikkarbonaat]]
[[es:Bicarbonato de sodio]]
[[fa:جوش شیرین]]
[[fr:Bicarbonate de sodium]]
[[ko:탄산 수소 나트륨]]
[[hi:सोडियम बाईकार्बोनेट]]
[[hr:Natrijev hidrogenkarbonat]]
[[id:Natrium bikarbonat]]
[[is:Matarsódi]]
[[it:Bicarbonato di sodio]]
[[he:סודה לשתייה]]
[[lt:Natrio hidrokarbonatas]]
[[hu:Nátrium-hidrogénkarbonát]]
[[ml:സോഡിയം ബൈകാർബണേറ്റ്]]
[[nl:Natriumwaterstofcarbonaat]]
[[ja:炭酸水素ナトリウム]]
[[no:Natron]]
[[pl:Wodorowęglan sodu]]
[[pt:Bicarbonato de sódio]]
[[ro:Bicarbonat de sodiu]]
[[ru:Гидрокарбонат натрия]]
[[simple:Sodium bicarbonate]]
[[sk:Hydrogénuhličitan sodný]]
[[sr:Natrijum bikarbonat]]
[[fi:Natriumbikarbonaatti]]
[[sv:Natriumvätekarbonat]]
[[te:సోడా]]
[[th:โซเดียมไบคาร์บอเนต]]
[[tr:Sodyum bikarbonat]]
[[uk:Гідрокарбонат натрію]]
[[vi:Natri bicacbonat]]
[[zh:碳酸氢钠]]' |
New page wikitext, after the edit (new_wikitext ) | '{{chembox
| Watchedfields = changed
| verifiedrevid = 311801095
| Name = Sodium Bicarbonate
| ImageFile = SodiumBicarbonate.svg
| ImageSize = 150px
| ImageFileL1 = Sodium-3D.png
| ImageSizeL1 = 80px
| ImageFileR1 = Bicarbonate-ion-3D-balls-B.png
| ImageSizeR1 = 120px
| ImageFile2 = Sodium bicarbonate.jpg
| IUPACName = Sodium hydrogen carbonate
| OtherNames = Sodium bicarbonate<br/>Bicarbonate of soda<br/>Baking soda<br/>Sodium hydrogencarbonate<br/>[[Nahcolite]]
| Section1 = {{Chembox Identifiers
| CASNo = 144-55-8
| CASNo_Ref = {{cascite}}
| PubChem = 516892
| ChemSpiderID = 8609
| RTECS = VZ0950000
}}
| Section2 = {{Chembox Properties
| Na=1|H=1|C=1|O=3
| Appearance = white crystalline solid
| Odor = odorless
| Density = 2.173 g/cm<sup>3</sup>
| Solubility = 7.8 g/100 mL (18 °C) <br /> 10 g/100 mL (20 °C)
| SolubleOther = insoluble in [[alcohol]], [[ether]]
| MeltingPt = decomp: 323.15 K (50 °C) - 543.15 K (270 °C)
| RefractIndex = 1.3344
| pKa = 10.3
}}
| Section7 = {{Chembox Hazards
| ExternalMSDS = [http://siri.org/msds/f2/bdm/bdmjw.html External MSDS]
| EUIndex = Not listed
| MainHazards =
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
| FlashPt = Non-flammable
| RPhrases =
| SPhrases =
| LD50 = 4220 mg/kg
}}
| Section8 = {{Chembox Related
| OtherAnions = [[Sodium carbonate]]
| OtherCations = [[Potassium bicarbonate]]<br/>[[Ammonium bicarbonate]]
| OtherCpds = [[Sodium bisulfate]]<br/>[[Sodium hydrogen phosphate]]
}}
}}
'''Sodium bicarbonate''' or '''sodium hydrogen carbonate''' is the [[chemical compound]] with the formula NaHCO<sub>3</sub>. 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 washing soda ([[sodium carbonate]]). It is a component of the mineral [[natron]] and is found dissolved in many [[mineral spring]]s. The natural mineral form is known as '''[[nahcolite]]'''. It is found in its dissolved form in [[bile]], where it serves to neutralize the acidity of the [[hydrochloric acid]] produced by the stomach, and is excreted into the duodenum of the small intestine via the bile duct. It is also produced artificially.
Since it has long been known and is widely used, the [[Salt (chemistry)|salt]] has many related names such as '''baking soda''', '''bread soda''', '''cooking soda''', '''bicarbonate of soda'''. Colloquially, its name is shortened to '''''sodium bicarb''''', '''''bicarb soda''''', or simply '''''bicarb'''''. 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]]. The term has now fallen out of common usage.
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==Production==
{{Main|Solvay process}}
NaHCO<sub>3</sub> is mainly prepared by the [[Solvay process]], which is the reaction of [[calcium carbonate]], [[sodium chloride]], [[ammonia]], and [[carbon dioxide]] in water. It is produced on the scale of about 100,000 ton/year (as of 2001).<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref>
NaHCO<sub>3</sub> may be obtained by the reaction of [[carbon dioxide]] with an aqueous solution of [[sodium hydroxide]]. The initial reaction produces [[sodium carbonate]]:
:CO<sub>2</sub> + 2 NaOH → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O
Further addition of [[carbon dioxide]] produces sodium bicarbonate, which at sufficiently high concentration will precipitate out of solution:
:Na<sub>2</sub>CO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O → 2 NaHCO<sub>3</sub>
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 method:
: Na<sub>2</sub>CO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O → 2 NaHCO<sub>3</sub>
==Mining==
Naturally occurring deposits of nahcolite (NaHCO<sub>3</sub>) are found in the [[Eocene]]-age (55.8 ± 0.2 - 33.9 ± 0.1 Ma) [[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 in-situ leach techniques involving dissolution of the nahcolite by heated water which is pumped through the nahcolite beds and reconstituted through a natural cooling crystallization process.
==Chemistry==
Sodium bicarbonate is an [[amphoteric]] compound. Aqueous solutions are mildly [[alkaline]] due to the formation of [[carbonic acid]] and [[hydroxide]] ion:
:HCO{{su|b=3|p=−}} + H<sub>2</sub>O → {{chem|H|2|CO|3}} + OH<sup>−</sup>
Sodium bicarbonate can be used as a wash to remove any acidic impurities from a "crude" liquid, producing a purer sample. Reaction of sodium bicarbonate and an [[acid]] to give a salt and carbonic acid, which readily decomposes to carbon dioxide and water:
:NaHCO<sub>3</sub> + HCl → NaCl + H<sub>2</sub>CO<sub>3</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]]) and presents a simple and showy demonstration of a [[chemical reaction]]. The products of the ensuing two-stage reaction are [[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)|base]]s such as [[sodium hydroxide]] to form [[carbonate]]s:
:NaHCO<sub>3</sub> + NaOH → Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O
Sodium bicarbonate reacts with [[carboxyl group]]s in proteins to give a brisk effervescence from the formation of {{chem|CO|2}}. This reaction is used to test for the presence of carboxylic groups in protein.
===Thermal decomposition===
Above 70 °C, sodium bicarbonate gradually decomposes into [[sodium carbonate]], [[water]] and [[carbon dioxide]]. The conversion is fast at 200 °C:<ref> {{cite web | publisher = General Chemistry Online | title = Decomposition of Carbonates | url = http://antoine.frostburg.edu/chem/senese/101/inorganic/faq/carbonate-decomposition.shtml}} </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]] (at around 1000 °C):
: Na<sub>2</sub>CO<sub>3</sub> → Na<sub>2</sub>O + CO<sub>2</sub>
These conversions are relevant to the use of NaHCO<sub>3</sub> as a fire-suppression agent ("BC powder") in some dry powder [[fire extinguisher]]s.
==Applications==
===Cooking===
{{Main|Leavening agent}}
Sodium bicarbonate is primarily used in [[cooking]] ([[baking]]) where it reacts with other components to release carbon dioxide, that helps [[dough]] rise. The acidic compounds that induce this reaction include [[phosphates]], [[cream of tartar]], [[Lemon|lemon juice]], [[yogurt]], [[buttermilk]], [[Cocoa solids|cocoa]], [[vinegar]], etc. Sodium bicarbonate can be substituted for [[baking powder]] provided sufficient acid reagent is also added to the recipe.<ref>Radiation Cookery Book 45<sup>th</sup> Edition, Radiation Group Sales Ltd 1954</ref> Many forms of baking powder contain sodium bicarbonate combined with one or more acidic phosphates (especially good) or cream of tartar. It can also be used for softening peas (⅛ tsp. per pint of water and bring to boil for one hour)
Thermal decomposition causes sodium bicarbonate alone to act as a raising agent by releasing carbon dioxide at baking temperatures. The mixture for cakes using this method can be allowed to stand before baking without any premature release of carbon dioxide.
===Neutralization of acids and bases===
Many laboratories keep a bottle of sodium bicarbonate powder within easy reach, because sodium bicarbonate is [[amphoterism|amphoteric]], reacting with [[PH|acids and bases]]. Furthermore, as it is relatively innocuous in most situations, there is no harm in using excess sodium bicarbonate. Lastly, sodium bicarbonate powder may be used to smother a small fire.<ref name="arm"/>
A wide variety of applications follows from its neutralization properties, including reducing the spread of [[white phosphorus]] from incendiary bullets inside an afflicted soldier's wounds.<ref>{{cite web | publisher = GlobalSecurity.org | title = White Phosphorus | url = http://www.globalsecurity.org/military/systems/munitions/wp.htm | accessdate = 2007-09-26}}</ref> Sodium bicarbonate can be added as a simple solution for raising the pH balance of water (increasing total alkalinity) where high levels of chlorine (2-5 ppm) are present as in swimming pools and aquariums.<ref>{{cite web | publisher = Arm & Hammer Baking Soda | title = Outdoor Fun: Pool Care | url = http://www.armhammer.com/myfamily/tips/outdoors.asp | date = 2003 | accessdate = 2007-09-26}}</ref>
===Medical uses===
Sodium bicarbonate is used in an [[aqueous solution]] as an [[antacid]] taken orally to treat [[acid indigestion]] and [[heartburn]].<ref>{{cite web | publisher = Jackson Siegelbaum Gastroenterology | url = http://www.gicare.com/pated/sodium_bicarbonate.htm | title = Sodium Bicarbonate | date = 1998}}</ref> It may also be used in an oral form to treat chronic forms of metabolic acidosis such as [[chronic renal failure]] and [[renal tubular acidosis]]. Sodium bicarbonate may also be useful in urinary alkalinization for the treatment of [[aspirin overdose]] and [[uric acid]] renal stones.
An aqueous solution is sometimes administered [[intravenous]]ly for cases of [[acidosis]], or when there are insufficient sodium or bicarbonate ions 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 = 2004-07-13}}</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. It is for this reason that sodium bicarbonate is used in medically supervised [[cardiopulmonary resuscitation]]. Infusion of bicarbonate is indicated only when the blood pH is marked (<7.1-7.0) low.<ref>{{Cite web |publisher=emedicine |url=http://emedicine.medscape.com/article/301574-treatment |title=Respiratory Acidosis: Treatment & Medication}}</ref>
It is used as well for treatment of [[hyperkalemia]]. Since sodium bicarbonate can cause [[alkalosis]], it is sometimes used to treat aspirin overdoses. Aspirin requires an acidic environment for proper absorption, and the basic environment diminishes aspirin absorption in the case of an overdose. Sodium bicarbonate has also been used in the treatment of [[tricyclic antidepressant overdose]].<ref name="pmid9142034">{{cite journal |pmid=9142034 |year=1997 |month=Apr |author=Knudsen, K; Abrahamsson, J |title=Epinephrine and sodium bicarbonate independently and additively increase survival in experimental amitriptyline poisoning |volume=25 |issue=4 |pages=669–74 |issn=0090-3493 |journal=Critical care medicine |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 insect bites.<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 = 2008-01-15}}</ref>
Adverse reactions to the administration of sodium bicarbonate can include [[metabolic alkalosis]], [[edema]] due to sodium overload, [[congestive heart failure]], [[hyperosmolar syndrome]], hypervolemic [[hypernatremia]], and [[hypertension]] due to increased sodium. In patients who consume a high calcium or dairy-rich diet, [[calcium supplements]], or calcium-containing antacids such as [[calcium carbonate]] (e.g., Tums), the use of sodium bicarbonate can cause [[milk-alkali syndrome]], which can result in [[metastatic calcification]], [[kidney stones]], and [[kidney failure]].
Sodium bicarbonate is also used as an ingredient in some mouthwashes. It works as a mechanical cleanser on the teeth and gums, neutralizes the production of acid in the mouth and also as an [[antiseptic]] to help prevent infections occurring.
Sodium bicarbonate can be used to cover an allergic reaction of poison ivy, oak, or sumac to relieve some of the itching that is associated with it (an alternative to buying hydrocortisone cream).<ref>http://www.virtuowl.com/bicarb-lab/WhatisSodiumBicarbonateUsedFor.html</ref>
Sodium bicarbonate can be used as an exfoliant. Its particles are rounded and fine in texture, making it both effective and gentle on the skin. Using baking soda as an exfoliating scrub will remove dead skin cells, which can be discolored from hyperpigmentation and scarring.
===Personal hygiene===
A paste made from sodium bicarbonate and a 3% [[hydrogen peroxide]] solution can be used as an alternative to commercial non-fluoride [[toothpaste]]s, and sodium bicarbonate in combination with other ingredients can be used to make a dry or wet [[deodorant]]. Sodium bicarbonate is a common ingredient in alternative and natural brands of toothpaste and deodorant. It may also be used as a shampoo.<ref name = "Bouchard"> Four Green Steps, Mallory Bouchard (2010). http://www.fourgreensteps.com/infozone/featured-zone/a-green-and-healthy-beauty-secret-going-shampoo-free </ref>
===Soda loading===
Small amounts of sodium bicarbonate have been shown to be useful as a supplement for endurance athletes,<ref>{{cite news| url=http://women.timesonline.co.uk/tol/life_and_style/women/body_and_soul/article4539000.ece | work=The Times | location=London | title=Is bicarbonate of soda a performanceenhancing drug | first=Peta | last=Bee | date=2008-08-16 | accessdate=2010-05-23}}</ref> but overdose is a serious risk.<ref>http://www.umm.edu/ency/article/002749all.htm</ref>
===As a cleaning agent===
A paste from baking soda can be very effective when used in cleaning and scrubbing.<ref>{{cite web|url=http://www.armhammer.com/basics/magic/#3 |title=Arm & Hammer Baking Soda - Basics - The Magic Of Arm & Hammer Baking Soda |publisher=Armhammer.com |date= |accessdate=2009-07-30}}</ref> For cleaning aluminium objects, the use of sodium bicarbonate is discouraged as it attacks the thin unreactive protective oxide layer of this otherwise very reactive metal. A solution in warm water will remove the [[tarnish]] from [[silver]] when the silver is in contact with a piece of [[aluminium foil]].<ref>[http://www.instructables.com/id/EWU42JVP9EEV2ZBWZL/ instructables.com]</ref>
Baking soda is commonly added to the rinse cycles of washing machines (together with the detergent) as a replacement for softener and also to remove odors. Sodium bicarbonate is also effective in removing heavy tea and coffee stains from cups when diluted with warm water.
===Cattle feed supplement===
Sodium bicarbonate is sold as a [[cattle]] feed supplement, in particular as a [[buffering agent]] for the [[rumen]].
===Miscellaneous===
Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire.<ref name=arm>{{cite web|url=http://www.armhammer.com/basics/magic/#9 |title=Arm & Hammer Baking Soda - Basics - The Magic Of Arm & Hammer Baking Soda |publisher=Armhammer.com |date= |accessdate=2009-07-30}}</ref> However, it should not be applied to fires in [[deep fryer]]s as it 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 [[ammonium phosphate]] in ABC extinguishers. The alkali 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. Because it can act as an alkali, the agent has a mild [[saponification]] effect on hot grease, which forms a smothering soapy foam. Dry chemicals have since fallen out of favor for kitchen fires as they have no cooling effect compared to the extremely effective wet chemical agents specifically designed for such hazards.{{Citation needed|date=September 2007}}
Sodium bicarbonate is used in a process for cleaning paint called [[sodablasting]]. It can be administered to pools, spas, and garden ponds to raise [[pH]] levels.<ref>{{cite web|url=http://www.armhammer.com/basics/magic/#8 |title=Arm & Hammer Baking Soda - Basics - The Magic Of Arm & Hammer Baking Soda |publisher=Armhammer.com |date= |accessdate=2009-07-30}}</ref> It has [[disinfectant]] and [[antiseptic]] properties,<ref>{{cite journal |pmid=16540196 |year=2006 |month=May |author=Malik, Ys; Goyal, Sm |title=Virucidal efficacy of sodium bicarbonate on a food contact surface against feline calicivirus, a norovirus surrogate |volume=109 |issue=1-2 |pages=160–3 |issn=0168-1605 |doi=10.1016/j.ijfoodmicro.2005.08.033 |journal=International journal of food microbiology}}</ref> and it may be an effective [[fungicide]] against some organisms.<ref>{{cite journal |pmid=18396809 |year=2007 |month= |author=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 |volume=72 |issue=4 |pages=773–7 |issn=1379-1176 |journal=Communications in agricultural and applied biological sciences |url=http://toxnet.nlm.nih.gov/cgi-bin/sis/search/r?dbs+hsdb:@term+@rn+7440-09-7 |format=Free full text}}</ref>
Because it can be used to absorb odors, it is a tried-and-true method of used booksellers. The baking soda will absorb the musty smell, leaving the books less odorous.<ref>{{cite journal |title=Book Repair for BookThinkers: How To Remove Odors From Books |author=Gail Altman |date=2006-05-22 |issue=69 |work=The BookThinker |url=http://www.bookthink.com/0069/69alt.htm}}</ref>
== See also ==
* [[Carbonic acid]]
* [[Baking powder]]
* [[List of minerals]]
* [[Nahcolite]]
* [[Natron]]
* [[Natrona]] (disambiguation)
* [[Trona]]
==References==
{{reflist|2}}
==Further reading==
*{{cite journal |pmid=15126714 |year=2004 |month=May |author=Bishop, D; Edge, J; Davis, C; Goodman, C |title=Induced metabolic alkalosis affects muscle metabolism and repeated-sprint ability. |volume=36 |issue=5 |pages=807–13 |issn=0195-9131 |journal=Medicine and science in sports and exercise}}
==External links==
{{Commons category|Sodium bicarbonate}}
{{Cookbook|Baking soda}}
*[http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc10/icsc1044.htm International Chemical Safety Card 1044]
*[http://chemistry.about.com/cs/foodchemistry/f/blbaking.htm/ Differences between Baking Soda and Baking Powder]
{{Sodium compounds}}
{{Antacids}}
{{DEFAULTSORT:Sodium Bicarbonate}}
[[Category:Sodium compounds]]
[[Category:Bases]]
[[Category:Antacids]]
[[Category:Bicarbonates]]
[[Category:Acid salts]]
[[Category:Fire suppression agents]]
[[Category:Household chemicals]]
[[Category:Leavening agents]]
[[ar:بيكربونات الصوديوم]]
[[bs:Natrijum hidrogen karbonat]]
[[bg:Натриев бикарбонат]]
[[ca:Bicarbonat de sodi]]
[[cs:Hydrogenuhličitan sodný]]
[[da:Natron]]
[[de:Natriumhydrogencarbonat]]
[[et:Naatriumvesinikkarbonaat]]
[[es:Bicarbonato de sodio]]
[[fa:جوش شیرین]]
[[fr:Bicarbonate de sodium]]
[[ko:탄산 수소 나트륨]]
[[hi:सोडियम बाईकार्बोनेट]]
[[hr:Natrijev hidrogenkarbonat]]
[[id:Natrium bikarbonat]]
[[is:Matarsódi]]
[[it:Bicarbonato di sodio]]
[[he:סודה לשתייה]]
[[lt:Natrio hidrokarbonatas]]
[[hu:Nátrium-hidrogénkarbonát]]
[[ml:സോഡിയം ബൈകാർബണേറ്റ്]]
[[nl:Natriumwaterstofcarbonaat]]
[[ja:炭酸水素ナトリウム]]
[[no:Natron]]
[[pl:Wodorowęglan sodu]]
[[pt:Bicarbonato de sódio]]
[[ro:Bicarbonat de sodiu]]
[[ru:Гидрокарбонат натрия]]
[[simple:Sodium bicarbonate]]
[[sk:Hydrogénuhličitan sodný]]
[[sr:Natrijum bikarbonat]]
[[fi:Natriumbikarbonaatti]]
[[sv:Natriumvätekarbonat]]
[[te:సోడా]]
[[th:โซเดียมไบคาร์บอเนต]]
[[tr:Sodyum bikarbonat]]
[[uk:Гідрокарбонат натрію]]
[[vi:Natri bicacbonat]]
[[zh:碳酸氢钠]]' |