Sodium bicarbonate

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Sodium bicarbonate
SodiumBicarbonate.svg
Ball and stick model of a sodium cation Ball and stick model of a bicarbonate anion
Sample of sodium bicarbonate
Identifiers
CAS number 144-55-8 YesY
PubChem 516892
ChemSpider 8609 YesY
UNII 8MDF5V39QO YesY
EC number 205-633-8
DrugBank DB01390
KEGG C12603 YesY
MeSH Sodium+bicarbonate
ChEBI CHEBI:32139 YesY
ChEMBL CHEMBL1353 YesY
RTECS number VZ0950000
ATC code B05CB04,B05XA02, QG04BQ01
Beilstein Reference 4153970
Jmol-3D images Image 1
Properties
Molecular formula NaHCO
3
Molar mass 84.007 g mol−1
Appearance White crystals
Odor odorless
Density 2.20 g cm−3[1]
Melting point 50 °C (122 °F; 323 K) (decomposes to sodium carbonate)
Solubility in water 9 g/100 mL

69 g/L (0 °C)[2]
96 g/L (20 °C)[3]
165 g/L (60 °C)[3]
236 g/L (100 °C)[2]

Solubility 0.02 %wt acetone, 2.13 %wt methanol @22°C.[4] insoluble in ethanol
log P -0.82
Acidity (pKa) 10.329[5]

6.351 (carbonic acid)[5]

Refractive index (nD) 1.3344
Structure
Crystal structure monoclinic
Pharmacology
Routes of
administration
Intravenous, oral
Hazards
MSDS External MSDS
Main hazards Causes serious eye irritation
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point incombustible
LD50 4220 mg/kg ( rat, oral ) [6]
Related compounds
Other anions Sodium carbonate
Other cations Ammonium bicarbonate

Potassium bicarbonate

Related compounds Sodium bisulfate

Sodium hydrogen phosphate

Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY (verify) (what is: YesY/N?)
Infobox references

Sodium bicarbonate or sodium hydrogen carbonate is the chemical compound with the formula NaHCO3. Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder. It has a slightly salty, alkaline taste resembling that of washing soda (sodium carbonate). The natural mineral form is nahcolite. It is a component of the mineral natron and is found dissolved in many mineral springs. It is among the food additives encoded by European Union, identified by the initials E 500. Since it has long been known and is widely used, the salt has many related names such as baking soda, bread soda, cooking soda, and bicarbonate of soda.[note 1] The word saleratus, from 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[edit]

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.[7]

This compound, referred to as saleratus, is mentioned in the famous novel Captains Courageous by Rudyard Kipling as being used extensively in the 1800s in commercial fishing to prevent freshly-caught fish from spoiling.[8]

Production[edit]

Main article: Solvay process

NaHCO3 is mainly prepared by the Solvay process, which is the reaction of sodium chloride, ammonia, and carbon dioxide in water. Calcium carbonate is used as the source of CO2 and the resultant calcium oxide is used to recover the ammonia from the ammonium chloride. The product shows a low purity (75%). Pure product is obtained from sodium carbonate, water and carbon dioxide as reported in one of the following reactions. It is produced on the scale of about 100,000 tonnes/year (as of 2001).[9]

NaHCO3 may be obtained by the reaction of carbon dioxide with an aqueous solution of sodium hydroxide. The initial reaction produces sodium carbonate:

CO2 + 2 NaOH → Na2CO3 + H2O

Further addition of carbon dioxide produces sodium bicarbonate, which at sufficiently high concentration will precipitate out of solution:

Na2CO3 + CO2 + H2O → 2 NaHCO3

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:

Na2CO3 + CO2 + H2O → 2 NaHCO3

Mining[edit]

Naturally occurring deposits of nahcolite (NaHCO3) 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 in situ leach techniques involving dissolution of the nahcolite by heated water pumped through the nahcolite beds and reconstituted through a natural cooling crystallization process.

Chemistry[edit]

Sodium bicarbonate is an amphoteric compound. Aqueous solutions are mildly alkaline due to the formation of carbonic acid and hydroxide ion:

HCO
3
+ H2O → H
2
CO
3
+ OH

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 produce a salt and carbonic acid, which readily decomposes to carbon dioxide and water:

NaHCO3 + HCl → NaCl + H2CO3
H2CO3 → H2O + CO2(g)

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

NaHCO3 + CH3COOH → CH3COONa + H2O + CO2(g)

Sodium bicarbonate reacts with bases such as sodium hydroxide to form carbonates:

NaHCO3 + NaOH → Na2CO3 + H2O

Sodium bicarbonate reacts with carboxyl groups in proteins to give a brisk effervescence from the formation of CO
2
. This reaction is used to test for the presence of carboxylic groups in protein.[citation needed]

Thermal decomposition[edit]

Above 50°C, sodium bicarbonate gradually decomposes into sodium carbonate, water and carbon dioxide. The conversion is fast at 200°C:[10]

2 NaHCO3 → Na2CO3 + H2O + CO2

Most bicarbonates undergo this dehydration reaction. Further heating converts the carbonate into the oxide (at over 850°C):[10]

Na2CO3 → Na2O + CO2

These conversions are relevant to the use of NaHCO3 as a fire-suppression agent ("BC powder") in some dry powder fire extinguishers.

Applications[edit]

Sodium bicarbonate is used in a process for removing paint and corrosion called sodablasting; the process is particularly suitable for cleaning aluminium panels which can be distorted by other types of abrasive. It can be administered to pools, spas, and garden ponds to raise pH levels.[11] It has weak disinfectant properties,[12][13] and it may be an effective fungicide against some organisms.[14] Because baking soda will absorb musty smells, it has become a reliable method for used-book sellers when making books less malodorous.[15]

Fire extinguisher[edit]

Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire.[16] However, it should not be applied to fires in deep fryers, as it may cause the grease to splatter.[16] Sodium bicarbonate is used in BC 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.

Cooking[edit]

Main article: Leavening agent

Sodium bicarbonate, referred to as "baking soda" is primarily used in cooking (baking), as a leavening agent. It reacts with acidic components in batters, releasing carbon dioxide, which causes expansion of the batter and forms the characteristic texture and grain in pancakes, cakes, quick breads, soda bread, and other baked and fried foods. Acidic compounds that induce this reaction include phosphates, cream of tartar, lemon juice, yogurt, buttermilk, cocoa, vinegar, etc. Sodium bicarbonate can be substituted for baking powder provided sufficient acid reagent is also added to the recipe.[17] Many forms of baking powder contain sodium bicarbonate combined with calcium acid phosphate, sodium aluminum sulphate [18] or cream of tartar.

Sodium bicarbonate was sometimes used in cooking vegetables, to make them softer, although this has gone out of fashion, as most people now prefer firmer vegetables. However, it is still used in Asian and Latin American cuisine to tenderise meats. Baking soda may react with acids in food, including vitamin C (L-ascorbic acid). It is also used in breadings such as for fried foods to enhance crispness.

Heat causes sodium bicarbonate to act as a raising agent by releasing carbon dioxide when used in baking. The carbon dioxide production starts at temperatures above 80°C. Since the reaction does not occur at room temperature, mixtures (cake batter, etc.) can be allowed to stand without rising until they are heated in the oven.

Neutralization of acids and bases[edit]

Sodium bicarbonate is amphoteric, reacting with acids and bases. It reacts violently with acids in an exothermic reaction. Sodium bicarbonate is not recommended for the clean up of acid spills, as the heat produced increases the reactivity of the acid. The large amount of carbon dioxide produced greatly increases the area of the spill. Also, sodium bicarbonate powder may be used to smother a small fire, as heating of sodium bicarbonate releases carbon dioxide.[16]

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.[19][medical citation needed]

Medical uses[edit]

Sodium bicarbonate mixed with water can be used as an antacid to treat acid indigestion and heartburn.[20] It is used as the medicinal ingredient in gripe water for infants.[21]

Intravenous sodium bicarbonate is an aqueous solution that is sometimes used for cases of acidosis, or when there are insufficient sodium or bicarbonate ions in the blood.[22] 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 markedly (<7.1–7.0) low.[23]

It is used for treatment of hyperkalemia.[medical citation needed] 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.[medical citation needed] Sodium bicarbonate has also been used in the treatment of tricyclic antidepressant overdose.[24] 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).[25]

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 consuming 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 can be used to treat an allergic reaction to plants such as poison -ivy -oak or -sumac to relieve some of the associated itching.[26]

Bicarbonate of soda can also be useful in removing splinters from the skin.[27]

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.[28]

Personal hygiene[edit]

Toothpaste containing sodium bicarbonate has in several studies shown to have a better whitening[29][29][30][31] and plaque removal effect[32][33] than toothpastes without it.

Sodium bicarbonate is also used as an ingredient in some mouthwashes. It has anti-caries and abrasive properties.[34] 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.[citation needed]

Sodium bicarbonate in combination with other ingredients can be used to make a dry or wet deodorant.[35][36] It may also be used as a shampoo.[37]

Sodium bicarbonate may be used as a buffering agent, combined with table salt, when creating a solution for nasal irrigation.[38]

In sports[edit]

Small amounts of sodium bicarbonate have been shown to be useful as a supplement for athletes in speed-based events, like middle distance running, lasting from about one to seven minutes.[39][40] However, overdose is a serious risk because sodium bicarbonate is slightly toxic;[41] gastrointestinal irritation is of particular concern.[40] Additionally, this practice causes a significant increase in dietary sodium.[citation needed]

As a cleaning agent[edit]

A paste from baking soda can be very effective when used in cleaning and scrubbing.[42] 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.[43][44] A paste of sodium bicarbonate and water is useful in removing surface rust as the rust forms a water soluble compound when in a concentrated alkaline solution.[45] Cold water should be used as hot water solutions can corrode steel.[46]

Baking soda is commonly added to washing machines as a replacement for softener and to remove odors from clothes. Sodium bicarbonate is also effective in removing heavy tea and coffee stains from cups when diluted with warm water.

During the Manhattan Project to develop the atomic bomb in the early 1940s, many scientists investigated the toxic properties of uranium. They found that uranium oxides stick very well to cotton cloth, but did not wash out with soap or laundry detergent. The uranium would wash out with a 2% solution of sodium bicarbonate (baking soda). Clothing can become contaminated with depleted uranium (DU) dust and normal laundering will not remove it. Those at risk of DU dust exposure should have their clothing washed with baking soda (about 6 ounces (170g) of baking soda in 2 gallons (7.5l) of water).[47]

As a biopesticide[edit]

Sodium bicarbonate can be an effective way of controlling fungus growth,[48] and in the United States is registered by the Environmental Protection Agency as a biopesticide.[49]

Cattle feed supplements[edit]

Sodium bicarbonate is sold as a cattle feed supplement, in particular as a buffering agent for the rumen.[50]

In popular culture[edit]

Film[edit]

Sodium bicarbonate, as 'bicarbonate of soda', was a frequent source of punch lines for Groucho Marx in Marx brothers movies. In 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."[51] In 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."[52]

Difference between baking soda and baking powder[edit]

In comparison to baking powder, baking soda is more alkaline and requires an acid to avoid the metallic taste when the chemical change creates sodium carbonate. Baking powder, on the other hand, contains baking soda, a powdered acid and cornstarch. In scientific terms, baking soda is a pure substance; baking powder is a mixture.[53]

If baking soda is used in baking, something acidic must be added to avoid the metallic taste of sodium carbonate; but with baking powder, non-acid ingredients such as whole milk or Dutch-processed cocoa must be added to avoid the over-flavouring of acidic taste.[54]

See also[edit]

Notes[edit]

  1. ^ In colloquial usage, the names sodium bicarbonate and bicarbonate of soda are often truncated. Forms such as sodium bicarb, bicarb soda, bicarbonate, bicarb or even bica are common.

References[edit]

  1. ^ "Physical Constants of Inorganic Compounds". CRC Handbook, p. 4-85.
  2. ^ a b "Aqueous solubility of inorganic compounds at various temperatures". CRC Handbook, p. 8-116.
  3. ^ a b "Sodium Bicarbonate". UNEP Publications. 
  4. ^ J. L. Ellingboe, J. H. Runnels (1966). "Solubilities of Sodium Carbonate and Sodium Bicarbonate in Acetone-Water and Methanol-Water Mixtures". J. Chem. Eng. Data 11 (3): 323–324. doi:10.1021/je60030a009. 
  5. ^ a b Goldberg, Robert N.; Kishore, Nand; Lennen, Rebecca M. "Thermodynamic quantities for the ionization reactions of buffers in water". CRC Handbook. pp. 7–13. 
  6. ^ ChemIDplus - 144-55-8 - UIIMBOGNXHQVGW-UHFFFAOYSA-M - Sodium bicarbonate [USP:JAN] - Similar structures search, synonyms, formulas, resource links, and other chemical info...
  7. ^ "Company History". Church & Dwight Co. 
  8. ^ Rudyard Kipling. Captains Courageous.  p. 25
  9. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  10. ^ a b "Decomposition of Carbonates". General Chemistry Online. 
  11. ^ "Arm & Hammer Baking Soda – Basics – The Magic Of Arm & Hammer Baking Soda". Armhammer.com. Retrieved 2009-07-30. 
  12. ^ Malik, Ys; Goyal, Sm (May 2006). "Virucidal efficacy of sodium bicarbonate on a food contact surface against feline calicivirus, a norovirus surrogate". International Journal of Food Microbiology 109 (1–2): 160–3. doi:10.1016/j.ijfoodmicro.2005.08.033. ISSN 0168-1605. PMID 16540196. 
  13. ^ William A. Rutala, Susan L. Barbee, Newman C. Aguiar, Mark D. Sobsey, David J. Weber, (2000). "Antimicrobial Activity of Home Disinfectants and Natural Products Against Potential Human Pathogens". Infection Control and Hospital Epidemiology (The University of Chicago Press on behalf of The Society for Healthcare Epidemiology of America) 21 (1): 33–38. doi:10.1086/501694. PMID 10656352. 
  14. ^ Zamani, M; Sharifi, Tehrani, A; Ali, Abadi, Aa (2007). "Evaluation of antifungal activity of carbonate and bicarbonate salts alone or in combination with biocontrol agents in control of citrus green mold". Communications in agricultural and applied biological sciences 72 (4): 773–7. PMID 18396809. 
  15. ^ Gail Altman (2006-05-22). "Book Repair for BookThinkers: How To Remove Odors From Books". The BookThinker (69). 
  16. ^ a b c "Arm & Hammer Baking Soda – Basics – The Magic Of Arm & Hammer Baking Soda". Armhammer.com. Retrieved 2009-07-30. 
  17. ^ Radiation Cookery Book 45th Edition, Radiation Group Sales Ltd 1954
  18. ^ "Glossary Ingredients". Cooking.com. 
  19. ^ "White Phosphorus". GlobalSecurity.org. Retrieved 2007-09-26. 
  20. ^ "Sodium Bicarbonate". Jackson Siegelbaum Gastroenterology. 1998. 
  21. ^ List of ingredients – Life Brand Gripe Water
  22. ^ "Sodium Bicarbonate Intravenous Infusion". Consumer Medicine Information. Better Health Channel. 2004-07-13. 
  23. ^ "Respiratory Acidosis: Treatment & Medication". emedicine. 
  24. ^ [old info]Knudsen, K; Abrahamsson, J (Apr 1997). "Epinephrine and sodium bicarbonate independently and additively increase survival in experimental amitriptyline poisoning". Critical Care Medicine 25 (4): 669–74. doi:10.1097/00003246-199704000-00019. ISSN 0090-3493. PMID 9142034. 
  25. ^ "Insect bites and stings: First aid". Mayo Clinic. 2008-01-15. 
  26. ^ [unreliable medical source?]What is Sodium Bicarbonate Used For?. Virtuowl.com. Retrieved on 2010-09-24.
  27. ^ How to Remove a Splinter with Baking Soda: 8 Steps
  28. ^ "Sodium Bicarbonate". American Cancer Society. 28 November 2008. Retrieved 7 September 2013. 
  29. ^ a b Kleber, CJ; Moore, MH, Nelson, BJ (1998). "Laboratory assessment of tooth whitening by sodium bicarbonate dentifrices.". The Journal of clinical dentistry 9 (3): 72–5. PMID 10518866. 
  30. ^ Koertge, TE; Brooks, CN, Sarbin, AG, Powers, D, Gunsolley, JC (1998). "A longitudinal comparison of tooth whitening resulting from dentifrice use.". The Journal of clinical dentistry 9 (3): 67–71. PMID 10518865. 
  31. ^ Yankell, SL; Emling, RC, Petrone, ME, Rustogi, K, Volpe, AR, DeVizio, W, Chaknis, P, Proskin, HM (1999). "A six-week clinical efficacy study of four commercially available dentifrices for the removal of extrinsic tooth stain.". The Journal of clinical dentistry 10 (3 Spec No): 115–8. PMID 10825858. 
  32. ^ Mankodi, S; Berkowitz, H; Durbin, K; Nelson, B (1998). "Evaluation of the effects of brushing on the removal of dental plaque.". The Journal of clinical dentistry 9 (3): 57–60. PMID 10518862. 
  33. ^ Putt, MS; Milleman, KR, Ghassemi, A, Vorwerk, LM, Hooper, WJ, Soparkar, PM, Winston, AE, Proskin, HM (2008). "Enhancement of plaque removal efficacy by tooth brushing with baking soda dentifrices: results of five clinical studies.". The Journal of clinical dentistry 19 (4): 111–9. PMID 19278079. 
  34. ^ Silje Storehagen, Nanna Ose og Shilpi Midha. "Dentifrices and mouthwashes ingredients and their use". Institutt for klinisk odontologi. Universitetet i Oslo. 
  35. ^ Lamb, John Henderson (31 May 1946). "Sodium Bicarbonate: An Excellent Deodorant". The Journal of Investigative Dermatology 7 (3): 131–133. doi:10.1038/jid.1946.13. 
  36. ^ "Bicarb soda: natural body deodorant". Retrieved 5 May 2012. 
  37. ^ Bouchard, Mallory (2010-05-04). "A Green and Healthy Beauty Secret: Going Shampoo-Free". Four Green Steps. 
  38. ^ Ralph B. Metson, M.D., The Harvard Medical School Guide to Healing Your Sinues (McGraw Hill 2005), at p. 68.
  39. ^ Bee, Peta (2008-08-16). "Is bicarbonate of soda a performance enhancing drug". The Times (London). Retrieved 2010-05-23. 
  40. ^ a b Ergogenic Aids. U. Retrieved on 2011-09-11.
  41. ^ Baking soda overdose – All Information. Umm.edu (2009-10-19). Retrieved on 2010-09-24.
  42. ^ "Arm & Hammer Baking Soda – Basics – The Magic Of Arm & Hammer Baking Soda". Armhammer.com. Retrieved 2009-07-30. 
  43. ^ Eco Silver Polishing. instructables.com (2006-12-20). Retrieved on 2011-10-07.
  44. ^ "Put a Shine on It". scifun.chem.wisc.edu. Retrieved 2011-03-06. 
  45. ^ Catherine E. Housecroft; Alan G. Sharpe (2008). "Chapter 22: d-block metal chemistry: the first row elements". Inorganic Chemistry, 3rd Edition. Pearson. p. 716. ISBN 978-0-13-175553-6. 
  46. ^ .http://www.sciencelab.com/msds.php?msdsId=9927263
  47. ^ Orcutt, JA. "Scientist". Pharmacology and Toxicology of Uranium Compounds. McGraw-Hill. Retrieved 21 March 2012. 
  48. ^ Potassium bicarbonate (073508) and Sodium bicarbonate (073505) Fact Sheet United States Environmental Protection Agency. Updated 17 February 2011. Retrieved 25 November 2011.
  49. ^ Registered Biopesticides 04/29/02 United States Environmental Protection Agency. Updated 29 March 2002. Retrieved 25 November 2011.
  50. ^ "Acidosis Health Warning for Livestock Farmers". Retrieved 5 May 2012. 
  51. ^ Duck Soup (1933) - Quotes - IMDb
  52. ^ A Night at the Opera (1935) - Quotes - IMDb
  53. ^ Joy the Baker Baking 101: The Difference Between Baking Soda and Baking Powder - Joy the Baker
  54. ^ joythebaker.com

Further reading[edit]

External links[edit]