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Sodium bicarbonate

Names
IUPAC name Sodium hydrogen carbonate
Other names Baking soda, bicarb (laboratory slang), bicarbonate of soda, nahcolite
Identifiers
CAS Number	144-55-8
3D model (JSmol)	Interactive image
Beilstein Reference	4153970
ChEBI	CHEBI:32139
ChEMBL	ChEMBL1353
ChemSpider	8609
DrugBank	DB01390
ECHA InfoCard	100.005.122
EC Number	205-633-8
E number	E500(ii) (acidity regulators, ...)
IUPHAR/BPS	4507
KEGG	C12603
MeSH	Sodium+bicarbonate
PubChem CID	516892
RTECS number	VZ0950000
UNII	8MDF5V39QO
CompTox Dashboard (EPA)	DTXSID9021269
InChI InChI=1S/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1Key: UIIMBOGNXHQVGW-UHFFFAOYSA-M InChI=1/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1Key: UIIMBOGNXHQVGW-REWHXWOFAQ
SMILES .OC()=O
Properties
Chemical formula	NaHCO 3
Molar mass	84.0066 g mol
Appearance	White crystals
Odor	Odorless
Density	2.20 g/cm
Melting point	(Decomposes to sodium carbonate starting at 50 °C)
Solubility in water	69 g/L (0 °C) 96 g/L (20 °C) 165 g/L (60 °C)
Solubility	0.02 wt% acetone, 2.13 wt% methanol @22 °C. insoluble in ethanol
log P	−0.82
Acidity (pKa)	10.329 6.351 (carbonic acid)
Refractive index (nD)	nα = 1.377 nβ = 1.501 nγ = 1.583
Structure
Crystal structure	Monoclinic
Thermochemistry
Heat capacity (C)	87.6 J/mol K
Std molar entropy (S298)	101.7 J/mol K
Std enthalpy of formation (ΔfH298)	−950.8 kJ/mol
Gibbs free energy (ΔfG)	−851.0 kJ/mol
Pharmacology
ATC code	B05CB04 (WHO) B05XA02 (WHO), QG04BQ01 (WHO)
Routes of administration	Intravenous, oral
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Causes serious eye irritation
NFPA 704 (fire diamond)	2 0 1
Flash point	Incombustible
Lethal dose or concentration (LD, LC):
LD50 (median dose)	4220 mg/kg (rat, oral)
Safety data sheet (SDS)	External MSDS
Related compounds
Other anions	Sodium carbonate
Other cations	Ammonium bicarbonate Potassium bicarbonate
Related compounds	Sodium bisulfate Sodium hydrogen phosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Y verify (what is  ?) Infobox references

Sodium bicarbonate (IUPAC name: sodium hydrogen carbonate), commonly known as baking soda (especially in North America and New Zealand) or bicarbonate of soda, is a chemical compound with the formula NaHCO₃. It is a salt composed of a sodium cation (Na) and a bicarbonate anion (HCO₃). 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.

Nomenclature

Because 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. The term baking soda is more common in the United States, whereas bicarbonate of soda is more common in Australia and Britain. In colloquial usage, the names sodium bicarbonate and bicarbonate of soda are often truncated; forms such as sodium bicarb, bicarb soda, bicarbonate, and bicarb are common.

The word saleratus, from Latin sal æratus (meaning "aerated salt"), was widely used in the 19th century for both sodium bicarbonate and potassium bicarbonate.

It is known as one of the E number food additives E500.

The prefix bi in bicarbonate comes from an outdated naming system and is based on the observation that there is twice as much carbonate (CO₃) per sodium in sodium bicarbonate (NaHCO₃) as there is in sodium carbonate (Na₂CO₃). The modern chemical formulas of these compounds express their precise chemical compositions (which were unknown when the names sodium carbonate and sodium bicarbonate were coined) as sodium hydrogen carbonate (NaHCO₃) and sodium carbonate (Na₂CO₃). These names are unambiguous since sodium always has the +1 oxidation state and carbonate the −2 oxidation state.

Uses

Cooking

Leavening

In cooking, baking soda is primarily used in baking as a leavening agent. When it reacts with acid, carbon dioxide is released, which causes expansion of the batter and forms the characteristic texture and grain in cakes, quick breads, soda bread, and other baked and fried foods. The acid-base reaction can be generically represented as follows:

NaHCO₃ + H → Na + CO₂ + H₂O

Acidic materials that induce this reaction include hydrogen phosphates, cream of tartar, lemon juice, yogurt, buttermilk, cocoa, and vinegar. Baking soda may be used together with sourdough, which is acidic, making a lighter product with a less acidic taste.

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 80 °C (180 °F), as follows:

2 NaHCO₃ → Na₂CO₃ + H₂O + CO₂

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 CO₂ is released (one CO₂ molecule is formed for every two equivalents of NaHCO₃). 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. 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.

When adding acid, alkaline ingredients such as whole milk or Dutch-processed cocoa are often added to baked foods to avoid an over-acidic taste from the added acid.

Baking powder

Baking powder, also sold for cooking, contains around 30% of bicarbonate, and various acidic ingredients which are activated by the addition of water, without the need for additional acids in the cooking medium. Many forms of baking powder contain sodium bicarbonate combined with calcium acid phosphate, sodium aluminium phosphate, or cream of tartar. Baking soda is alkaline; the acid used in baking powder avoids a metallic taste when the chemical change during baking creates sodium carbonate.

Other

Sodium bicarbonate was sometimes used in cooking green vegetables, as it gives them a bright green colour—which has been described as artificial-looking—due to its reacting with chlorophyll to produce chlorophyllin. However, this tends to affect taste, texture and nutritional content, and is no longer common.

Baking soda is used to soften pulses (peas, beans) before and during cooking, as in the traditional British mushy peas recipe for soaking the peas. The main effect of sodium bicarbonate is to modify the pH of the soaking solution and cooking water; this softens the hard external shell, reduces cooking times and may alter the percentage of nutrients in the dish, its flavour and consistence.

Baking soda may react with acids in food, including vitamin C (L-ascorbic acid).

It is used in Asian and Latin American cuisine to tenderize meats. It is also used in breading, such as for fried foods, to enhance crispness and allow passages for steam to escape, so the breading is not blown off during cooking.

Fungicide and pest control

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

Alkalinity/pH increase

Sodium bicarbonate can be added to swimming pools, spas, and garden ponds to raise the total alkalinity (increase the pH).

Pyrotechnics

Sodium bicarbonate is one of the main components of the common "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.

Mild disinfectant

It has weak disinfectant properties, and it may be an effective fungicide against some organisms. Because baking soda will absorb musty smells, it has become a reliable method for used book sellers when making books less malodorous.

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. However, it should not be applied to fires in deep fryers; the sudden release of gas may cause the grease to splatter. Sodium bicarbonate is used in BC dry chemical fire extinguishers as an alternative to the more corrosive diammonium 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. Because it can act as an alkali, the agent has a mild saponification effect on hot grease, which forms a smothering, soapy foam.

Neutralization of acids

Sodium bicarbonate reacts spontaneously with acids, releasing CO₂ gas as a reaction product. It is commonly used to neutralize unwanted acid solutions or acid spills in chemical laboratories. It is not appropriate to use sodium bicarbonate to neutralize base even though it is amphoteric, reacting with both acids and bases.

Medical uses and health

Sodium bicarbonate mixed with water can be used as an antacid to treat acid indigestion and heartburn. Its reaction with stomach acid produces salt, water, and carbon dioxide:

NaHCO₃ + HCl → NaCl + H₂O + CO₂(g)

A mixture of sodium bicarbonate and polyethylene glycol such as PegLyte, dissolved in water and taken orally, is an effective gastrointestinal lavage preparation and laxative prior to gastrointestinal surgery, gastroscopy, etc.

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. 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. For this reason, sodium bicarbonate is used in medically supervised cardiopulmonary resuscitation. Infusion of bicarbonate is indicated only when the blood pH is markedly low (< 7.1–7.0).

HCO₃ is used for treatment of hyperkalemia, as it will drive K back into cells during periods of acidosis. 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. 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).

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. 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".

Sodium bicarbonate can be added to local anesthetics, to speed up the onset of their effects and make their injection less painful. It is also a component of Moffett's solution, used in nasal surgery.

It has been proposed that acidic diets weaken bones. One systematic meta-analysis of the research shows no such effect. 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.

Antacid (such as baking soda) solutions have been prepared and used by protesters to alleviate the effects of exposure to tear gas during protests.

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 (HCO₃ + H → H₂O + CO₂↑ or, more precisely, HCO₃ + H₃O → 2 H₂O + CO₂↑) leaving the medication dissolved in the water together with the resulting salt (in this example, sodium tartrate).

Personal hygiene

Toothpaste containing sodium bicarbonate has in several studies been shown to have a better whitening and plaque removal effect than toothpastes without it.

Sodium bicarbonate is also used as an ingredient in some mouthwashes. It has anticaries and abrasive properties. 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. Sodium bicarbonate in combination with other ingredients can be used to make a dry or wet deodorant. Sodium bicarbonate may be used as a buffering agent, combined with table salt, when creating a solution for nasal irrigation.

It is used in eye hygiene to treat blepharitis. This is done by addition of 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.

Veterinary uses

Sodium bicarbonate is used as a cattle feed supplement, in particular as a buffering agent for the rumen.

In sports

Although small doses of sodium bicarbonate have been used as a supplement for athletes in speed-based events, such as middle-distance running, there is insufficient evidence for benefit, and overdose is a health risk because sodium bicarbonate may cause gastrointestinal irritation.

Cleaning agent

Sodium bicarbonate is used in a process for removing paint and corrosion called sodablasting. As a blasting medium, sodium bicarbonate is used to remove removal surface contamination from softer and less resilient substrates such as aluminium, copper or timber which could be damaged by silica sand abrasive media.

A manufacturer recommends a paste made from baking soda with minimal water as a gentle scouring powder, and is useful in removing surface rust, as the rust forms a water-soluble compound when in a concentrated alkaline solution; cold water should be used, as hot-water solutions can corrode steel. Sodium bicarbonate attacks the thin protective oxide layer that forms on aluminium, making it unsuitable for cleaning this metal. A solution in warm water will remove the tarnish from silver when the silver is in contact with a piece of aluminium foil. Baking soda is commonly added to washing machines as a replacement for water softener and to remove odors from clothes. It is also effective in removing heavy tea and coffee stains from cups when diluted with warm water.

During the Manhattan Project to develop the nuclear bomb in the early 1940s, the chemical toxicity of uranium was an issue. Uranium oxides 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 used for counterweights in a civilian context, and in armour-piercing projectiles. DU is not removed by normal laundering; washing with about 6 ounces (170 g) of baking soda in 2 gallons (7.5 l) of water will help to wash it out.

Odor control

It is often claimed that baking soda is an effective odor remover, and it is often recommended that an open box be kept in the refrigerator to absorb odor. This idea was promoted by the leading U.S. brand of baking soda, Arm & Hammer, in an advertising campaign starting in 1972. 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, there is little evidence that it is in fact effective in this application.

Chemistry

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
₂CO
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 produces 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

Thermal decomposition

At temperatures from 80-100 °C (176-212 °F), sodium bicarbonate gradually decomposes into sodium carbonate, water, and carbon dioxide. The conversion is faster at 200 °C (392 °F):

2 NaHCO₃ → Na₂CO₃ + H₂O + CO₂

Most bicarbonates undergo this dehydration reaction. Further heating converts the carbonate into the oxide (above 850 °C/1,560 °F):

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.

History

In 1791, French chemist Nicolas Leblanc produced sodium carbonate, also known as soda ash. In 1846, two American bakers, John Dwight and Austin Church, established the first factory in the United States to produce baking soda from sodium carbonate and carbon dioxide.

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.

In 1919, a U.S. Senator declared that bicarbonate of soda could cure the Spanish flu.... In the midst of the debate on January 26, 1919, Senator Overman 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." - American Pandemic: The Lost Worlds of the 1918 Influenza Epidemic, Oxford University Press, March 15, 2012, page 178

Production

Sodium bicarbonate is produced industrially from sodium carbonate:

Na₂CO₃ + CO₂ + H₂O → 2 NaHCO₃

It is produced on the scale of about 100,000 tonnes/year (as of 2001). 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.

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).

NaCl + CO₂ + NH₃ + H₂O → NaHCO₃ + NH₄Cl

Although of no practical value, NaHCO₃ may be obtained by the reaction of carbon dioxide with an aqueous solution of sodium hydroxide:

CO₂ + NaOH → NaHCO₃

Mining

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 common underground mining techniques such as bore, drum, and longwall mining in a fashion very similar to coal mining.

Limited amounts of product are further obtained by solution mining, pumping heated water through previously mined nahcolite beds and reconstituting the dissolved nahcolite above ground through a natural cooling crystallization process. Currently, only Genesis Alkali (formerly Tronox, formerly FMC) in the Green River Wyoming basin has successfully commercially solution mined the product.

In popular culture

Film

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." 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."

See also

• Carbonic acid
• List of ineffective cancer treatments
• List of minerals
• Natron
• Natrona (disambiguation)
• Trona

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Bibliography

• Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. ISBN 978-1439855119. {{cite book}}: Unknown parameter |name-list-format= ignored (|name-list-style= suggested) (help)

External links

• International Chemical Safety Card 1044

• Acid salts
• Antacids
• Bases (chemistry)
• Bicarbonates
• Chemical substances for emergency medicine
• Fire suppression agents
• Household chemicals
• Leavening agents
• Sodium compounds
• E-number additives