Cupcakes baked with baking soda as a raising agent
Sodium bicarbonate (IUPAC name:sodium hydrogencarbonate[9]), commonly known asbaking soda orbicarbonate of soda, is achemical compound with the formulaNaHCO3. It is asalt composed of asodiumcation (Na+) and abicarbonateanion (HCO3−). Sodium bicarbonate is a white solid that iscrystalline 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 isnahcolite, although it is more commonly found as a component of the mineraltrona.[10]
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 nearbaking powder in stores. The termbaking soda is more common in the United States, whilebicarbonate of soda is more common in Australia, the United Kingdom, and New Zealand.[11] Abbreviated colloquial forms such assodium bicarb, bicarb soda,bicarbonate, andbicarb are common.[12]
The prefixbi- in "bicarbonate" comes from an outdated naming system predating molecular knowledge. It is based on the observation that there is twice as much carbonate (CO32-) per sodium in sodium bicarbonate (NaHCO3) as there is in sodium carbonate (Na2CO3).[13] The modern chemical formulas of these compounds now express their precise chemical compositions which were unknown when the namebi-carbonate of potash was coined (see also:bicarbonate).
In cooking, baking soda is primarily used inbaking as aleavening 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 breads,soda bread, and other baked and fried foods. When an acid is used, theacid–base reaction can be generically represented as follows:[14]
NaHCO3 + H+ → Na+ + CO2 + H2O
Acidic materials that induce this reaction includehydrogen phosphates,cream of tartar,lemon juice,yogurt,buttermilk,cocoa, andvinegar. Baking soda may be used together withsourdough, which is acidic, making a lighter product with a less acidic taste.[15] 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]
Heat can also by itself cause sodium bicarbonate to act as a raising agent in baking because ofthermal decomposition, releasing carbon dioxide at temperatures above 80 °C (180 °F), as follows:[16]
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 producessodium carbonate, which is strongly alkaline and gives the baked product a bitter, soapy taste and a yellow color.
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.[17][18][19] Many forms of baking powder contain sodium bicarbonate combined withcalcium acid phosphate,sodium aluminium phosphate, orcream of tartar.[20] Baking soda is alkaline; the acid used in baking powder avoids a metallic taste when the chemical change during baking creates sodium carbonate.[21]
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.[24] Sodium bicarbonate also delays combustion reactions through the release of carbon dioxide and water, both of which are flame retardants, when heated.
It has weakdisinfectant properties[25][26] and it may be an effectivefungicide against some organisms.[27] As baking soda will absorb musty smells, it has become a reliable method forused booksellers when making books less malodorous.[28]
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.[29] However, it should not be applied to fires indeep fryers; the sudden release of gas may cause the grease to splatter.[29] Sodium bicarbonate is used in BCdry chemicalfire extinguishers as an alternative to the more corrosivemonoammonium phosphate in ABC extinguishers. The alkaline nature of sodium bicarbonate makes it the only dry chemical agent, besidesPurple-K, that was used in large-scale fire suppression systems installed in commercial kitchens.[30]
Sodium bicarbonate has several fire-extinguishing mechanisms that act simultaneously. It decomposes into water and carbon dioxide when heated, anendothermic reaction that deprives the fire of heat. In addition, it forms intermediates that can scavenge thefree radicals which are responsible for thepropagation of fire.[31] Withgrease fires specifically, it also has a mildsaponification effect, producing a soapy foam that can help smother the fire.[30]
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.[32] It is not appropriate to use sodium bicarbonate to neutralize base[33] even though it isamphoteric, reacting with both acids and bases.[34]
Sodium bicarbonate is taken as a sports supplement to improve muscular endurance.[35] Studies conducted mostly in males have shown that sodium bicarbonate is most effective in enhancing performance in short-term, high-intensity activities.[36]
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) andchlorosis (one percent solution).[37] Sodium bicarbonate is also commonly used as a free choice dietary supplement in sheep to help prevent bloat.
Intravenous sodium bicarbonate in an aqueous solution is sometimes used for cases ofacidosis, or when insufficient sodium or bicarbonate ions are in the blood.[41] 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 supervisedcardiopulmonary resuscitation. Infusion of bicarbonate is indicated only when the bloodpH is markedly low (< 7.1–7.0).[42]
HCO3− is used for treatment ofhyperkalemia, as it will drive K+ back into cells during periods of acidosis.[43] Since sodium bicarbonate can causealkalosis, 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.[44] Sodium bicarbonate has also been used in the treatment oftricyclic antidepressant overdose.[45] 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).[46]
Some alternative practitioners, such asTullio 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.[47]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".[48]
Sodium bicarbonate can be added tolocal anaesthetics, to speed up the onset of their effects and make their injection less painful.[49] It is also a component ofMoffett's solution, used innasal surgery.[50]
It has been proposed that acidic diets weaken bones.[51] One systematic meta-analysis of the research shows no such effect.[52] 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.[53]
Antacid (such as baking soda) solutions have been prepared and used by protesters to alleviate the effects of exposure totear gas during protests.[failed verification][54]
Similarly to its use in baking, sodium bicarbonate is used together with a mild acid such astartaric 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↑). 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).[55]
Sodium bicarbonate is also used as an ingredient in some mouthwashes. It has anticaries and abrasive properties.[56] It works as a mechanical cleanser on the teeth and gums, neutralizes the production of acid in the mouth, and also acts as anantiseptic to help prevent infections.[57][58] Sodium bicarbonate in combination with other ingredients can be used to make a dry or wetdeodorant.[59][60] Sodium bicarbonate may be used as abuffering agent, combined with table salt, when creating a solution fornasal irrigation.[61]
It is used in eye hygiene to treatblepharitis. 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.[62][63]
Sodium bicarbonate is used in a process to remove paint and corrosion calledsodablasting. As a blasting medium, sodium bicarbonate is used to remove surface contamination from softer and less resilientsubstrates such as aluminium, copper, or timber that could be damaged by silica sand abrasive media.[65]
A manufacturer recommends a paste made from baking soda with minimal water as a gentle scouring powder.[29] Such a paste can be useful in removing surface rust because the rust forms a water-soluble compound when in a concentrated alkaline solution.[66] Cold water should be used since hot-water solutions can corrode steel.[67] Sodium bicarbonate attacks the thin protective oxide layer that forms on aluminium, making it unsuitable for cleaning this metal.[68] A solution in warm water will remove thetarnish from silver when the silver is in contact with a piece ofaluminium foil.[68][69] 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 assodium hydroxide.
During theManhattan Project to develop thenuclear bomb in the early 1940s, thechemical toxicity ofuranium was an issue.Uranium oxides were found to stick very well tocotton cloth and did not wash out withsoap orlaundry detergent. However, the uranium would wash out with a 2% solution of sodium bicarbonate. Clothing can become contaminated with toxic dust ofdepleted 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 6 ounces (170 g) of baking soda in 2 gallons (7.5 L) ofwater will help wash it out.[70]
It is often claimed that baking soda is an effective odor remover[71][better source needed] and recommended that an open box be kept in the refrigerator to absorb odor.[72] This idea was promoted by the leading U.S. brand of baking soda,Arm & Hammer, in an advertising campaign starting in 1972.[73] 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,[74][75] there is little evidence that it is effective in this application.[76][77]
An educational science experiment known as the "Baking Soda and Vinegar Volcano" uses the acid-base reaction withvinegar acid to mimic a volcanic eruption. The rapid production of CO2 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.[78] If this reaction is performed inside of a closed vessel (such as a bottle) with no way for gas to escape, it can cause anexplosion if the pressure is high enough.
Sodium bicarbonate can sometimes be used as a mildneutralization agent and a safer alternative to strong bases likesodium hydroxide.[79] Reaction of sodium bicarbonate and anacid produces a salt and carbonic acid, which readily decomposes to carbon dioxide and water:[79]
At temperatures from 80–100 °C (176–212 °F), sodium bicarbonate gradually decomposes intosodium carbonate, water, and carbon dioxide. The conversion is faster at 200 °C (392 °F):[80]
2 NaHCO3 → Na2CO3 + H2O + CO2
Most bicarbonates undergo thisdehydration reaction. Further heating converts the carbonate into theoxide (above 850 °C/1,560 °F):[80]
Na2CO3 → Na2O + CO2
The generation of carbon dioxide and water partially explain the fire-extinguishing properties of NaHCO3,[30] although other factors likeheat absorption and radicalscavenging are more significant.[31]
In nature, sodium bicarbonate occurs almost exclusively as eithernahcolite ortrona. Trona is more common, as nahcolite is more soluble in water and thechemical equilibrium between the two minerals favors trona.[10] Significant nahcolite deposits are in the United States, Botswana and Kenya, Uganda, Turkey, and Mexico.[81] The biggest trona deposits are in theGreen River basin in Wyoming.[82]
Nahcolite is sometimes found as a component ofoil shale.[83]
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.[84][85][86][87]
The wordnatron has been in use in many languages throughoutmodern times (in the forms ofanatron,natrum andnatron) and originated (likeSpanish,French andEnglishnatron as well as 'sodium') via Arabicnaṭrūn (oranatrūn; cf. the Lower Egyptian “Natrontal”Wadi El Natrun, where a mixture ofsodium carbonate and sodium hydrogen carbonate for the dehydration ofmummies was used[88]) from Greeknítron (νίτρον) (Herodotus; Atticlítron (λίτρον)), which can be traced back to ancient Egyptianntr. The Greeknítron (soda, saltpeter) was also used in Latin(sal) nitrum and in GermanSalniter (the source ofNitrogen,Nitrat etc.).[89][90] The wordsaleratus, fromLatinsal æratus (meaning "aerated salt"), was widely used in the 19th century for both sodium bicarbonate andpotassium bicarbonate.[91]
In 1791, French chemistNicolas Leblanc produced sodium carbonate (also known as soda ash). PharmacistValentin Rose the Younger is credited with the discovery of sodium bicarbonate in 1801 in Berlin. In 1846, two American bakers,John Dwight andAustin Church, established the first factory in the United States to produce baking soda from sodium carbonate andcarbon dioxide.[92]
Saleratus, potassium or sodium bicarbonate, is mentioned in the novelCaptains Courageous byRudyard Kipling as being used extensively in the 1800s in commercial fishing to prevent freshly caught fish from spoiling.[93]
In 1919,US Senator Lee Overman declared that bicarbonate of soda could cure theSpanish 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."[94]
It is produced on the scale of about 100,000 tonnes/year (as of 2001)[dubious –discuss][96] with a worldwide production capacity of 2.4 million tonnes per year (as of 2002).[97] Commercial quantities of baking soda are also produced by a similar method: soda ash, mined in the form of the oretrona, is dissolved in water and treated with carbon dioxide. Sodium bicarbonate precipitates as a solid from this solution.[citation needed]
Naturally occurring deposits ofnahcolite (NaHCO3) are found in theEocene-age (55.8–33.9 Mya)Green River Formation,Piceance Basin inColorado. 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]
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 inshale, it can be produced as a co-product ofshale oil extraction, where it is recovered by solution mining.[83]
Sodium bicarbonate, as "bicarbonate of soda", was a frequent source of punch lines forGroucho Marx inMarx Brothers movies. InDuck 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."[98] InA 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."[99]
In the Joseph L. Mankewicz classicAll 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.
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