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{{use dmy dates |date=April 2021}} |
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{{chembox |
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{{chembox |
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| Watchedfields = changed |
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| verifiedrevid = 443645229 |
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| verifiedrevid = 449871863 |
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| Name = Ammonium bicarbonate |
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| ImageFile = Ammonium bicarbonate.png |
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| Name = Ammonium bicarbonate |
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| ImageName = 2D model of ammonium bicarbonate |
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| ImageFile = Ammonium bicarbonate.svg |
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| ImageName = 2D model of ammonium bicarbonate |
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| ImageFileL1 = Ammonium-3D-balls.png |
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| ImageFile1 = Ammonium bicarbonate.jpg |
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| ImageNameL1 = Ball-and-stick model of the ammonium cation |
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| ImageClass = skin-invert |
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| ImageFileR1 = Bicarbonate-ion-3D-balls.png |
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| ImageFileL1 = Ammonium-3D-balls.png |
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| ImageSizeR1 = 125px |
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| ImageNameR1 = Ball-and-stick model of the bicarbonate anion |
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| ImageNameL1 = Ball-and-stick model of the ammonium cation |
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| ImageFileR1 = Bicarbonate-ion-3D-balls.png |
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| IUPACName = Ammonium hydrogen carbonate |
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| ImageNameR1 = Ball-and-stick model of the bicarbonate anion |
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| OtherNames = Bicarbonate of ammonia<br/>Hartshorn<br/>Baking ammonia |
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| IUPACName = Ammonium hydrogen carbonate |
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| Section1 = {{Chembox Identifiers |
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| OtherNames = Bicarbonate of ammonia, ammonium bicarbonate, hartshorn, AmBic, powdered baking ammonia |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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|Section1={{Chembox Identifiers |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = 45JP4345C9 |
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| UNII = 45JP4345C9 |
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| UNNumber = 3077 |
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| PubChem = 14013 |
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| InChI = 1/CH2O3.H3N/c2-1(3)4;/h(H2,2,3,4);1H3 |
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| InChI = 1/CH2O3.H3N/c2-1(3)4;/h(H2,2,3,4);1H3 |
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| SMILES = C(=O)O. |
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| SMILES = C(=O)O. |
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| StdInChIKey = ATRRKUHOCOJYRX-UHFFFAOYSA-N |
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| StdInChIKey = ATRRKUHOCOJYRX-UHFFFAOYSA-N |
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| CASNo = 1066-33-7 |
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| CASNo = 1066-33-7 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| RTECS = BO8600000 |
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| RTECS = BO8600000 |
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| EC_number = 213-911-5 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID=13395 |
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| ChemSpiderID =13395 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = NH<sub>4</sub>HCO<sub>3</sub> |
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| Formula = NH<sub>4</sub>HCO<sub>3</sub> |
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| MolarMass = 79.056 g/mol |
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| MolarMass = 79.056 g/mol |
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| Solubility = 11.9 g/100 mL (0 °C) <br> 21.6 g/100 mL (20 °C) <br> 36.6 g/100 mL (40 °C) |
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| Solubility = 11.9 g/100 mL (0 °C) <br /> 21.6 g/100 mL (20 °C) <br /> 24.8 g/100 mL (25 °C) <br />36.6 g/100 mL (40 °C) |
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| SolubleOther = insoluble in ] |
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| SolubleOther = insoluble in ] |
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| Density = 1.586 g/cm<sup>3</sup> |
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| Density = 1.586 g/cm<sup>3</sup> |
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| MeltingPt = 41.9 °C, 315 K, decomp. |
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| MeltingPtC = 41.9 |
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| MeltingPt_notes = decomposes |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| GHSPictograms = {{GHSp|GHS07}}<ref name="sigma">{{SigmaLink |
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| GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|sial|id=09830|name=Ammonium bicarbonate|accessdate=2022-02-15}}</ref> |
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| GHSSignalWord = Warning |
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| Productgroup = Fluka |
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| HPhrases = {{H-phrases|302}}<ref name="sigma" /> |
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| Productcode = 09830 |
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| PPhrases = {{P-phrases|264|270|301+312|330|501}}<ref>Pubchem</ref> |
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| Accessdate = June 8, 2011 |
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| ExternalSDS = |
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}}</ref> |
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| MainHazards = Decomposes to release ] |
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| HPhrases = {{H-phrases|302}}<ref name="sigma" /> |
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| NFPA-H = 2 |
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| PPhrases = none<!-- {{P-phrases|}} The above mentioned link to the sigma cataloque offers only the pictogram and an Hphrase --><ref name="sigma" /> |
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| NFPA-F = 0 |
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| ExternalMSDS = |
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| EUIndex = Not listed |
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| NFPA-R = 0 |
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| FlashPt = Non-flammable |
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| MainHazards = Decomposes to release ] |
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| NFPA-H = 2 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| FlashPt = Non-flammable |
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| RPhrases = |
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| SPhrases = |
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}} |
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| Section8 = {{Chembox Related |
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| OtherAnions = ] |
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| OtherCations = ]<br/>] |
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| OtherCpds = |
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}} |
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}} |
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|Section8={{Chembox Related |
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| OtherAnions = ] |
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| OtherCations = ]<br/>] |
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| OtherCompounds = |
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}} |
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'''Ammonium bicarbonate''', a ] with formula |
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NH<sub>4</sub>(C(=O)OHO), also called ''bicarbonate of ammonia'', '''ammonium hydrogen carbonate''', '''hartshorn''', '''AmBic''' or ''powdered baking ammonia'', is the ] ] of ]. |
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'''Ammonium bicarbonate''' is an ] with formula (NH<sub>4</sub>)HCO<sub>3</sub>. The compound has many names, reflecting its long history. Chemically speaking, it is the ] ] of the ] ion. It is a colourless solid that degrades readily to carbon dioxide, water and ammonia. |
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Ammonium bicarbonate is produced in the process that also leads to ]. Commercial ammonium carbonate was formerly known as ] or salt of ] and was formerly obtained by the dry distillation of nitrogenous organic matter such as hair, horn, decomposed urine, etc., but is now obtained by heating a mixture of ], or ammonium sulfate and ], to redness in ] retorts, the vapours being condensed in ]en receivers. The crude product is refined by sublimation, when it is obtained as a white fibrous mass, which consists of a mixture of hydrogen ammonium carbonate, NH<sub>4</sub>•HCO<sub>3</sub>, and ammonium carbamate, NH<sub>2</sub>COONH<sub>4</sub>, in molecular proportions; on account of its possessing this constitution it is sometimes called ammonium sesquicarbonate. It possesses a strong ammoniacal smell, and on digestion with alcohol the carbamate is dissolved and a residue of ammonium bicarbonate is left; a similar decomposition taking place when the sesquicarbonate is exposed to air. Ammonia gas passed into a strong aqueous solution of the sesquicarbonate converts it into normal ammonium carbonate, (NH<sub>4</sub>)<sub>2</sub>CO<sub>3</sub>, which can be obtained in the crystalline condition from a solution prepared at about 30 °C. This compound on exposure to air gives off ammonia and passes back to ammonium bicarbonate. |
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==Production== |
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Ammonium bicarbonate can also be formed by passing ] through a solution of the normal compound, when it is deposited as a white powder, which has no smell and is only slightly soluble in water. The ] solution of this salt liberates carbon dioxide on exposure to air or on heating, and becomes ] in reaction. The aqueous solutions of all the carbonates when boiled undergo decomposition with liberation of carbon dioxide and the substance with which the carbonate ion reacted to form the bicarbonate, in this case, ammonia: |
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Ammonium bicarbonate is produced by combining carbon dioxide and ammonia: |
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:NH<sub>4</sub>HCO<sub>3</sub> → NH<sub>3</sub> + H<sub>2</sub>O + CO<sub>2</sub>. |
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:<chem>CO2 + NH3 + H2O -> (NH4)HCO3</chem> |
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Since ammonium bicarbonate is thermally unstable, the reaction ] is kept cold, which allows the precipitation of the product as white solid. About 100,000 tons were produced in this way in 1997.<ref name=Ullmann>{{Cite book|doi=10.1002/14356007.a02_243|chapter=Ammonium Compounds|title=Ullmann's Encyclopedia of Industrial Chemistry|year=2000|last1=Zapp|first1=Karl-Heinz|last2=Wostbrock|first2=Karl-Heinz|last3=Schäfer|first3=Manfred|last4=Sato|first4=Kimihiko|last5=Seiter|first5=Herbert|last6=Zwick|first6=Werner|last7=Creutziger|first7=Ruthild|last8=Leiter|first8=Herbert|isbn=3527306730}}</ref> |
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Ammonia gas passed into a strong ] of the sesquicarbonate (a 2:1:1 mixture of (NH<sub>4</sub>)HCO<sub>3</sub>, (NH<sub>4</sub>)<sub>2</sub>CO<sub>3</sub>, and H<sub>2</sub>O) converts it into normal ammonium carbonate ((NH<sub>4</sub>)<sub>2</sub>CO<sub>3</sub>), which can be obtained in the crystalline condition from a solution prepared at about 30 °C. This compound on exposure to air gives off ammonia and reverts to ammonium bicarbonate. |
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==Properties== |
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At room temperature, ammonium bicarbonate is a white, crystalline powder with a slight odor of ammonia that can dissolve in ] to give a mildly ]ne ]. It is insoluble in ] and ]s. Ammonium bicarbonate decomposes at 36 to 60 °C into ], ], and water vapor in an ] process (as it is with many ]s) and so causes a drop in the temperature of the water. When reacted with ]s, carbon dioxide is produced, while reactions with alkalis produce ammonia. |
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===Salt of hartshorn=== |
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==Uses== |
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Compositions containing ammonium carbonate have long been known. They were once produced commercially, formerly known as ] or salt of ]. It was obtained by the ] of nitrogenous organic matter such as hair, horn, leather. In addition to ammonium bicarbonate, this material contains ] (NH<sub>4</sub>CO<sub>2</sub>NH<sub>2</sub>), and ] ((NH<sub>4</sub>)<sub>2</sub>CO<sub>3</sub>). It is sometimes called ammonium sesquicarbonate. It possesses a strong ammoniacal smell, and on digestion with alcohol, the carbamate is dissolved leaving a residue of ammonium bicarbonate.<ref name=Ullmann/> |
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Ammonium bicarbonate is used in the food industry as a ] for flat baked goods, such as cookies and crackers, and in China in steamed buns and Chinese almond cookies. It was commonly used in the home before modern day baking powder was made available to home bakers. In China it is called edible or food-grade "smelly powder". Many baking cookbooks (especially from Scandinavian countries) may still refer to it as ] or hornsalt <ref>{{cite web|url=http://www.studenttorget.no/index.php?artikkelid=849|title=separation of hornsalt}}</ref><ref>{{cite web|url=http://www.tranexp.com:2000/InterTran?type=url&url=http%3A%2F%2Fwww.studenttorget.no%2Findex.php%3Fartikkelid%3D849&text=&from=nor&to=eng|title="separation of hornsalt" translated into English}}</ref> (e.g., NO: “hjortetakksalt”, “salt of hart’s horn”) In many cases it may be substituted with baking soda or baking powder or a combination of both, depending on the recipe composition and leavening requirements.<ref>{{cite web|url=http://www.ochef.com/539.htm|title=What is hartshorn?|accessdate=2007-03-19}}</ref> Compared to baking soda or ], hartshorn has the advantage of producing more gas for the same amount of agent, and of not leaving any salty or soapy taste in the finished product, as it completely decomposes into water and gaseous products which evaporate during baking. It cannot be used for moist, bulky baked goods however, such as normal bread or cakes, since some ammonia will be trapped inside and will cause an unpleasant taste. |
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A similar decomposition takes place when the sesquicarbonate is exposed to air. |
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It is commonly used as an inexpensive nitrogen ] in China, but is now being phased out in favor of ] because of its relatively low quality and instability. This compound is used as a component in the production of fire-extinguishing compounds, pharmaceuticals, ]s, pigments, and it is also a basic fertilizer being a source of ammonia. Ammonium bicarbonate is still widely used in the plastic and rubber industry, in the manufacture of ]s, in chrome leather ], and for the synthesis of ]s.{{citation needed|date=February 2008}} |
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== Uses == |
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It is also used for buffering solutions to slightly alkaline pH during chemical purification, such as HPLC. Because it entirely decomposes to volatile compounds this allows rapid recovery of the compound of interest by ]. |
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Ammonium bicarbonate is used in the food industry as a ] for flat baked goods, such as cookies and crackers. It was commonly used in the home before modern-day ] was made available. Many baking cookbooks, especially from Scandinavian countries, may still refer to it as ] or hornsalt,<ref>{{Cite web| url=http://www.studenttorget.no/index.php?artikkelid=849 |title=Naturfag : Hornsalt øvelse |language=no |trans-title=Science: Hornsalt exercise |date=November 26, 2003 |publisher=Studenttorget.no |access-date=March 3, 2013}}</ref><ref>. studenttorget.no (in Norwegian)</ref> while it is known as "hirvensarvisuola" in Finnish, "hjortetakksalt" in Norwegian, "hjortetakssalt" in Danish, "hjorthornssalt" in Swedish, and "Hirschhornsalz" in German (lit., "salt of hart's horn"). Although there is a slight smell of ammonia during baking, this quickly dissipates, leaving no taste. It is used in, for example, Swedish "drömmar" biscuits and Danish "klejner" Christmas biscuits, and German Lebkuchen. In many cases it may be replaced with ] or baking powder, or a combination of both, depending on the recipe composition and leavening requirements.<ref>{{Cite web|url=http://www.ochef.com/539.htm|title=What is hartshorn?|access-date=2007-03-19|archive-url=https://web.archive.org/web/20070401184630/http://www.ochef.com/539.htm|archive-date=1 April 2007|url-status=dead}}</ref> Compared to baking soda or ], hartshorn has the advantage of producing more gas for the same amount of agent, and of not leaving any salty or soapy taste in the finished product, as it completely decomposes into water and gaseous products that evaporate during baking. It cannot be used for moist, bulky baked goods however, such as normal bread or cakes, since some ammonia will be trapped inside and will cause an unpleasant taste. It has been assigned ] E503 for use as a food additive in the ]. |
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It is commonly used as an inexpensive nitrogen ] in China, but is now being phased out in favor of ] for quality and stability. This compound is used as a component in the production of fire-extinguishing compounds, pharmaceuticals, ]s, pigments, and it is also a basic fertilizer, being a source of ammonia. Ammonium bicarbonate is still widely used in the plastics and rubber industry, in the manufacture of ]s, in chrome leather ], and for the synthesis of ].{{Citation needed|date=February 2008}} |
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It is also used for buffering solutions to make them slightly alkaline during chemical purification, such as ]. Because it entirely decomposes to volatile compounds, this allows rapid recovery of the compound of interest by ]. Relatedly it is also useful as an alkaline buffering agent for analytical ] as its volatility allows it to be rapidly removed automatically from the sample stream in the low pressure spray chambers used by many standard mass spectrometry detectors found at the end of typical LC-MS systems, such as ] detectors. This is critical as most mass spectrometry detectors become signal saturated or even damaged with more than a trace amount of ions entering the detector proper at any one time. This issue limits buffering agents and other additives in LC-MS buffers to either extremely trace concentrations or to fairly volatile compounds. In pH ranges from about 7 to 9, ammonium bicarbonate is one of the only options available as the primary buffering agent for most LC-MS buffers. |
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Ammonium bicarbonate is also a key component of the ] cough syrup "] and Ammonia". |
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It's also used as an attractant for catching insect such as walnut husk fly (]). |
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==Reactions== |
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==Reactions== |
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It dissolves in ] to give a mildly ]ne solution. It is insoluble in ] and ]s. |
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Ammonium bicarbonate decomposes to carbon dioxide, ], and water vapor on heating; it liberates CO2 when treated with dilute mineral acids: |
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:NH<sub>4</sub>HCO<sub>3</sub> + ] → NH<sub>4</sub>Cl + CO<sub>2</sub> + H<sub>2</sub>O. |
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Ammonium bicarbonate decomposes above about 36 °C into ], ], and water in an ] process and so causes a drop in the temperature of the water: |
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It reacts with sulfates of alkaline-earth metals precipitating out their carbonates: |
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:<chem>NH4HCO3 -> NH3 + H2O + CO2</chem> |
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:] + 2 NH<sub>4</sub>HCO<sub>3</sub> → ] + ] + ] + H<sub>2</sub>O. |
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When treated with ]s, ammonium salts are also produced: |
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:<chem>NH4HCO3 + HCl -> NH4Cl + CO2 + H2O</chem> |
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Reaction with base produces ammonia. |
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It reacts with sulfates of alkaline-earth metals precipitating their carbonates: |
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:<chem>CaSO4 + 2 NH4HCO3 -> CaCO3 + (NH4)2SO4 + CO2 + H2O</chem> |
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It also reacts with alkali metal halides, giving alkali metal bicarbonate and ammonium halide: |
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It also reacts with alkali metal halides, giving alkali metal bicarbonate and ammonium halide: |
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:<chem>NH4HCO3 + NaCl -> NH4Cl + NaHCO3</chem> |
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:NH<sub>4</sub>HCO<sub>3</sub> + ] → ] + ]; |
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:<chem>NH4HCO3 + KI -> NH4I + KHCO3</chem> |
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:NH<sub>4</sub>HCO<sub>3</sub> + ] → ] + ]; |
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:<chem>NH4HCO3 + NaBr -> NH4Br + NaHCO3</chem> |
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:NH<sub>4</sub>HCO<sub>3</sub> + ] → ] + NaHCO<sub>3</sub>. |
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==Natural occurrence== |
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The compound occurs in nature as an exceedingly rare mineral ].<ref>{{Cite web|url=https://www.mindat.org/min-3918.html|title=Teschemacherite}}</ref><ref>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> It can also be obtained from deer antlers.<ref>{{cite web |last1=Olver |first1=Lynne |author1-link=Lynne Olver |title=history notes{{mdash}}cookies, crackers & biscuits |url=http://www.foodtimeline.org/foodcookies.html#ammonia |website=] |access-date=January 6, 2021 |archive-url=https://web.archive.org/web/20120717061521/http://www.foodtimeline.org/foodcookies.html/#ammonia |archive-date=July 17, 2012 |date=June 24, 2012 |url-status=dead}}{{cbignore|bot=InternetArchiveBot}}</ref> |
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==Safety== |
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==Safety== |
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Ammonium bicarbonate is an ] to the ], ]s and ]. Ammonium bicarbonate from China used to make cookies was found to be contaminated with ], and imports banned in ] in the ]. |
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Ammonium bicarbonate is an ] to the ], ]s and ]. Short-term health effects may occur immediately or shortly after exposure to ammonium bicarbonate. Breathing ammonium bicarbonate can irritate the nose, throat and lungs causing coughing, wheezing and/or shortness of breath. Repeated exposure may cause bronchitis to develop with cough, and/or shortness of breath. Health effects can occur some time after exposure to ammonium bicarbonate and can last for months or years. |
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Where possible, operations should be enclosed and the use of local exhaust ventilation at the site of chemical release is recommended. If local exhaust ventilation or enclosure is not used, respirators are necessary. Wear protective work clothing and change clothes and wash thoroughly immediately after exposure to ammonium bicarbonate.<ref>{{cite web|last=Bicarbonate|first=Ammonium|title=Hazardous Substance Fact Sheet|url=http://nj.gov/health/eoh/rtkweb/documents/fs/0088.pdf|publisher=New Jersey Department of Health and Senior Services}}</ref> |
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Ammonium bicarbonate from China used to make cookies was found to be contaminated with ], and imports were banned in Malaysia following the ].<ref>{{cite web|url=https://www.thefreelibrary.com/Melamine+found+in+Malaysian+biscuits%2C+traced+to+China+ingredient.-a0187691670|title=Melamine found in Malaysian biscuits, traced to China ingredient.|publisher=]|via=]|date=16 October 2008|access-date=12 March 2019}}</ref> |
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==References== |
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==References== |
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{{Reflist}} |
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<references /> |
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{{Ammonium salts}} |
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{{Carbonates}} |
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{{Authority control}} |
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{{DEFAULTSORT:Ammonium Bicarbonate}} |
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{{DEFAULTSORT:Ammonium Bicarbonate}} |
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