Ammonium bicarbonate

Last updated

Contents

Ammonium bicarbonate
2D model of ammonium bicarbonate Ammonium bicarbonate.svg
2D model of ammonium bicarbonate
Ammonium bicarbonate.jpg
Ball-and-stick model of the ammonium cation Ammonium-3D-balls.png
Ball-and-stick model of the ammonium cation
Ball-and-stick model of the bicarbonate anion Bicarbonate-ion-3D-balls.png
Ball-and-stick model of the bicarbonate anion
Names
IUPAC name
Ammonium hydrogen carbonate
Other names
Bicarbonate of ammonia, ammonium bicarbonate, hartshorn, AmBic, powdered baking ammonia
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.012.647 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 213-911-5
E number E503(ii) (acidity regulators, ...)
PubChem CID
RTECS number
  • BO8600000
UNII
UN number 3077
  • InChI=1S/CH2O3.H3N/c2-1(3)4;/h(H2,2,3,4);1H3 Yes check.svgY
    Key: ATRRKUHOCOJYRX-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/CH2O3.H3N/c2-1(3)4;/h(H2,2,3,4);1H3
    Key: ATRRKUHOCOJYRX-UHFFFAOYAW
  • [O-]C(=O)O.[NH4+]
Properties
NH4HCO3
Molar mass 79.056 g/mol
Density 1.586 g/cm3
Melting point 41.9 °C (107.4 °F; 315.0 K) decomposes
11.9 g/100 mL (0 °C)
21.6 g/100 mL (20 °C)
24.8 g/100 mL (25 °C)
36.6 g/100 mL (40 °C)
Solubility insoluble in methanol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Decomposes to release ammonia
GHS labelling:
GHS-pictogram-exclam.svg [1]
Warning
H302 [1]
P264, P270, P301+P312, P330, P501 [2]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Safety data sheet (SDS) ICSC 1333
Related compounds
Other anions
Ammonium carbonate
Other cations
Sodium bicarbonate
Potassium bicarbonate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)

Ammonium bicarbonate is an inorganic compound with formula (NH4)HCO3. The compound has many names, reflecting its long history. Chemically speaking, it is the bicarbonate salt of the ammonium ion. It is a colourless solid that degrades readily to carbon dioxide, water and ammonia.

Production

Ammonium bicarbonate is produced by combining carbon dioxide and ammonia:

CO2 + NH3 + H2O → (NH4)HCO3

Since ammonium bicarbonate is thermally unstable, the reaction solution is kept cold, which allows the precipitation of the product as white solid. About 100,000 tons were produced in this way in 1997. [3]

Ammonia gas passed into a strong aqueous solution of the sesquicarbonate (a 2:1:1 mixture of (NH4)HCO3, (NH4)2CO3, and H2O) converts it into normal ammonium carbonate ((NH4)2CO3), 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.

Salt of hartshorn

Compositions containing ammonium carbonate have long been known. They were once produced commercially, formerly known as sal volatile or salt of hartshorn. It was obtained by the dry distillation of nitrogenous organic matter such as hair, horn, leather. In addition to ammonium bicarbonate, this material contains ammonium carbamate (NH4CO2NH2), and ammonium carbonate ((NH4)2CO3). 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. [3]

A similar decomposition takes place when the sesquicarbonate is exposed to air.

Uses

Ammonium bicarbonate is used in the food industry as a leavening agent for flat baked goods, such as cookies and crackers. It was commonly used in the home before modern-day baking powder was made available. Many baking cookbooks, especially from Scandinavian countries, may still refer to it as hartshorn or hornsalt, [4] [5] while it is known as "hirvensarvisuola" in Finnish, "hjortetakksalt" or "hornsalt" 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 baking soda or baking powder, or a combination of both, depending on the recipe composition and leavening requirements. [6] Compared to baking soda or potash, 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 E number E503 for use as a food additive in the European Union.

It is commonly used as an inexpensive nitrogen fertilizer in China, but is now being phased out in favor of urea for quality and stability. This compound is used as a component in the production of fire-extinguishing compounds, pharmaceuticals, dyes, 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 ceramics, in chrome leather tanning, and for the synthesis of catalysts.[ citation needed ]

It is also used for buffering solutions to make them slightly alkaline during chemical purification, such as high-performance liquid chromatography. Because it entirely decomposes to volatile compounds, this allows rapid recovery of the compound of interest by freeze-drying. Relatedly it is also useful as an alkaline buffering agent for analytical LC–MS 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 electrospray ionization 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.

Ammonium bicarbonate is also a key component of the expectorant cough syrup "Senega and Ammonia".

It's also used as an attractant for catching insect such as walnut husk fly (Rhagoletis completa).

Reactions

It dissolves in water to give a mildly alkaline solution. It is insoluble in acetone and alcohols.

Ammonium bicarbonate decomposes above about 36 °C into ammonia, carbon dioxide, and water in an endothermic process and so causes a drop in the temperature of the water:

NH4HCO3 → NH3 + H2O + CO2

When treated with acids, ammonium salts are also produced:

NH4HCO3 + HCl → NH4Cl + CO2 + H2O

Reaction with base produces ammonia.

It reacts with sulfates of alkaline-earth metals precipitating their carbonates:

CaSO4 + 2 NH4HCO3 → CaCO3 + (NH4)2SO4 + CO2 + H2O

It also reacts with alkali metal halides, giving alkali metal bicarbonate and ammonium halide:

NH4HCO3 + NaCl → NH4Cl + NaHCO3
NH4HCO3 + KI → NH4I + KHCO3
NH4HCO3 + NaBr → NH4Br + NaHCO3

Natural occurrence

The compound occurs in nature as an exceedingly rare mineral teschemacherite. [7] [8] It can also be obtained from deer antlers. [9]

Safety

Ammonium bicarbonate is an irritant to the skin, eyes and respiratory system. 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.

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. [10]

Ammonium bicarbonate from China used to make cookies was found to be contaminated with melamine, and imports were banned in Malaysia following the 2008 Chinese milk scandal. [11]

Related Research Articles

<span class="mw-page-title-main">Bicarbonate</span> Polyatomic anion

In inorganic chemistry, bicarbonate is an intermediate form in the deprotonation of carbonic acid. It is a polyatomic anion with the chemical formula HCO−
3.

<span class="mw-page-title-main">Base (chemistry)</span> Type of chemical substance

In chemistry, there are three definitions in common use of the word "base": Arrhenius bases, Brønsted bases, and Lewis bases. All definitions agree that bases are substances that react with acids, as originally proposed by G.-F. Rouelle in the mid-18th century.

<span class="mw-page-title-main">Sodium bicarbonate</span> Chemical compound

Sodium bicarbonate (IUPAC name: sodium hydrogencarbonate), commonly known as baking soda 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, although it is more commonly found as a component of the mineral trona.

<span class="mw-page-title-main">Sodium carbonate</span> Chemical compound

Sodium carbonate is the inorganic compound with the formula Na2CO3 and its various hydrates. All forms are white, odourless, water-soluble salts that yield alkaline solutions in water. Historically, it was extracted from the ashes of plants grown in sodium-rich soils, and because the ashes of these sodium-rich plants were noticeably different from ashes of wood, sodium carbonate became known as "soda ash". It is produced in large quantities from sodium chloride and limestone by the Solvay process, as well as by carbonating sodium hydroxide which is made using the chloralkali process.

<span class="mw-page-title-main">Sodium nitrate</span> Chemical compound

Sodium nitrate is the chemical compound with the formula NaNO
3. This alkali metal nitrate salt is also known as Chile saltpeter to distinguish it from ordinary saltpeter, potassium nitrate. The mineral form is also known as nitratine, nitratite or soda niter.

Carbonation is the chemical reaction of carbon dioxide to give carbonates, bicarbonates, and carbonic acid. In chemistry, the term is sometimes used in place of carboxylation, which refers to the formation of carboxylic acids.

<span class="mw-page-title-main">Ammonium chloride</span> Chemical compound

Ammonium chloride is an inorganic chemical compound with the chemical formula NH4Cl, also written as [NH4]Cl. It is an ammonium salt of hydrogen chloride. It consists of ammonium cations [NH4]+ and chloride anions Cl−. It is a white crystalline salt that is highly soluble in water. Solutions of ammonium chloride are mildly acidic. In its naturally occurring mineralogic form, it is known as salammoniac. The mineral is commonly formed on burning coal dumps from condensation of coal-derived gases. It is also found around some types of volcanic vents. It is mainly used as fertilizer and a flavouring agent in some types of liquorice. It is a product of the reaction of hydrochloric acid and ammonia.

<span class="mw-page-title-main">Salammoniac</span> Halide mineral

Salammoniac, also sal ammoniac or salmiac, is a rare naturally occurring mineral composed of ammonium chloride, NH4Cl. It forms colorless, white, or yellow-brown crystals in the isometric-hexoctahedral class. It has very poor cleavage and is brittle to conchoidal fracture. It is quite soft, with a Mohs hardness of 1.5 to 2, and it has a low specific gravity of 1.5. It is water-soluble. Salammoniac is also the archaic name for the chemical compound ammonium chloride.

<span class="mw-page-title-main">Magnesium carbonate</span> Chemical compound

Magnesium carbonate, MgCO3, is an inorganic salt that is a colourless or white solid. Several hydrated and basic forms of magnesium carbonate also exist as minerals.

The Solvay process or ammonia–soda process is the major industrial process for the production of sodium carbonate (soda ash, Na2CO3). The ammonia–soda process was developed into its modern form by the Belgian chemist Ernest Solvay during the 1860s. The ingredients for this are readily available and inexpensive: salt brine (from inland sources or from the sea) and limestone (from quarries). The worldwide production of soda ash in 2005 was estimated at 42 million tonnes, which is more than six kilograms (13 lb) per year for each person on Earth. Solvay-based chemical plants now produce roughly three-quarters of this supply, with the remaining being mined from natural deposits. This method superseded the Leblanc process.

<span class="mw-page-title-main">Hartshorn</span> Antler of male red deer

Hartshorn is the antler of male red deer.

<span class="mw-page-title-main">Smelling salts</span> Ammonium carbonate used in the past to restore consciousness after fainting

Smelling salts, also known as ammonia inhalants, spirit of hartshorn or sal volatile, are chemical compounds used as stimulants to restore consciousness after fainting.

<span class="mw-page-title-main">Ammonium carbonate</span> Chemical used as leavening agent and smelling salt

Ammonium carbonate is a chemical compound with the chemical formula [NH4]2CO3. It is an ammonium salt of carbonic acid. It is composed of ammonium cations [NH4]+ and carbonate anions CO2−3. Since ammonium carbonate readily degrades to gaseous ammonia and carbon dioxide upon heating, it is used as a leavening agent and also as smelling salt. It is also known as baker's ammonia and is a predecessor to the more modern leavening agents baking soda and baking powder. It is a component of what was formerly known as sal volatile and salt of hartshorn, and produces a pungent smell when baked. It comes in the form of a white powder or block, with a molar mass of 96.09 g/mol and a density of 1.50 g/cm3. It is a strong electrolyte.

<span class="mw-page-title-main">Ammonium sulfate</span> Chemical compound

Ammonium sulfate (American English and international scientific usage; ammonium sulphate in British English); (NH4)2SO4, is an inorganic salt with a number of commercial uses. The most common use is as a soil fertilizer. It contains 21% nitrogen and 24% sulfur.

Calcium bicarbonate, also called calcium hydrogencarbonate, has the chemical formula Ca(HCO3)2. The term does not refer to a known solid compound; it exists only in aqueous solution containing calcium (Ca2+), bicarbonate (HCO−
3), and carbonate (CO2−
3) ions, together with dissolved carbon dioxide (CO2). The relative concentrations of these carbon-containing species depend on the pH; bicarbonate predominates within the range 6.36–10.25 in fresh water.

<span class="mw-page-title-main">Barium chlorate</span> Chemical compound

Barium chlorate, Ba(ClO3)2, is the barium salt of chloric acid. It is a white crystalline solid, and like all soluble barium compounds, irritant and toxic. It is sometimes used in pyrotechnics to produce a green colour. It also finds use in the production of chloric acid.

<span class="mw-page-title-main">Ammonium cyanide</span> Chemical compound

Ammonium cyanide is an unstable inorganic compound with the formula NH4CN.

<span class="mw-page-title-main">Ammonium carbamate</span> Chemical compound

Ammonium carbamate is a chemical compound with the formula [NH4][H2NCO2] consisting of ammonium cation NH+4 and carbamate anion NH2COO−. It is a white solid that is extremely soluble in water, less so in alcohol. Ammonium carbamate can be formed by the reaction of ammonia NH3 with carbon dioxide CO2, and will slowly decompose to those gases at ordinary temperatures and pressures. It is an intermediate in the industrial synthesis of urea (NH2)2CO, an important fertilizer.

<span class="mw-page-title-main">Magnesium bicarbonate</span> Chemical compound

Magnesium bicarbonate or magnesium hydrogencarbonate, Mg(HCO3)2, is the bicarbonate salt of magnesium. It can be formed through the reaction of dilute solutions of carbonic acid (such as seltzer water) and magnesium hydroxide (milk of magnesia).

<span class="mw-page-title-main">Total inorganic carbon</span> Sum of the inorganic carbon species

Total inorganic carbon is the sum of the inorganic carbon species.

References

  1. 1 2 Sigma-Aldrich Co., Ammonium bicarbonate. Retrieved on 2022-02-15.
  2. ↑ Pubchem
  3. 1 2 Zapp, Karl-Heinz; Wostbrock, Karl-Heinz; Schäfer, Manfred; Sato, Kimihiko; Seiter, Herbert; Zwick, Werner; Creutziger, Ruthild; Leiter, Herbert (2000). "Ammonium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a02_243. ISBN   3527306730.
  4. ↑ "Naturfag : Hornsalt øvelse" [Science: Hornsalt exercise] (in Norwegian). Studenttorget.no. 26 November 2003. Retrieved 3 March 2013.
  5. ↑ Naturfag : Hornsalt øvelse. studenttorget.no (in Norwegian)
  6. ↑ "What is hartshorn?". Archived from the original on 1 April 2007. Retrieved 19 March 2007.
  7. ↑ "Teschemacherite".
  8. ↑ "List of Minerals". 21 March 2011.
  9. ↑ Olver, Lynne (24 June 2012). "history notes—cookies, crackers & biscuits". The Food Timeline . Archived from the original on 17 July 2012. Retrieved 6 January 2021.
  10. ↑ Bicarbonate, Ammonium. "Hazardous Substance Fact Sheet" (PDF). New Jersey Department of Health and Senior Services.
  11. ↑ "Melamine found in Malaysian biscuits, traced to China ingredient". Kyodo News. 16 October 2008. Retrieved 12 March 2019– via The Free Library.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.