ammonium bicarbonate

Ammonium bicarbonate
IUPAC name Ammonium hydrogen carbonate
Other names Bicarbonate of ammonia, ammonium hydrogen carbonate, hartshorn, AmBic, powdered baking ammonia
Identifiers
CAS number	1066-33-7 Y
ChemSpider	13395 Y
UNII	45JP4345C9 Y
RTECS number	BO8600000
Jmol-3D images	Image 1
SMILES [O-]C(=O)O.[NH4+]
InChI InChI=1S/CH2O3.H3N/c2-1(3)4;/h(H2,2,3,4);1H3 Y Key: ATRRKUHOCOJYRX-UHFFFAOYSA-N Y InChI=1/CH2O3.H3N/c2-1(3)4;/h(H2,2,3,4);1H3 Key: ATRRKUHOCOJYRX-UHFFFAOYAW
Properties
Molecular formula	NH4HCO3
Molar mass	79.056 g/mol
Density	1.586 g/cm3
Melting point	41.9 °C, 315 K, decomp.
Solubility in water	11.9 g/100 mL (0 °C) 21.6 g/100 mL (20 °C) 36.6 g/100 mL (40 °C)
Solubility	insoluble in methanol
Hazards
MSDS	ICSC 1333
GHS pictograms	[1]
GHS hazard statements	H302[1]
GHS precautionary statements	none[1]
EU Index	Not listed
Main hazards	Decomposes to release ammonia
NFPA 704	0 2 0
Flash point	Non-flammable
Related compounds
Other anions	Ammonium carbonate
Other cations	Sodium bicarbonate Potassium bicarbonate
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

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 ammonium. It is a colourless solid that degrades readily to carbon dioxide and ammonia.

Production

Ammonium bicarbonate is produced in 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.^[2]

Ammonia gas passed into a strong aqueous solution of the sesquicarbonate (a 2:1:1 mixture of (NH₄)HCO₃, (NH₄)₂CO₃, and H₂O) and 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 commericially, 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). Iit 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.^[2]

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

Uses

Ammonium bicarbonate is used in the food industry as a raising agent 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. In China it is called edible or food-grade "smelly powder". Many baking cookbooks (especially from Scandinavian countries) may still refer to it as hartshorn or hornsalt ^[3][4] (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.^[5] 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 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.

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 plastic 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 slightly alkaline pH 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.

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, carbon dioxide is also produced:

NH₄HCO₃ + HCl → NH₄Cl + CO₂ + H₂O.

Reaction with base produces ammonia.

It reacts with sulfates of alkaline-earth metals to 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.

Safety

Ammonium bicarbonate is an irritant to the skin, eyes and respiratory system. Ammonium bicarbonate from China used to make cookies was found to be contaminated with melamine, and imports were banned in Malaysia for the 2008 Chinese milk scandal.

References

1. ^ ^{a b c} Online Sigma Catalogue , accessdate: June 8, 2011.
2. ^ ^{a b} Karl-Heinz Zapp "Ammonium Compounds" in Ullmann's Encylopedia of Industrial Chemistry 2012, Wiley-VCH, Weinheim. doi:10.1002/14356007.a02_243
3. ^ "separation of hornsalt". http://www.studenttorget.no/index.php?artikkelid=849. 
4. ^ ""separation of hornsalt" translated into English". http://www.tranexp.com:2000/InterTran?type=url&url=http%3A%2F%2Fwww.studenttorget.no%2Findex.php%3Fartikkelid%3D849&text=&from=nor&to=eng. 
5. ^ "What is hartshorn?". http://www.ochef.com/539.htm. Retrieved 2007-03-19.