Difference between revisions of "Ammonium bicarbonate"

Revision as of 17:36, 2 November 2022

Ammonium bicarbonate

Food grade NH4HCO3
Names
IUPAC name Ammonium hydrogen carbonate
Other names AmBic Ammonium hydrogen carbonate Azanium bicarbonate Azanium hydrogen carbonate Bicarbonate of ammonia Baking soda Hartshorn Powdered baking ammonia
Identifiers
Jmol-3D images	Image
SMILES C(=O)(O)O.N
Properties
Chemical formula	CH5O3N NH4HCO3
Molar mass	79.056 g/mol
Appearance	White crystalline solid
Odor	Ammonia
Density	1.586 g/cm3
Melting point	41.9 °C (107.4 °F; 315.0 K) (with decomposition)
Boiling point	107 °C (225 °F; 380 K) (complete decomposition)
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	Reacts with acids, alkalis Insoluble in acetone, benzene, ethanol, ethers, methanol
Solubility in glycerol	10 g/100 ml
Vapor pressure	58.9 mm Hg (25.4 °C)
Hazards
Safety data sheet	Sigma-Aldrich
Flash point	Non-flammable
Related compounds
Related compounds	Ammonium carbonate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Ammonium bicarbonate or ammonium hydrogen carbonate is an inorganic compound with the chemical formula NH₄HCO₃. In older literature it may be referred to as hartshorn, as is ammonium carbonate.

Properties

Chemical

Ammonium carbonate will slowly decompose to give off ammonia, carbon dioxide and water vapors. The reaction occurs faster at higher temperatures:

NH₄HCO₃ → NH₃ + H₂O + CO₂

Ammonium carbamate is another potential by-product of decomposition.

When treated with acids, it releases carbon dioxide:

NH₄HCO₃ + HCl → NH₄Cl + H₂O + CO₂

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

NH₄HCO₃ + LiCl → NH₄Cl + LiHCO₃

NH₄HCO₃ + NaBr → NH₄Br + NaHCO₃

NH₄HCO₃ + KI → NH₄I + KHCO₃

Physical

Ammonium bicarbonate is a white salt, soluble in water, but insoluble in organic solvents like methanol, diethyl ether, hydrocarbons. It will slowly decompose over time, even at low temperatures, releasing ammonia gas, which gives the salt a strong smell. The decomposition occurs faster at high temperatures.

Availability

Ammonium bicarbonate can be bought from food stores as "smelly" baking powder, either very pure or mixed with other carbonates, such as sodium bicarbonate or magnesium carbonate. To determine if it's pure ammonium bicarbonate, take a small amount of the smelly baking powder and heat it until it decomposes. If no residue remains, then it's very pure. Sometimes this type of baking powder is referred to as simply "ammonium", usually the label name.

Preparation

Ammonium bicarbonate can be made by bubbling an excess of carbon dioxide gas through a cold solution of ammonia.

CO₂ + NH₃ + H₂O → NH₄HCO₃

Alternatively, it can be made by heating a mixture of ammonium nitrate, sodium bicarbonate or carbonate, and water in one container, and channeling the generated gases into a chilled empty container, where it will crystallize on the walls.

Projects

• Ammonium carbonate synthesis
• Generate ammonia gas
• Synthesize any other ammonium salt. Both forms of Hartshorn are very convenient precursors to all salts of ammonium.

Handling

Safety

Ammonium bicarbonate gives off ammonia fumes, which are irritating and toxic if they build up in a closed environment.

Storage

Ammonium bicarbonate is best stored in closed containers and kept in cold places. To limit the ammonia gas released, you can store the ammonium bicarbonate in a resealable bag, which in turn can be placed in a container. Avoid storing this compound near anything with copper or copper alloys, as well as the acid cabinet.

Disposal

Ammonium bicarbonate can be neutralized with any acid and safely dumped in both soil and down the drain, as it poses no danger to the environment. It can also be a very good nitrogen source for plants.

References

Relevant Sciencemadness threads

• ammonium bicarbonate manufacture
• What to do with my Ammonium Bicarbonate?