Facts about Ammonia
Ammonia may itself diffuse across the renal tubules, combine with a hydrogen ion, and thus allow for further acid excretion.
At a later period, when sal ammoniac was obtained by distilling the hoofs and horns of oxen and neutralizing the resulting carbonate with hydrochloric acid (HCl), the name "spirit of hartshorn" was applied to ammonia.
Anhydrous ammonia must be stored under pressure or at low temperature to maintain it as a liquid.
Sulfur sticks are burnt to detect small leaks in industrial ammonia refrigeration systems.
The ammonia molecule readily undergoes nitrogen inversion at room temperature—that is, the nitrogen atom passes through the plane of symmetry of the three hydrogen atoms.
About 80 percent or more of the ammonia produced is used for fertilizing agricultural crops.
Ammonia solutions should not be mixed with halogens, as toxic and/or explosive products are formed.
Ammonia was first detected in interstellar space in 1968, based on microwave emissions from the direction of the galactic core.
The strength of ammonium hydroxide is measured in units of baume (density), with 26 degrees baume (about 30 percent ammonia by weight, at 15.5 °C) being the typical high-concentration commercial product.
The nitrogen atom in the molecule has a lone electron pair, and ammonia acts as a base.
Liver dysfunction, such as that seen in cirrhosis, may lead to elevated amounts of ammonia in the blood (hyperammonemia).
Anhydrous ammonia is classified as toxic (T) and dangerous for the environment (N).
Amides can be prepared by the reaction of ammonia with a number of carboxylic acid derivatives.
Larger quantities can be detected by warming the salts with a caustic alkali or with quicklime, when the characteristic smell of ammonia will be at once apparent.
Apart from these remarkable solutions, much of the chemistry in liquid ammonia can be classified by analogy with related reactions in aqueous solutions.
Anhydrous ammonia corrodes copper- and zinc-containing alloys, and so brass fittings should not be used for handling the gas.
In certain organisms, ammonia is produced from atmospheric nitrogen (N2) by enzymes called nitrogenases.
Ammonium compounds should never be allowed to come in contact with bases (unless an intended and contained reaction), as dangerous quantities of ammonia gas could be released.
During the 1960s, tobacco companies such as Brown & Williamson and Philip Morris began using ammonia in cigarettes.
Ammonia is one of the most extensively manufactured inorganic chemicals, used mainly for the production of fertilizers, explosives, and polymers.
The ammonia vapor from concentrated ammonia solutions is severely irritating to the eyes and the respiratory tract, and these solutions should only be handled in a fume hood.
The energy barrier to this inversion is 24.7 kJ/mol in ammonia, and the resonance frequency is 23.79 GHz, corresponding to microwave radiation of a wavelength of 1.260 cm.
Acyl chlorides are the most reactive, but the ammonia must be present in at least a twofold excess to neutralize the hydrogen chloride formed.
The addition of ammonia enhances the delivery of nicotine into the bloodstream.
Some plants rely on ammonia and other nitrogenous wastes incorporated into the soil by decaying matter.
Perfectly dry ammonia, however, will not combine with perfectly dry hydrogen chloride (a gas), as moisture is necessary to bring about the reaction.
Ammonia does not sustain combustion, and it does not burn readily unless mixed with oxygen, when it burns with a pale yellowish-green flame.
Most ammonium salts are soluble, and these salts act as acids in liquid ammonia solutions.
At high temperature and in the presence of a suitable catalyst, ammonia is decomposed into its constituent elements.
The hazards of ammonia solutions depend on the concentration: "dilute" ammonia solutions are usually 5–10 percent by weight (<5.62 mol/L); "concentrated" solutions are usually prepared at >25 percent by weight.
The maximum concentration of ammonia in water (a saturated solution) has a density of 0.880 g /cmі and is often known as '.880 Ammonia'.
Ammonia is a chemical compound of nitrogen and hydrogen, with the formula NH3.
The most important single use of ammonia is in the production of nitric acid.
Methylamine is prepared commercially by the reaction of ammonia with chloromethane, and the reaction of ammonia with 2-bromopropanoic acid has been used to prepare alanine in 70 percent yield.
Ammonia solution is also used as universal indicator that could be used to test for different gases that require a universal indicator solution to show the gases were present.
Ammonia continues to be used as a refrigerant in large industrial processes such as bulk icemaking and industrial food processing.
Liquid ammonia has a very high standard enthalpy change of vaporization (23.35 kJ/mol).
An ammine ligand bound to a metal ion is markedly more acidic than a free ammonia molecule, although deprotonation in aqueous solution is still rare.
Solutions of ammonia (5–10 percent by weight) are used as household cleaners, particularly for glass.
Given that liquid ammonia is an ionizing solvent, it can dissolve a range of ionic compounds, including many nitrates, nitrites, cyanides, and thiocyanates.
Today, the smallest refrigerators mostly use solid state peltier thermopile heat pumps rather than the ammonia absorption cycle.
Chlorine catches fire when passed into ammonia, forming nitrogen and hydrochloric acid; unless the ammonia is present in excess, the highly explosive nitrogen trichloride (NCl3) is also formed.
Today, the typical modern ammonia-producing plant first converts natural gas (that is, methane) or liquified petroleum gas (mainly propane and butane) or petroleum naphtha into gaseous hydrogen.
Ammonia reacts violently with the halogens, and causes the explosive polymerization of ethylene oxide.
The ammonia was used to produce explosives to sustain their war effort.
The relative intensity of the ammonia lines can be used to measure the temperature of the emitting medium.
The ammonia molecule has also been detected in the atmospheres of the gas giant planets, including Jupiter, along with other gases like methane, hydrogen, and helium.
Liquid ammonia will dissolve alkali metals and other electropositive metals such as calcium, strontium, barium, europium, and ytterbium.
Ammonia has continued to be used for miniature and multifuel fridges, such as in minibars and caravans.
Before the start of World War I, most ammonia was obtained by the dry distillation of nitrogenous vegetable and animal waste products, including camel dung.
A mixture of one part ammonia to nine parts air is passed over a platinum gauze catalyst at 850 °C, whereupon the ammonia is oxidized to nitric oxide.
The liver converts ammonia to urea through a series of reactions known as the urea cycle.
The European Union classification of ammonia solutions is given in the table.
Others, such as nitrogen-fixing legumes, benefit from symbiotic relationships with rhizobia that create ammonia from atmospheric nitrogen.
In 1909, Fritz Haber and Carl Bosch developed a method of producing ammonia from atmospheric nitrogen.
Gaseous ammonia was first isolated in 1774 by Joseph Priestley, who called it alkaline air.
Ammonia's thermodynamic properties made it one of the refrigerants commonly used in refrigeration units prior to the discovery of dichlorodifluoromethane in 1928, also known as Freon or R12.
Where necessary in substitutive nomenclature, IUPAC recommendations prefer the name azane to ammonia: hence chloramine would be named chloroazane in substitutive nomenclature, not chloroammonia.
Liquid ammonia is a strong ionizing solvent that can dissolve alkali metals to form colored, electrically conducting solutions.
The catalyst is essential, as the normal oxidation (or combustion) of ammonia gives dinitrogen and water: the production of nitric oxide is an example of kinetic control.
Ammonia is converted to carbamoyl phosphate by the enzyme carbamoyl phosphate synthase, and then enters the urea cycle to be either incorporated into amino acids or excreted in the urine.
Liquid ammonia is the best-known and most widely studied nonaqueous ionizing solvent.
One of the most characteristic properties of ammonia is its power of combining directly with acids to form salts.
All the ammonia contained in an aqueous solution of the gas may be expelled by boiling.
Liquid ammonia possesses strong ionizing powers (? = 22), and solutions of salts in liquid ammonia have been extensively studied.
Ammonia does not sustain combustion, and it does not burn readily unless mixed with oxygen, when it burns with a pale yellowish-green flame.
Household ammonia ranges in concentration from 5 to 10 percent ammonia by weight.
The salts produced by the action of ammonia on acids are known as the ammonium salts and all contain the ammonium ion (NH4+).