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3D model (JSmol)
|E number||E527 (acidity regulators, ...)|
|NH4OH or NH5O|
|Molar mass||35.04 g/mol|
|Odor||"Fishy", highly pungent|
|Density||0.91 g/cm3 (25 % w/w)
0.88 g/cm3 (35 % w/w)
|Melting point||−57.5 °C (−71.5 °F; 215.7 K) (25 % w/w)
−91.5 °C (35% w/w)
|Boiling point||37.7 °C (99.9 °F; 310.8 K) (25 % w/w)|
|−31.5 ∙ 10−6 cm3/mol|
Std enthalpy of
|R-phrases (outdated)||R34, R50|
|S-phrases (outdated)||(S1/2), S26, S36/37/39, S45, S61|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Ammonia solution, also known as ammonia water, ammoniacal liquor, ammonia liquor, aqua ammonia, aqueous ammonia, or (inaccurately) ammonia, is a solution of ammonia in water. It can be denoted by the symbols NH3(aq). It is sometimes thought of as a solution of ammonium hydroxide. Although the name ammonium hydroxide suggests an alkali with composition [NH4+][OH−], it is actually impossible to isolate samples of NH4OH. The ions NH4+ and OH− do not account for a significant fraction of the total amount of ammonia except in extremely dilute solutions.
Like other gases, ammonia exhibits decreasing solubility in solvent liquids as the temperature of the solvent increases. Ammonia solutions decrease in density as the concentration of dissolved ammonia increases. At 15.6 °C (60.1 °F), the density of a saturated solution is 0.88 g/ml and contains 35% ammonia by mass, 308 g/l w/v, (308 grams of ammonia per litre of solution) and has a molarity of approximately 18 mol L−1. At higher temperatures, the molarity of the saturated solution decreases and the density increases.
Upon warming saturated solutions, ammonia gas is released. Warming sealed containers can lead to explosions.
In contrast to anhydrous ammonia, aqueous ammonia finds few non-niche uses outside of cleaning agents.
In addition to use as an ingredient in cleansers with other cleansing ingredients, ammonia in water is also sold as a cleaning agent by itself, usually labeled as simply "ammonia". It may be sold plain, lemon-scented (and typically colored yellow), or pine-scented (green). Commonly available ammonia with soap added is known as "cloudy ammonia".
In industry, aqueous ammonia can be used as a precursor to some alkyl amines, although anhydrous ammonia is usually preferred. Hexamethylenetetramine forms readily from aqueous ammonia and formaldehyde. Ethylenediamine forms from 1,2-dichloroethane and aqueous ammonia.
Ammonia is used to produce chloramine, which is used as a disinfectant. Chloramine is preferred over chlorination for its ability to remain active in stagnant water pipes longer, reducing the risk of waterborne infections.
Baking ammonia was one of the first chemical leavening agents invented. Originally harvested from grinding up deer antlers into a powder.. It is useful as a leavening agent because Ammonium carbonate is heat activated. This allows bakers to avoid yeast's long proofing time and avoiding the quick [[CO2]] dissipation of baking soda in making breads and cookies rise. It is still used to make ammonia cookies and other crisp baked goods, but its popularity has waned because of ammonia's off putting smell and concerns over its use as a food ingredient compared to modern day baking powder formulations.
Ammonia Hydroxide is a base that can be used as an acidity regulator to bring down the acid levels in food. It is classified in the United States by the Food and Drug Administration as generally recognized as safe (GRAS) when using the food grade version. Its pH control abilities make it an effective antimicrobial agent.
In furniture-making, ammonia solution was traditionally used to darken or stain wood containing tannic acid. After being sealed inside a container with the wood, fumes from the solution react with the tannic acid and iron salts naturally found in wood, creating a rich, dark stained look to the wood. This was commonly used during the arts and crafts movement in furniture- a furniture style which was primarily constructed of oak and stained using these methods.
Aqueous ammonia is used in traditional qualitative inorganic analysis as a complexant and base. Like many amines, it gives a deep blue coloration with copper(II) solutions. Ammonia solution can dissolve silver oxide residues, such as that formed from Tollens' reagent. It is often found in solutions used to clean gold, silver, and platinum jewelry, but may have negative effects on porous gem stones like opals and pearls.
When ammonia solution is mixed with dilute hydrogen peroxide in the presence of a metal ion, such as Cu2+, the peroxide will undergo rapid decomposition.