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Ammonium chloride is an inorganic chemical compound with the chemical formula , also written as . It is an ammonium salt of hydrogen chloride. It consists of ammonium cations and chloride anions . 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.

Production

It is a product of the Solvay process used to produce sodium carbonate:
:CO₂ + 2 NH₃ + 2 NaCl + H₂O → 2 NH₄Cl + Na₂CO₃

Not only is that method the principal one for the manufacture of ammonium chloride, but also it is used to minimize ammonia release in some industrial operations.

Ammonium chloride is prepared commercially by combining ammonia (NH₃) with either hydrogen chloride (gas) or hydrochloric acid (water solution):
:NH₃ + HCl → NH₄Cl

Ammonium chloride occurs naturally in volcanic regions, forming on volcanic rocks near fume-releasing vents (fumaroles). The crystals deposit directly from the gaseous state and tend to be short-lived, as they dissolve easily in water.

Reactions

Ammonium chloride appears to sublime upon heating but actually reversibly decomposes into ammonia and hydrogen chloride gas:
: NH₄Cl NH₃ + HCl

Ammonium chloride reacts with a strong base, like sodium hydroxide, to release ammonia gas:
: NH₄Cl + NaOH → NH₃ + NaCl + H₂O
Similarly, ammonium chloride also reacts with alkali-metal carbonates at elevated temperatures, giving ammonia and alkali-metal chloride:
: 2 NH₄Cl + Na₂CO₃ → 2 NaCl + CO₂ + H₂O + 2 NH₃

A solution of 5% by mass of ammonium chloride in water has a pH in the range 4.6 to 6.0.

Some reactions of ammonium chloride with other chemicals are endothermic, such as its reaction with barium hydroxide and its dissolving in water.

Applications

Agriculture

The dominant application of ammonium chloride is as a nitrogen source in fertilizers (corresponding to 90% of the world production of ammonium chloride) such as chloroammonium phosphate. The main crops fertilized this way are rice and wheat in Asia. When using ammonium chloride as a nitrogen fertilizer for plants, the appropriate concentration is applied to provide sufficient nutrients without causing harm. Ammonium chloride is approximately 26% nitrogen by weight and can be used to supply nitrogen to plants, especially those preferring slightly acidic conditions. The concentration for nitrogen fertilization in solution is between 50 and 100 milligrams of nitrogen per liter of water (mg N/L), which is equivalent to 50–100 parts per million (ppm) nitrogen, which translates to approximately 0.2 to 0.4 grams of ammonium chloride per liter of water. Ammonium chloride can acidify the soil over time, so soil pH is regularly monitored, especially when growing plants sensitive to acidic conditions. Some plants are sensitive to chloride ions (e.g., avocados, beans, grapes), so applying ammonium chloride to such plants should be done with extra caution to prevent chloride toxicity. While ammonium chloride can be beneficial as a nitrogen source, improper use can harm plants and the environment.

Ammonium chloride solutions are generally stable and can be stored for a certain period if kept under appropriate conditions, that is in airtight containers (to prevent contamination, evaporation and hydrolysis), away from light (to prevent photodegradation) and heat sources (to reduce microbial growth and chemical degradation), and if contamination is prevented. In agricultural applications the solution is used shortly after preparation, for the following reasons:
# Nutrient-rich solutions can promote the growth of microorganisms over time, so that microbial activity can alter the chemical composition of the solution, potentially reducing its efficacy as a fertilizer and introducing pathogens to plants.
# Over time, water can evaporate from the solution, especially if not stored in a tightly sealed container, which increases the concentration of ammonium chloride, and may lead to over-fertilization and potential damage to plants when applied.
# While ammonium chloride is relatively stable, prolonged storage may lead to minor changes in pH due to ongoing hydrolysis, especially if the solution is exposed to air, potentially impacting plants sensitive to acidity of the soil.
# If the water used is not distilled or deionized, dissolved minerals and impurities may precipitate over time, altering the nutrient balance of the solution.

Pyrotechnics

Ammonium chloride was used in pyrotechnics in the 18th century but was superseded by safer and less hygroscopic chemicals. Its purpose was to provide a chlorine donor to enhance the green and blue colours from copper ions in the flame.

It had a secondary use to provide white smoke, but its ready double decomposition reaction with potassium chlorate producing the highly unstable ammonium chlorate made its use very dangerous.

Metalwork

Ammonium chloride is used as a flux in preparing metals to be tin coated, galvanized or soldered. It works as a flux by cleaning the surface of workpieces by reacting with the metal oxides at the surface to form a volatile metal chloride. For that purpose, it is sold in blocks at hardware stores for use in cleaning the tip of a soldering iron, and it can also be included in solder as flux.

Medicine

Ammonium chloride is used as an expectorant in cough medicine. Its expectorant action is caused by irritative action on the bronchial mucosa, which causes the production of excess respiratory tract fluid, which presumably is easier to cough up. Ammonium salts are an irritant to the gastric mucosa and may induce nausea and vomiting.

Ammonium chloride is used as a systemic acidifying agent in treatment of severe metabolic alkalosis, in oral acid loading test to diagnose distal renal tubular acidosis, to maintain the urine at an acid pH in the treatment of some urinary-tract disorders.

Food

Ammonium chloride, under the name ''sal ammoniac'' or ''salmiak'' is used as food additive under the E number E510, working as a yeast nutrient in breadmaking and as an acidifier. It is a feed supplement for cattle and an ingredient in nutritive media for yeasts and many microorganisms.

Ammonium chloride is used in baking to give cookies a very crisp texture, to spice up dark sweets called salty liquorice (popular in the Nordic countries, Benelux and northern Germany), and in the liquor Salmiakki Koskenkorva for flavouring. In Turkey, Iran, Tajikistan, India, Pakistan and Arab countries it is called "noshader" and is used to improve the crispness of snacks such as ''samosas'' and ''jalebi''.

In the laboratory

Ammonium chloride has been used historically to produce low temperatures in cooling baths.

Ammonium chloride solutions with ammonia are used as buffer solutions including ACK (Ammonium-Chloride-Potassium) lysis buffer.

In paleontology, ammonium chloride vapor is deposited on fossils, where the substance forms a brilliant white, easily removed and fairly harmless and inert layer of tiny crystals that covers up any coloration the fossil may have, and if lighted at an angle highly enhances contrast in photographic documentation of three-dimensional specimens. The same technique is applied in archaeology to eliminate reflection on glass and similar specimens for photography.

In organic synthesis saturated NH₄Cl solution is typically used to quench reaction mixtures.

It has a lambda transition at 242.8 K and zero pressure.

Flotation

Giant squid and some other large squid species maintain neutral buoyancy in seawater through an ammonium chloride solution which is found throughout their bodies and is less dense than seawater. This differs from the method of flotation used by most fish, which involves a gas-filled swim bladder.

Batteries

Around the turn of the 20th century, ammonium chloride was used in aqueous solution as the electrolyte in Leclanché cells that found a commercial use as the "local battery" in subscribers' telephone installations. Those cells later evolved into zinc–carbon batteries still using ammonium chloride as electrolyte.

Concrete treatments

Ammonium chloride is known to be an aggressive cleaning agent.

A penetrating and intense reddish brown color is stained into concrete surfaces with a mixture of ammonium chloride and ferric chloride. Pre-treatment with acid is unnecessary.

Photography

Ammonium chloride can also be used in the process of making albumen silver prints, commonly known as albumen prints. In traditional photographic printing processes of the 19th century, ammonium chloride served as a key component in preparing the albumen solution used to coat the photographic paper. Albumen printing was the dominant photographic printing technique from the 1850s through the 1890s, prized for its fine detail and rich tonal rendition. The incorporation of ammonium chloride in the albumen solution was a significant factor in the quality and popularity of this photographic process. The process involves mixing egg whites (albumen) with ammonium chloride to create a viscous solution. This mixture is then applied as a thin layer onto paper, which, after drying, forms a smooth and glossy surface. Ammonium chloride acts as a salting agent, contributing chloride ions that are essential for forming light-sensitive silver chloride when the coated paper is subsequently sensitized with a solution of silver nitrate. Upon exposure to light, the silver chloride reduces to metallic silver, creating a visible image. The use of ammonium chloride, as opposed to sodium chloride (common salt), can influence the contrast and tonal range of the final print, often yielding warmer tones and greater image clarity.

Other applications

Ammonium chloride is used in a ~5% aqueous solution to work on oil wells with clay swelling problems. Other uses include in hair shampoo, in the glue that bonds plywood, and in cleaning products. In hair shampoo, it is used as a thickening agent in ammonium-based surfactant systems such as ammonium lauryl sulfate. Ammonium chloride is used in the textile and leather industry, in dyeing, tanning, textile printing and cotton clustering. In woodworking, a solution of ammonium chloride and water, when applied to unfinished wood, will burn when subjected to a heat gun resulting in a branding iron mark without use of a branding iron. The solution can be painted onto the wood or applied with a common rubber stamp.

History

Etymology

Pliny, in Book XXXI of his ''Natural History'', refers to a salt produced in the Roman province of Cyrenaica named ''hammoniacum'', so called because of its proximity to the nearby Temple of Jupiter Amun (Greek Ἄμμων ''Ammon''). However, the description Pliny gives of the salt does not conform to the properties of ammonium chloride. According to Herbert Hoover's commentary in his English translation of Georgius Agricola's '' De re metallica'', it is likely to have been common sea salt. Nevertheless, that salt ultimately gave ammonia and ammonium compounds their name.

Ancient China

The earliest mention of ammonium chloride was in 554 in China. At that time, ammonium chloride came from two sources: (1) the vents of underground coal fires in Central Asia, specifically, in the Tian Shan mountains (which extend from Xinjiang province of northwestern China through Kyrgyzstan) as well as in the Alay (or Alai) mountains of southwestern Kyrgyzstan, and (2) the fumaroles of the volcano Mount Taftan in southeastern Iran. (Indeed, the word for ammonium chloride in several Asian languages derives from the Iranian phrase ''anosh adur'' (immortal fire), a reference to the underground fires.) Ammonium chloride was then transported along the Silk Road eastwards to China and westwards to the Muslim lands and Europe.

Jabirian alchemists

Around 800 A.D. the Arabian chemist Jabir ibn Hayyan discovered ammonium chloride in the soot that resulted from burning camel dung, and this source became an alternative to those in Central Asia.

The Jabirian alchemists were the authors of the Jabirian corpus, tentatively dated to .This is the dating put forward by . For its acceptance by other scholars, see the references in . Notable critics of Kraus' dating are and (cf. ). The word for ammonium chloride in the Jabirian corpus was ''nošāder'', Arabian in origin. Whereas Greek alchemical texts had been almost exclusively focused on the use of mineral substances, Jabirian alchemy pioneered the use of vegetable and animal substances, and so represented an innovative shift towards 'organic chemistry'.. In the Jabirian corpus, the production of ammonium chloride from organic substances (such as plants, blood, and hair) is described. These are the oldest known instructions for deriving an inorganic compound from organic substances by chemical means.

One of the innovations in Jabirian alchemy was the addition of ammonium chloride to the category of chemical substances known as 'spirits' (i.e., strongly volatile substances). This included both naturally occurring sal ammoniac and synthetic ammonium chloride produced from organic substances. The addition of sal ammoniac to the list of 'spirits' can perhaps also be seen as a product of this new focus on organic chemistry.

Late Middle Ages

The first attested reference to ''sal ammoniac'' as ammonium chloride is in the Pseudo-Geber work ''De inventione veritatis'', where a preparation of sal ammoniac is given in the chapter ''De Salis ammoniaci præparatione'', ''sal ammoniacus (genitive: salis ammoniaci)'' being a common name in Latin of the Middle Ages for sal ammoniac.

References

Bibliography

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External links

* Calculators
surface tensions
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densities, molarities and molalities
of aqueous ammonium chloride

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Ammonium compounds
Chlorides
Edible salt
Nonmetal halides
Alchemical substances
Food additives