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Revision as of 13:50, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 476333817 of page Ammonium_chloride for the Chem/Drugbox validation project (updated: 'ChEMBL').		Latest revision as of 14:54, 24 December 2024 edit 2.145.240.61 (talk) →Jabirian alchemists: Fixed location of discoveryTags: Mobile edit Mobile web edit
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			{{Redirect2|Salmiac|Salmiak|the candy|Salty liquorice}}
	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
			{{Use dmy dates|date=November 2023}}
	{{chembox		{{chembox
	| Verifiedfields = changed		| Watchedfields = changed
	| verifiedrevid = 464362661		| verifiedrevid = 477003841
	| ImageFile = Ammonium chloride.jpg		| ImageFile = NH4Cl.png
			| ImageSize = 150px
	| ImageFile1 = NH4Cl.png
			| ImageName = Unit cell of ammonium chloride
	| ImageSize =
			| ImageFile1 = Ammoniumchlorid Kristalle.jpg
	| IUPACName = Ammonium chloride
			| ImageName1 = Crystalline ammonium chloride
	| OtherNames = Sal ammoniac, salmiac, nushadir salt, sal armagnac, salt armoniack
			| IUPACName = Ammonium chloride
	| Section1 = {{Chembox Identifiers
			| OtherNames = {{Unbulleted list|Sal ammoniac|Salmiac|Nushadir salt|Sal armagnac|Ammonium Muriate|Amchlor|Salt armoniack|Salmiak}}
	| UNII_Ref = {{fdacite|correct|FDA}}
			| Section1 = {{Chembox Identifiers
	| UNII = 01Q9PC255D
	| KEGG_Ref = {{keggcite|correct|kegg}}		|UNII_Ref = {{fdacite|correct|FDA}}
	| KEGG = D01139		|UNII = 01Q9PC255D
			|UNNumber = 3077
	| ChEMBL_Ref = {{ebicite|changed|EBI}}
			|KEGG_Ref = {{keggcite|correct|kegg}}
	| ChEMBL = <!-- blanked - oldvalue: 1200939 -->
	| InChI = 1/ClH.H3N/h1H;1H3		|KEGG = D01139
			|InChI = 1/ClH.H3N/h1H;1H3
	| ChEBI_Ref = {{ebicite|correct|EBI}}		|ChEBI_Ref = {{ebicite|correct|EBI}}
	| ChEBI = 31206		|ChEBI = 31206
	| SMILES = .		|SMILES = .
	| InChIKey = NLXLAEXVIDQMFP-UHFFFAOYAI		|InChIKey = NLXLAEXVIDQMFP-UHFFFAOYAI
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/ClH.H3N/h1H;1H3		|StdInChI = 1S/ClH.H3N/h1H;1H3
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = NLXLAEXVIDQMFP-UHFFFAOYSA-N		|StdInChIKey = NLXLAEXVIDQMFP-UHFFFAOYSA-N
	| CASNo = 12125-02-9		|CASNo = 12125-02-9
	| CASNo_Ref = {{cascite|correct|CAS}}		|CASNo_Ref = {{cascite|correct|CAS}}
	| PubChem =		|PubChem = 25517
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID=23807		|ChemSpiderID=23807
	| RTECS = BP4550000		|RTECS = BP4550000
	| EINECS = 235-186-4		|EINECS = 235-186-4
	| ATCCode_prefix = B05
	| ATCCode_suffix = XA04
	| ATC_Supplemental = {{ATC|G04|BA01}}
	}}
	| Section2 = {{Chembox Properties
	| Formula = NH<sub>4</sub>Cl
	| MolarMass = 53.491 g/mol
	| Appearance = White solid <br> ]
	| Odor = odorless
	| Density = 1.5274 g/cm<sup>3</sup>
	| MeltingPt = 338 °C (decomposes)
	| Solubility = 297 g/L (0 °C) <br> 372 g/L (20 °C) <br> 773 g/L (100 °C)
	| SolubleOther = 6 g/L (19 °C)
	| Solvent = alcohol
	| RefractIndex = 1.642
	| pKa = 9.245
	}}
	| Section3 = {{Chembox Thermochemistry
	| DeltaHf = −314.55 kJ/mol<ref name="NIST">Solid state data from {{nist|name=Ammonium chloride |id=C12125029 |accessdate=2008-10-22 |mask=1F |units=SI}}</ref>
	| Entropy = 94.85 J&thinsp;K<sup>−1</sup>&thinsp;mol<sup>−1</sup> <ref name="NIST" />
	}}
	| Section4 = {{Chembox Hazards
	| GHSPictograms = {{GHSp|GHS07}}<ref name="sigma">{{SigmaLink
	| Productgroup = Fluka
	| Productcode = 09718
	| Accessdate = June 16, 2011
	}}</ref>
	| HPhrases = {{H-phrases|302|319}}<ref name="sigma" />
	| PPhrases = {{P-phrases|305+351+338}}<ref name="sigma" />
	| ExternalMSDS =
	| EUClass = Harmful ('''Xn''')<br/>Irritant ('''Xi''')
	| EUIndex = 017-014-00-8
	| RPhrases = {{R22}}, {{R36}}
	| SPhrases = {{S2}}, {{S22}}
	| NFPA-H = 1
	| NFPA-F = 0
	| NFPA-R = 0
	| NFPA-O =
	| FlashPt = Non-flammable
	| LD50 = 1650 mg/kg, oral (rat)
	}}
	| Section8 = {{Chembox Related
	| OtherAnions = ]<br/>]<br/>]
	| OtherCations = ]<br/>]<br/>]
	}}
	}}		}}
			| Section2 = {{Chembox Properties
			|N=1 | H=4 | Cl=1
			|Appearance = White or colorless crystalline solid, ]
			|Odor = Odorless
			|Density = 1.519 g/cm<sup>3</sup><ref name=b92>{{RubberBible92nd|page=4.46}}</ref>
			|SublimationConditions = Decomposes at 337.6&nbsp;°C at 1&nbsp;atm<ref name=chemister /><br> Δ<sub>decomp</sub>''H''<sup><s>o</s></sup> = 176.1 kJ/mol<ref name = "Wiberg&Holleman"/>
			|Solubility = 244 g/L (−15 °C)<br> 294 g/L (0 °C)<br> 383.0 g/L (25 °C)<br> 454.4 g/L (40 °C)<br> 740.8 g/L (100 °C)<ref name=sioc>{{cite book |last1 = Seidell |first1 = Atherton |last2 = Linke |first2 = William F. |year = 1919 |title = Solubilities of Inorganic and Organic Compounds |publisher = D. van Nostrand Company |edition = 2nd}}<br> Results here are multiplied by water's density at temperature of solution for unit conversion.</ref>
			|Solubility1 = 32 g/kg (17 °C)<br> 33.5 g/kg (19 °C)<br> 35.4 g/kg (25 °C)<ref name=chemister> {{Webarchive|url=https://web.archive.org/web/20150723041321/http://chemister.ru/Database/properties-en.php?dbid=1&id=371 |date=23 July 2015 }}. Chemister.ru (2007-03-19). Retrieved on 2018-01-23.</ref>
			|Solvent1 = methanol
			|Solubility2 = 6 g/L (19 °C)<ref name=pphoic>{{cite book|last = Pradyot|first = Patnaik|year = 2003|title = Handbook of Inorganic Chemicals|publisher = The McGraw-Hill Companies, Inc.|isbn = 978-0-07-049439-8}}</ref>
			|Solvent2 = ethanol
			|Solubility3 = 97 g/kg<ref name=chemister />
			|Solvent3 = glycerol
			|Solubility4 = 0.09 g/kg (0 °C)<br> 0.031 g/kg (25 °C)<ref name=chemister />
			|Solvent4 = sulfur dioxide
			|Solubility5 = 0.67 g/kg (16.6 °C)<ref name=chemister />
			|Solvent5 = acetic acid
			|SolubleOther = Soluble in liquid ], ], <br> Slightly soluble in ]<br> Insoluble in ], ]<ref name=chemister />
			|RefractIndex = 1.642 (20 °C)<ref name=chemister />
			|pKa = 9.24
			|VaporPressure = 133.3 Pa (160.4 °C)<ref name="sigma" /><br> 6.5 kPa (250 °C)<br> 33.5 kPa (300 °C)<ref name=pphoic />
			|SolubilityProduct = 30.9 (395 g/L)<ref name=slm>{{cite web|url = http://www.saltlakemetals.com/SolubilityProducts.htm|title = Solubility Products of Selected Compounds|publisher = Salt Lake Metals|access-date = 2014-06-11|archive-date = 21 October 2015|archive-url = https://web.archive.org/web/20151021103642/http://www.saltlakemetals.com/SolubilityProducts.htm|url-status = live}}</ref>
			|MagSus = -36.7·10<sup>−6</sup> cm<sup>3</sup>/mol<ref>{{RubberBible92nd|page=4.131}}</ref>
			| MeltingPt={{convert|338|C|F}}
			}}
			| Section3 = {{Chembox Structure
			|CrystalStruct = ], ]<ref>{{cite journal|doi=10.1016/0038-1098(93)90362-Q|title=Phase transition temperatures and thermal hysteresis in NH<sub>4</sub>Cl<sub>1−x</sub>Br<sub>x</sub> (x≤0.05) crystals determined through charge transfer spectra of Cu<sup>2+</sup>(II) centres|journal=Solid State Communications|volume=85|issue=2|pages=135|year=1993|last1=Breñosa|first1=A.G|last2=Rodríguez|first2=F|last3=Moreno|first3=M|bibcode=1993SSCom..85..135B}}</ref>
			|SpaceGroup = Pm{{overline|3}}m, No. 221
			|LattConst_a = 0.3876 nm
			|UnitCellFormulas = 1
			}}
			| Section4 = {{Chembox Thermochemistry
			|DeltaHf = −314.43 kJ/mol<ref name=pphoic />
			|Entropy = 94.56 J/mol·K<ref name=pphoic />
			|DeltaGf = −202.97 kJ/mol<ref name=pphoic />
			|HeatCapacity = 84.1 J/mol·K<ref name=pphoic />
			}}
			| Section5 = {{Chembox Pharmacology
			|ATCCode_prefix = B05
			|ATCCode_suffix = XA04
			|ATC_Supplemental = {{ATC|G04|BA01}}
			}}
			| Section6 = {{Chembox Hazards
			|ExternalSDS =
			|GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=326372|name=Ammonium chloride|accessdate=2014-06-11}}</ref>
			|GHSSignalWord = Warning
			|HPhrases = {{H-phrases|302|319}}<ref name="sigma" />
			|PPhrases = {{P-phrases|305+351+338}}<ref name="sigma" />
			|NFPA-H = 2
			|NFPA-F = 0
			|NFPA-R = 0
			|FlashPt = Non-flammable
			|LD50 = 1650 mg/kg (rats, oral)
			|PEL = none<ref name=NIOSH>{{PGCH|0029}}</ref>
			|REL = TWA 10 mg/m<sup>3</sup> ST 20 mg/m<sup>3</sup> (as fume)<ref name=NIOSH/>
			|IDLH = N.D.<ref name=NIOSH/>
			}}
			| Section7 = {{Chembox Related
			|OtherAnions = ]<br> ]<br> ]
			|OtherCations = ]<br> ]<br> ]
			}}
			}}
			'''Ammonium chloride''' is an ] with the ] {{chem2|NH4Cl|auto=1}}, also written as {{chem2|Cl}}. It is an ] salt of ]. It consists of ammonium ] {{chem2|+}} and ] ] {{chem2|Cl−}}. It is a white crystalline ] that is highly soluble in water. Solutions of ammonium chloride are mildly acidic. In its naturally occurring mineralogic form, it is known as ]. The mineral is commonly formed on burning ] 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 ] of ]. It is a product of the reaction of ] and ].
			==Production==
			]
			It is a product of the ] used to produce ]:<ref name = "Wiberg&Holleman">{{cite book|first1 = Egon|last1 = Wiberg|first2 = Nils|last2 = Wiberg|year = 2001|title = Inorganic Chemistry|url = https://books.google.com/books?id=vEwj1WZKThEC&pg=PA614|publisher = Academic Press|isbn = 978-0-12-352651-9|page = 614|edition = illustrated|access-date = 2 November 2016|archive-date = 21 December 2016|archive-url = https://web.archive.org/web/20161221235956/https://books.google.com/books?id=vEwj1WZKThEC&pg=PA614|url-status = live}}</ref>
			:CO<sub>2</sub> + 2 NH<sub>3</sub> + 2 NaCl + H<sub>2</sub>O → 2 NH<sub>4</sub>Cl + Na<sub>2</sub>CO<sub>3</sub>
			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 ] (NH<sub>3</sub>) with either ] (gas) or ] (water solution):<ref name = "Wiberg&Holleman"/>
			:NH<sub>3</sub> + HCl → NH<sub>4</sub>Cl
			Ammonium chloride occurs naturally in ] regions, forming on volcanic rocks near fume-releasing vents (]s). The crystals deposit directly from the gaseous state and tend to be short-lived, as they dissolve easily in water.<ref name=Rowley>{{Cite book|title=General Chemistry I Laboratory Manual|edition=Second|last=Rowley|first=Steven P.|publisher=Kendall Hunt|year=2011|isbn=978-0-7575-8942-3}}</ref>
			==Reactions==
			]
			Ammonium chloride appears to ] upon heating but actually reversibly ] into ] and ] gas:<ref name = "Wiberg&Holleman"/>
			: NH<sub>4</sub>Cl {{eqm}} NH<sub>3</sub> + HCl
			Ammonium chloride reacts with a strong base, like ], to release ammonia gas:
			: NH<sub>4</sub>Cl + NaOH → NH<sub>3</sub> + NaCl + H<sub>2</sub>O
			Similarly, ammonium chloride also reacts with alkali-metal carbonates at elevated temperatures, giving ammonia and alkali-metal chloride:
			: 2 NH<sub>4</sub>Cl + Na<sub>2</sub>CO<sub>3</sub> → 2 NaCl + CO<sub>2</sub> + H<sub>2</sub>O + 2 NH<sub>3</sub>
			A solution of 5% by mass of ammonium chloride in water has a ] in the range 4.6 to 6.0.<ref>{{cite book |author=Bothara, K. G. |title=Inorganic Pharmaceutical Chemistry |url=https://books.google.com/books?id=vOtFj8b7P9MC&pg=SA13-PA7 |date=2008 |publisher=Pragati Books Pvt. Ltd. |isbn=978-81-85790-05-3 |pages=13– |access-date=2 November 2016 |archive-date=22 December 2016 |archive-url=https://web.archive.org/web/20161222001036/https://books.google.com/books?id=vOtFj8b7P9MC&pg=SA13-PA7 |url-status=live}}</ref>
			Some reactions of ammonium chloride with other chemicals are ], such as its reaction with ] and its dissolving in water.
			==Applications==
			===Agriculture===
			]
			The dominant application of ammonium chloride is as a ] source in ]s (corresponding to 90% of the world production of ammonium chloride) such as chloroammonium phosphate.<ref>{{cite book |last1=Kishi |first1=Atsushi |chapter=Ammonium Compounds |title=Ullmann's Encyclopedia of Industrial Chemistry |edition=7th |publisher=Wiley-VCH |year=2012 |doi=10.1002/14356007.a02_161.pub3 |pages=1–6|doi-broken-date=2024-11-24 }}</ref> The main ]s fertilized this way are ] and ] in ].<ref>Zapp, Karl-Heinz (2012) "Ammonium Compounds" in ''Ullmann's Encyclopedia of Industrial Chemistry''. Wiley-VCH, Weinheim. {{doi|10.1002/14356007.a02_243}}</ref><ref>{{cite journal |last1=Sanjuan |first1=Juan |last2=Ventura |first2=Yamini |last3=Wenkert |first3=Derek |title=Ammonium Chloride as a Nitrogen Source in Asian Agriculture: Effects on Rice and Wheat Production |journal=Journal of Plant Nutrition |volume=35 |issue=8 |year=2012 |pages=1234–1245 |doi=10.1080/01904167.2012.686993|doi-broken-date=2024-11-24 }}</ref> When using ammonium chloride as a nitrogen fertilizer for plants, the appropriate concentration is applied to provide sufficient nutrients without causing harm.<ref>{{cite book |last1=Havlin |first1=John L. |last2=Beaton |first2=James D. |last3=Tisdale |first3=Samuel L. |last4=Nelson |first4=Werner L. |title=Soil Fertility and Fertilizers: An Introduction to Nutrient Management |edition=7th |publisher=Prentice Hall |year=2005 |isbn=978-0130278241 |pages=146–148 |chapter=Nitrogen Fertilizers}}</ref> Ammonium chloride is approximately 26% nitrogen by weight and can be used to supply nitrogen to plants, especially those preferring slightly acidic conditions.<ref>{{cite book |last1=Brady |first1=Nyle C. |last2=Weil |first2=Ray R. |title=The Nature and Properties of Soils |edition=15th |publisher=Pearson Education |year=2016 |isbn=978-0133254488 |pages=594–595 |chapter=Nitrogen and Sulfur |url=https://www.pearson.com/us/higher-education/program/Brady-Nature-and-Properties-of-Soils-The-15th-Edition/PGM203380.html}}</ref> 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.<ref>{{cite book |last1=Jones |first1=J. Benton Jr. |title=Hydroponics: A Practical Guide for the Soilless Grower |edition=2nd |publisher=CRC Press |year=2005 |isbn=978-0849331671 |pages=181–183 |chapter=Formulating Hydroponic Nutrient Solutions}}</ref> Ammonium chloride can acidify the soil over time, so soil pH is regularly monitored, especially when growing plants sensitive to acidic conditions.<ref>{{cite journal |last1=Fageria |first1=N. K. |title=Influence of Nitrogen Sources on Soil Acidity Under Common Bean |journal=Scientia Agricola |volume=64 |issue=5 |year=2007 |pages=583–587 |doi=10.1590/S0103-90162007000500011}}</ref> 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.<ref>{{cite journal |last1=White |first1=Philip J. |title=Chloride in soils and its uptake and movement within the plant: A review |journal=Annals of Botany |volume=88 |issue=6 |year=2001 |pages=967–988 |doi=10.1006/anbo.2001.1540|bibcode=2001AnBot..88..967W }}</ref> While ammonium chloride can be beneficial as a nitrogen source, improper use can harm plants and the environment.<ref>{{cite journal |last1=Goulding |first1=Keith W. T. |title=Nitrate leaching from arable and horticultural land |journal=Soil Use and Management |volume=16 |issue=4 |year=2000 |pages=145–151 |doi=10.1111/j.1475-2743.2000.tb00189.x}}</ref>
			Ammonium chloride solutions are generally stable and can be stored for a certain period if kept under appropriate conditions,<ref name="merck">{{cite book |editor-last1=Windholz |editor-first1=Martha |title=The Merck Index: An Encyclopedia of Chemicals, Drugs, and Biologicals |edition=10th |publisher=Merck & Co. |year=1983 |isbn=9780911910278 |page=71 |entry=Ammonium Chloride |url=https://www.powerpak.com/courses/107888/107888_sample.pdf}}</ref> that is in airtight containers (to prevent contamination, evaporation and hydrolysis), away from light (to prevent ]) and heat sources (to reduce microbial growth and chemical degradation), and if contamination is prevented.<ref name="merck"/> In agricultural applications the solution us used shortly after preparation,<ref>{{cite journal |last1=Shaviv |first1=Avner |last2=Johnson |first2=Craig M. |title=Controlled Release Fertilizers to Increase Efficiency of Nitrogen Use in Agricultural Systems |journal=Fertilizer Research |volume=3 |issue=1 |year=1982 |pages=263–279 |doi=10.1007/BF01063471|pmid=67590 }}</ref> 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.<ref>{{cite journal |last1=Jiao |first1=Wei |last2=Zhou |first2=Wei |last3=Tan |first3=Dongxu |title=Effects of Nitrogen Fertilization on Soil Microbial Biomass and Community Structure with Ammonium Chloride Application |journal=Frontiers in Microbiology |volume=10 |year=2019 |page=2449 |doi=10.3389/fmicb.2019.02528 |doi-access=free |pmid=31736838|pmc=6834691 }}</ref>
			# 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.<ref>{{cite journal |last1=Guertal |first1=Elizabeth A. |title=Avoiding Fertilizer Burn in Plants |journal=Crop, Soil and Environmental News |publisher=Virginia Cooperative Extension |year=2000 |url=https://vtechworks.lib.vt.edu/bitstream/handle/10919/48303/424-036.pdf}}</ref>
			# While ammonium chloride is relatively stable, prolonged storage may lead to minor changes in ] due to ongoing hydrolysis, especially if the solution is exposed to air, potentially impacting plants sensitive to acidity of the soil.<ref>{{cite book |last1=Marschner |first1=Petra |title=Marschner's Mineral Nutrition of Higher Plants |edition=3rd |publisher=Academic Press |year=2012 |isbn=978-0-12-384905-2 |pages=597–598 |chapter=Functions of Fertilizer Nutrients}}</ref>
			# If the water used is not distilled or deionized, dissolved minerals and impurities may precipitate over time, altering the nutrient balance of the solution.<ref>{{cite book |last1=Jones |first1=J. Benton Jr. |title=Hydroponics: A Practical Guide for the Soilless Grower |edition=2nd |publisher=CRC Press |year=2005 |isbn=978-0-8493-3167-1 |pages=181–183 |chapter=Formulating Hydroponic Nutrient Solutions}}</ref>
			===Pyrotechnics===
			Ammonium chloride was used in ] in the 18th century but was superseded by safer and less ] 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 ] reaction with ] producing the highly unstable ] made its use very dangerous.<ref>{{cite book |title=Chemistry of Pyrotechnics |author=Conkling, John A. |author2=Mocella, Christopher J. |edition=2nd |publisher=CRC Press |year=2010 |isbn=978-1574447408}}</ref><ref>{{cite book |title=Chemistry of Powder and Explosives |author=Davis, Tenney L |publisher=Angriff Press |year=2012 |isbn=978-0945001171}}</ref><ref>{{cite book |title=Encyclopedic Dictionary of Pyrotechnics (and Related Subjects) |author=Kosanke, K. L. |author2=Kosanke, B. J. |author3=Sturman, Barry T. |author4=Winokur, Robert M. |publisher=Journal of Pyrotechnics |year=2012 |isbn=978-1889526195}}</ref>
			===Metalwork===
			Ammonium chloride is used as a ] 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 ] 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 ] agent in treatment of severe metabolic ], in oral acid loading test to diagnose distal renal tubular acidosis, to maintain the ] at an acid pH in the treatment of some urinary-tract disorders.{{Citation needed|date=August 2017}}
			===Food===
			Ammonium chloride, under the name '']'' or ''salmiak'' is used as ] under the ] E510, working as a yeast nutrient in breadmaking and as an acidifier.<ref>{{cite book|last1=Smith|first1=Jim|last2=Hong-Shum|first2=Lily|title=Food Additives Data Book|date=2011|publisher=John Wiley & Sons|isbn=978-1444397734|page=540|edition=2nd}}</ref> It is a feed supplement for cattle and an ingredient in nutritive media for yeasts and many microorganisms.
			Ammonium chloride is used to spice up dark sweets called ] (popular in the Nordic countries, ] and northern Germany),<ref>{{cite web |url=http://www.thecrimson.com/column/summer-postcards/article/2011/8/8/salmiak-taste-people-available/ |title=In Salmiak Territory |author=Christine S. |work=] |date=8 August 2011 |access-date=8 August 2017 |archive-date=12 September 2017 |archive-url=https://web.archive.org/web/20170912111330/http://www.thecrimson.com/column/summer-postcards/article/2011/8/8/salmiak-taste-people-available/ |url-status=live }}</ref> in baking to give cookies a very crisp texture, and in the liquor ] 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 ] and '']''.
			===In the laboratory===
			Ammonium chloride has been used historically to produce low temperatures in ]s.<ref>{{cite journal|title=A New Frigorifick Experiment Shewing, How a Considerable Degree of Cold May be Suddenly Produced without the Help of Snow, Ice, Haile, Wind, or Niter, and That at Any Time of the Year|journal=Philosophical Transactions|date=18 July 1666|volume=1|issue=15|pages=255–261|url=https://archive.org/details/philtrans01311687|doi=10.1098/rstl.1665.0106 |doi-access=free}}</ref> <!--- sodium chloride For example, the zero point of the Fahrenheit temperature scale is determined by placing the thermometer in a mixture of ice, water, and ammonium chloride.--->
			Ammonium chloride solutions with ] are used as ]s including ACK (Ammonium-Chloride-Potassium) ].<ref> {{Webarchive|url=https://web.archive.org/web/20200811190240/http://cshprotocols.cshlp.org/content/2014/11/pdb.rec083295.short |date=11 August 2020 }}. Cshprotocols.cshlp.org (2014-11-01). Retrieved on 2018-01-23.</ref>
			In ], ammonium chloride vapor is ] on ]s, 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.<ref>{{cite journal |url=http://jpaleontol.geoscienceworld.org/content/49/3/565.short |title=New techniques for coating paleontological specimens prior to photography |journal=Journal of Paleontology |year=1975 |volume=49 |issue=3 |pages=565–566 |author=Marsh, L. F. and Marsh, R. C. |access-date=17 December 2012 |archive-date=16 April 2016 |archive-url=https://web.archive.org/web/20160416161037/http://jpaleontol.geoscienceworld.org/content/49/3/565.short |url-status=live }}</ref> The same technique is applied in ] to eliminate reflection on glass and similar specimens for photography.<ref> {{Webarchive|url=https://web.archive.org/web/20130516152933/http://www.bcin.ca/Interface/openbcin.cgi?submit=submit&Chinkey=61221 |date=16 May 2013 }}. Bcin.ca (2017-08-01). Retrieved on 2018-01-23.</ref>
			In organic synthesis saturated NH<sub>4</sub>Cl solution is typically used to quench reaction mixtures.<ref>{{cite journal|journal=Org. Synth.|year=2015|volume=92|pages=309–319|title=(S)-1,1-Diphenylprolinol Trimethylsilyl Ether|author1=Robert K. Boeckman, Jr. |author2=Douglas J. Tusch |author3=Kyle F. Biegasiewicz|doi=10.15227/orgsyn.092.0309|doi-access=free}}</ref>
			It has a ] at 242.8 K and zero pressure.<ref>{{Cite journal |last=Pippard |first=A. B. |date=May 1956 |title=XLVIII. Thermodynamic relations applicable near a lambda-transition |url=http://dx.doi.org/10.1080/14786435608238127 |journal=Philosophical Magazine |volume=1 |issue=5 |pages=473–476 |doi=10.1080/14786435608238127 |bibcode=1956PMag....1..473P |issn=0031-8086}}</ref>
			===Flotation===
			] and some other large squid species maintain neutral ] in ] through an ammonium chloride solution which is found throughout their bodies and is less dense than seawater.<ref>{{Cite journal|url = https://www.jstor.org/stable/75757|jstor = 75757|title = A Buoyancy Mechanism Found in Cranchid Squid|last1 = Denton|first1 = E. J.|last2 = Gilpin-Brown|first2 = J. B.|last3 = Shaw|first3 = T. I.|journal = Proceedings of the Royal Society of London. Series B, Biological Sciences|year = 1969|volume = 174|issue = 1036|pages = 271–279|doi = 10.1098/rspb.1969.0093|bibcode = 1969RSPSB.174..271D|s2cid = 94534922|access-date = 27 December 2020|archive-date = 22 April 2021|archive-url = https://web.archive.org/web/20210422050824/https://www.jstor.org/stable/75757|url-status = live}}</ref> This differs from the method of flotation used by most fish, which involves a gas-filled ].
			===Batteries===
			Around the turn of the 20th century, ammonium chloride was used in aqueous solution as the electrolyte in ]s that found a commercial use as the "local battery" in subscribers' telephone installations. Those cells later evolved into ] 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 ].<ref>{{cite web |last1=Swift |first1=Ernest H. |title=Process for staining concrete |url=https://patents.google.com/patent/US2379502A/en |website=Google Patents |access-date=8 October 2023 |archive-date=26 November 2020 |archive-url=https://web.archive.org/web/20201126220730/https://patents.google.com/patent/US2379502A/en |url-status=live }}</ref> Pre-treatment with acid is unnecessary.
			===Photography===
			{{main article|Albumen print}}
			Ammonium chloride can also be used in the process of making albumen silver prints, commonly known as ]s. 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.<ref>{{cite book |last=Eder |first=Josef Maria |title=History of Photography |publisher=Dover Publications |year=1978 |pages=338–342 |isbn=978-0486235868}}</ref> 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.<ref>{{cite book |last=Reilly |first=James M. |title=The Albumen & Salted Paper Book: The History and Practice of Photographic Printing, 1840–1895 |publisher=Light Impressions Corporation |year=1980 |isbn=978-1933360782 |pages=28–35}}</ref> 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.<ref>{{cite journal |last=Ware |first=Mike |title=Mechanisms of Image Deterioration in Early Photographs |journal=Science Museum |year=1994 |pages=15–18 |url=http://www.mikeware.co.uk/downloads/Mechanisms_of_Image_Deterioration.pdf}}</ref> 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.<ref>{{cite book |last1=Towler |first1=John |title=The Silver Sunbeam: A Practical and Theoretical Text-book on Sun Drawing and Photographic Printing |publisher=Joseph H. Ladd |year=1864 |pages=88–90 |url=https://archive.org/details/silversunbeampr00towlgoog }}</ref>
			===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 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.<ref>{{Cite AV media|url=https://www.youtube.com/watch?v=3K4J7yn7ga0 | archive-url=https://ghostarchive.org/varchive/youtube/20211117/3K4J7yn7ga0| archive-date=2021-11-17 | url-status=live|title=Shop Tips #1 // Wood Branding without a Branding Iron |author=] |via=YouTube |date=2017-06-11 |access-date=2018-01-23}}{{cbignore}}</ref>
			== History ==
			=== Etymology ===
			], in Book XXXI of his '']'', refers to a salt produced in the Roman province of ] named ''hammoniacum'', so called because of its proximity to the nearby Temple of ] (] Ἄμμων ''Ammon'').<ref>{{Cite web |title=Pliny the Elder, The Natural History, Book XXXI, Chapter 39. (7.) - The various kinds of salt; the methods of preparing it, and the remedies derived from it. |url=https://www.perseus.tufts.edu/hopper/text?doc=urn:cts:latinLit:phi0978.phi001.perseus-eng1:31.39 |access-date=22 August 2024 |archive-date=9 July 2023 |archive-url=https://web.archive.org/web/20230709210136/http://www.perseus.tufts.edu/hopper/text?doc=urn:cts:latinLit:phi0978.phi001.perseus-eng1:31.39 |url-status=live }}</ref><ref>{{Cite journal |last=Stapleton |first=H. E. |date=1905 |title=Sal-Ammoniac: A Study in Primitive Chemistry |url=http://n2t.net/ark:/13960/t1vf25m9j |journal=Memoirs of the Asiatic Society of Bengal |volume=1 |issue=4 |pages=25--42, i--iii |via=Archive.org}}</ref> However, the description Pliny gives of the salt does not conform to the properties of ammonium chloride. According to ] commentary in his English translation of ] '']'', it is likely to have been common sea salt.<ref>{{Cite book |last=Hoover |first=Herbert |title=Georgius Agricola De Re Metallica - Translated from the first Latin edition of 1556 |publisher=Dover Publications |year=1950 |isbn=978-0486600062 |location=New York |pages=560}}</ref> Nevertheless, that salt ultimately gave ] and ] compounds their name.
			=== Ancient China ===
			The earliest mention of ammonium chloride was in 554 in China.<ref>That ammonium chloride was imported into China from ]na in Central Asia is mentioned in the ''Wei shu'' (History of the ] ), which was compiled by ] 魏收 (506–572). (Sutton et al., 2008), p. 596. However, it may have been imported into China even before 150: there is a brief mention of what might have been ammonium chloride in the Chinese ] 周易参同契註 (142) by ]. ], p. 439.</ref> At that time, ammonium chloride came from two sources: (1) the vents of underground coal fires in Central Asia, specifically, in the ] mountains (which extend from ] province of northwestern China through ]) as well as in the ] mountains of southwestern Kyrgyzstan, and (2) the ]s of the volcano ] in southeastern ].<ref>The locations of the sources of ammonium chloride in the burning coal deposits of Central Asia are shown on the following map:
			*], pp. 595-596, especially Fig. 6 (map).
			Ammonium chloride was also found in burning coal deposits in Europe.
			*Jameson, Robert, ''Manual of Mineralogy'' … (Edinburgh, Scotland: Archibald Constable & Co. and Hurst, Robinson & Co., 1821), p. 12. "'''Volcanic Sal Ammoniac.''' … ''Geographic Situation''.—It occurs in the vicinity of burning beds of coal, both in Scotland and England; and in many volcanic districts in different parts of the world."
			*Nicol, James, ''Manual of Mineralogy;'' … (Edinburgh, Scotland: Adam and Charles Black and Longman, Brown, Green, and Longmans, 1849). "It is sometimes found near ignited coal seams, as at St Etienne in France, near Newcastle, and in Scotland."
			*], pp. 213–214: "Chloride of ammonium is also found at other places, as a sublimate arising from the combustion of coal strata; for instance, at St. Etienne, near Lyons, at Newcastle and at Glan in Rhenish Bavaria."
			*les Élèves mineurs de Saint-Étienne (1822) {{Webarchive|url=https://web.archive.org/web/20201017042026/https://babel.hathitrust.org/cgi/pt?id=iau.31858046217810;view=1up;seq=162 |date=17 October 2020 }} (Note on the ammonium salt that a burning coal mine produces), ''Annales de Chimie et de Physique'', '''21''' : 158–159. </ref><ref>The Arab geographer ] (1179–1229) or "Jakut" mentioned that ammonium chloride was harvested from "Damindan" (Tamindan), a valley on the volcano Mount Taftan in southwestern Iran. See: von Lippmann, E.O., "Wan and wofür erscheint zuerst die Bezeichnung Ammoniak?" (When and why did the term "ammonia" first appear?) In: Lippmann, Edmund O., ed., ''Abhandlungen und Vorträge zur Geschichte der Naturwissenschaften'' (Essays and Lectures on the History of the Sciences), vol. 2, (Leipzig, Germany: Veit & Co., 1913), {{Webarchive|url=https://web.archive.org/web/20200725232841/https://books.google.com/books?id=hqM9AQAAMAAJ&pg=RA1-PA232 |date=25 July 2020 }} ''" … berichtet er, daß der Höhle Demindân in Persien ein Dampf entströme und sich beim Erkalten als Nuschadir niederschlage, den man von da aus in alle Welt versende."'' ( … he reported that a vapor streams out of the caves at Damindan in Persia and upon cooling precipitates as ''nushadir'' , which is conveyed from there throughout the world.) In discussing ancient China's sources of ammonium chloride. ], p. 439: "The most westerly region of all lies further to the south, in Persian Baluchistan, where the Damindān (now Tamindan) valley in the Kūh-i-Taftan range, a relatively inactive volcanic massif, produces sal ammoniac down to this day."</ref><ref>Ammonium chloride was later harvested from other volcanoes: The Arabs harvested it from ] in ] during the 10th century.
			*The Arab geographer ] (c. 945/946 - 991) mentioned that ammonium chloride was obtained from Mt. Etna. See: Lippmann, Edmund Oskar von, ''Entstehung und Ausbreitung der Alchemie'' … (Origin and Spread of Alchemy … ), vol. 1, (Berlin, Germany: Springer, 1919), p. 404. {{Webarchive|url=https://web.archive.org/web/20210416172529/https://babel.hathitrust.org/cgi/pt?id=nyp.33433079413435;view=1up;seq=426 |date=16 April 2021 }} ''" … er erwähnt, daß der dortige Salmiak nicht von gleicher Güte ist wie der Siciliens, dessen Lager jetzt aber schon erschöpft seien, … "'' ( … he mentions that the salmiak there ] ] is not of equal value to that of Sicily’s, whose deposits are now, however, exhausted, … )
			*The Arab geographer ] (d. ca. 978) also mentioned that ammonium chloride was obtained from fumaroles on the slopes of Mt. Etna. {{cite journal|author=Ruska, Julius |title=Die Salmiak in die Geschichte der Alchemie|trans-title=Ammonium chloride in the history of alchemy|journal=Zeitschrift für Angewandte Chemie|volume=41|issue=50|pages=1321–1324|doi=10.1002/ange.19280415006|year=1928|bibcode=1928AngCh..41.1321R }}
			*], p. 595.
			Europeans later harvested it from the ] crater and ] near ], Italy.
			*Breislak, Scipion, ''Essais mineralogiques sur la solfatare de Pouzzole'' (Naples, Italy: Janvier Giaccio, 1792), p. 140. ''"Deux endroits de la Solfatare, celui où est construite la fontaine de vapeurs, et un autre à peu de distance produisent le muriate d'ammoniaque."'' (Two places on Solfatare — that where the fumerole has formed and another a little distance away — produce muriate of ammonia .)
			*(]) (1705) "Diverses observations chimiques. I." (Various chemical observations. I.), ''Histoire de l'Académie royale des sciences: année MDCCV, avec les memoires'' … , p. 66. {{Webarchive|url=https://web.archive.org/web/20170814083733/http://gallica.bnf.fr/ark:/12148/bpt6k3487x/f74.image |date=14 August 2017 }} ''"Monsieur Lémery a eu entre les mains un Sel tiré du Mont Vesuve, & que l'on appelle Sel Armoniac naturel."'' (Mr. Lémery got hold of a salt extracted from Mount Vesuvius, and which is called natural Armenian salt .)
			*], p. 212.
			*], p. 599.
			Ammonium chloride was also found on the island of ] in the western Indian Ocean.
			*Marcellin, Jean Baptiste Geneviève, Baron Bory de Saint-Vincent, ''Dictionnaire classique d'histoire naturelle'', vol. 1 (Paris, France: Rey et Gravier, 1822). {{Webarchive|url=https://web.archive.org/web/20200725233829/https://books.google.com/books?id=jp4AAAAAYAAJ&pg=PA270 |date=25 July 2020 }} ''"On trouve ce Minéral dans presque tous les volcans. … Elle se trouve également en Tartarie, dans le pays des Kalmuks; en Perse, au Thibet, dans l'île de Bourbon, en Bucharie, … "'' (One finds this mineral in nearly every volcano … It is found also in ] , in the country of the ], in Persia, in Tibet, on Bourbon Island , in Bucharia ] through ] and ] ] … )
			Ammonium chloride was subsequently found at Mount ] in ], Mount Chinyero on ] in the ], and the ] in ].
			*Bunsen, Robert (1847) {{Webarchive|url=https://web.archive.org/web/20210416075401/https://babel.hathitrust.org/cgi/pt?id=uva.x002457927;view=1up;seq=397 |date=16 April 2021 }} (On the intrinsic relationship of pseudo-volcanic phenomena of Iceland), ''Annalen der Chemie and Pharmacie'', '''62''' : 1–59, see pp. 8–9. {{Webarchive|url=https://web.archive.org/web/20201017173722/https://babel.hathitrust.org/cgi/pt?id=uva.x002457927;view=1up;seq=404 |date=17 October 2020 }} ''"Im Juli 1846, also nur wenige Monate nach dem Ausbruch des Vulkans, wo ich in diesen Gegenden verweilte, zeigte sich der untere Theil dieses Stromes mit dampfenden Fumarolen übersäet, in denen sich eine solche Menge reiner, zum Theil sehr schön krystallisirter Salmiak sublimirte, dass man dort, trotz der unaufhörlichen Regengüsse, dieses wertvolle Salz zu Hunderten von Pfunden hätte sammeln können."'' (In July 1846, thus only months after the eruption of the volcano , where I stayed in this region, the lower part of this flow appeared studded with steaming fumaroles, in which such a quantity of pure and sometimes very beautifully crystallized ammonium chloride had sublimated that one could have collected there — despite ceaseless downpours — hundreds of pounds of this valuable salt.)
			*Del Campo, Ángel (1912) "Los sublimados blancos del volcán Chinyero (Canarias)" (The white sublimates of the volcano Chinyero in the Canary Islands), ''Anales de la Sociedad Española de Física y Química'', '''10''' : 431–449.
			*{{cite journal|author=Shipley, J.W.|year=1919|title=Scientific results of the Katmai expeditions of the National Geographic Society: VII. Ammonia and nitrous nitrogen in the rain water of southwestern Alaska|journal=Ohio Journal of Science|volume=19|issue=4|pages=230–234|hdl=1811/2027/V19N04_230.pdf}}
			*], p. 599.</ref> (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.)<ref>The term for "ammonium chloride" in Arabic is ''nūshādir'' or ''nūshādur'', in Sanskrit, ''navasadaru'' or ''navasara'', in Chinese, ''nao sha'', and similarly in Armenian and Syriac. ], p. 596.</ref> Ammonium chloride was then transported along the ] eastwards to China and westwards to the Muslim lands and Europe.
			=== Jabirian alchemists ===
			Around 800 A.D. the iranian chemist jaber ibn hayan discovered ammonium chloride in the soot that resulted from burning camel dung, and this source became an alternative to those in Central Asia.<ref>In ''De Lapidibus'' (About Stones), which is attributed to "Pseudo-Aristotle" and which dates from ca. 750–870 A.D., is a brief statement that ammonium chloride was created at the public baths (from the soot of the fires that served to heat the bath waters). Ruska, Julius, ''Das Steinbuch des Aristoteles mit literargeschichtlichen Untersuchungen nach der arabischen Handschrift der Bibliothèque Nationale'' (Heidelberg, Germany: Carl Winter, 1912), p. 191. ''"Et unus lapis est qui vocatur nasciadhor ''i. liscianada'' qui fit in balneis."'' (And there is one stone that is called ''nasciadhor'' or ''liscianada'' that is made in the baths.) See also: ], p. 595.</ref><ref>The Persian geographer ] (d. 957 A.D.) stated that ammonium chloride was obtained from the soot of camel dung that was burned to heat the public baths in Alexandria. See: (Lippmann, 1919), p. 403. {{Webarchive|url=https://web.archive.org/web/20201017195552/https://babel.hathitrust.org/cgi/pt?id=nyp.33433079413435;view=1up;seq=425 |date=17 October 2020 }} Istakhri ''" … bestätigt das persische Vorkommen … des Nûschâdirs, 'den die Ägypter aus dem Rauche ihrer Bäder haben' , … "'' (Istakhri confirms the occurrence in Persia … of ammonium chloride (''nûshâdir''), "which the Egyptians have from the smoke of their baths" … ) See also: ], p. 595.<br>
			The production of ammonium chloride from the soot of burned animal dung was reported early in the 18th century by a number of European observers:
			*] (S.J.), ''Nouveaux Mémoires de la Compagnie de Jesus dans le Levant'' , vol. 2 (Paris, France: Nicolas le Clerc, 1717), pp. 96–98. ''" … nous arrivâmes sur le midy à ''Desmayer'' … "'' ( … we arrived at midday at ''Desmayer'', a town which is inhabited only by Muslims. It is in this place that the most esteemed sal armoniac in all Egypt is made. This salt is made in ovens, whose top is vented lengthwise and in several places. One places in these vents twenty or thirty round glass bottles, about a foot and a half in diameter, with a neck of half a foot . The bottles are sealed well: filled with soot and a little sea salt, and animal urine. Then one constructs a layer of loam and brick , which covers everything except the tops of the bottles' necks, which to the air. Then a fire is lit in the oven, and it is maintained continually for three days and three nights. The phlegm of the material contained in the bottles is driven off, and the acid salts and alkalies meet and cling to each other near the neck, form a white, round mass. The operation being completed, all of the bottles are broken, and these masses are removed, which are called "sal armoniac". It is to be noted that the soot of which I spoke, is produced by the smoke of pats, which is called ''gellée'' in Arabic. They are formed from animal manure. Any other smoke is unlikely to condense into sal armoniac.)
			*] (1720) {{Webarchive|url=https://web.archive.org/web/20200725235622/https://books.google.com/books?id=JC8yj5j2RMYC&pg=PA189 |date=25 July 2020 }} (Observations on the nature and composition of ammonium chloride), ''Histoire de l'Académie Royale des Sciences: année MDCCXX, avec les memoires'' … , pp. 189–191.
			*Lemere (1719) {{Webarchive|url=https://web.archive.org/web/20200726020127/https://books.google.com/books?id=JC8yj5j2RMYC&pg=PA191 |date=26 July 2020 }} (Address to the Academy on ammonium chloride, etc.), ''Histoire de l'Académie Royale des Sciences: année MDCCXX, avec les memoires'' … , pp. 191–194.
			*(Lemere) (1716) {{Webarchive|url=https://web.archive.org/web/20200726000230/https://books.google.com/books?id=JC8yj5j2RMYC&pg=PA195 |date=26 July 2020 }} ''Histoire de l'Académie Royale des Sciences: année MDCCXX, avec les memoires'' … , pp. 195–207. On p. 202, Lemere states that ammonium chloride can be made by combining ] and ]: ''"L'on prend de l'esprit ou du sel volatil d'urine; on jette dessus de l'esprit de sel marin, jusqu'à ce qu'il ne se fasse plus de fermentation; on fait évaporer au sable la liqueur, qui, étant séche, fournit un sel salé qui a les mêmes effets que le sel ammoniac."'' (One takes the spirit or volatile salt of urine ; one tosses on it spirit of sea salt , until it no longer makes fermentation ; one evaporates, on a sand , the solution, which, being dry, furnishes a salty solid which has the same effects as ammonium chloride.)
			*Duhamel du Monceau, Henri-Louis (1735) "Sur le sel ammoniac," ''Histoire de l'Académie Royale des Sciences: année MDCCXXXV, avec les memoires'' … , {{Webarchive|url=https://web.archive.org/web/20200725233533/https://books.google.com/books?id=EyUrWrwrrk4C&pg=RA1-PA106 |date=25 July 2020 }}
			*{{cite journal|author=Ellis, John|year=1760|url=https://archive.org/details/philtrans03735083|title=The method of making sal ammoniac in Egypt; as communicated by Dr. Linnaeus from his pupil Dr. Hasselquist, who had been lately in those parts|journal=Philosophical Transactions of the Royal Society of London|volume=51|pages=504–506|doi=10.1098/rstl.1759.0050|doi-access=free}}
			*Beckmann, Johann, ''Beyträge zur Geschichte der Erfindungen'' (Leipzig, Germany: Paul Gotthelf Kummer, 1805), vol. 5, 4. Salmiak, English translations: (1) Beckmann, Johann with William Johnston, trans., ''A History of Inventions and Discoveries'', 2nd ed. (London, England: Walker, 1814), vol. 4, {{Webarchive|url=https://web.archive.org/web/20201020051425/https://babel.hathitrust.org/cgi/pt?id=hvd.hxhqx6;view=1up;seq=376 |date=20 October 2020 }} ; and (2) Beckmann, Johann with William Johnston, trans., ''A History of Inventions, Discoveries, and Origins'', 4th ed. (London, England: Henry G. Bohn, 1846), vol. 2, {{Webarchive|url=https://web.archive.org/web/20210416172909/https://babel.hathitrust.org/cgi/pt?id=hvd.32044024313751;view=1up;seq=416 |date=16 April 2021 }}
			*{{cite journal|author= Multhauf, Robert P. |year=1965|title=Sal Ammoniac: a case history in industrialization|journal=Technology and Culture|volume=6|issue=9|pages=569–586|jstor=3101750|doi=10.2307/3101750|s2cid=113031715 }}</ref>
			The ] were the authors of the ], tentatively dated to {{circa|850|950}}.<ref name="datingcorpus">This is the dating put forward by {{harvnb|Kraus|1942–1943|loc=vol. I, p. lxv}}. For its acceptance by other scholars, see the references in {{harvnb|Delva|2017|loc=p. 38, note 14}}. Notable critics of Kraus' dating are {{harvnb|Sezgin|1971}} and {{harvnb|Nomanul Haq|1994|pp=3–47}} (cf. {{harvnb|Forster|2018}}).</ref> The word for ammonium chloride in the Jabirian corpus was ''nošāder'', Iranian in origin. Whereas ] 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 ']'.<ref name="auto">{{harvnb|Kraus|1942–1943|loc=vol. II, p. 41}}.</ref> 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.<ref>{{harvnb|Kraus|1942–1943|loc=vol. II, pp. 41–42}} (referring to {{harvnb|Stapleton|1905}}; {{harvnb|Ruska|1923a}}; {{harvnb|Ruska|1928}}). See also {{harvnb|Stapleton|Azo|Hidayat Husain|1927|pp=338–340}}.</ref>
			One of the innovations in Jabirian alchemy was the addition of ammonium chloride to the category of chemical substances known as ']' (i.e., strongly volatile substances). This included both naturally occurring ] 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 ] work ''De inventione veritatis'', where a preparation of sal ammoniac is given in the chapter ''De Salis armoniaci præparatione'', ''salis armoniaci'' being a common name in the Middle Ages for sal ammoniac.<ref>{{Cite web |year=1542 |title=Geberis philosophi perspicacissimi, summa perfectionis magisterii in sua natur ex bibliothecae Vaticanae exemplari |url=https://archive.org/details/geberisphilosoph00gebe/page/n4}}</ref>
			==References==
			{{reflist}}
			==Bibliography==
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			* {{cite journal |last1=Delva |first1=Thijs |year=2017 |title=The Abbasid Activist Ḥayyān al-ʿAṭṭār as the Father of Jābir b. Ḥayyān: An Influential Hypothesis Revisited |journal=Journal of Abbasid Studies |volume=4 |issue=1 |pages=35–61 |doi=10.1163/22142371-12340030}}
			* {{cite encyclopedia|last1=Forster|first1=Regula|year=2018|title=Jābir b. Ḥayyān|editor1-last=Fleet|editor1-first=Kate|editor2-last=Krämer|editor2-first=Gudrun|editor2-link=Gudrun Krämer|editor3-last=Matringe|editor3-first=Denis|editor4-last=Nawas|editor4-first=John|editor5-last=Rowson|editor5-first=Everett|editor5-link=Everett K. Rowson|encyclopedia=Encyclopaedia of Islam, Three|doi=10.1163/1573-3912_ei3_COM_32665}}
			* {{Cite book|last=Kraus|first=Paul|author-link=Paul Kraus (Arabist)|year=1942–1943|title=Jâbir ibn Hayyân: Contribution à l'histoire des idées scientifiques dans l'Islam. I. Le corpus des écrits jâbiriens. II. Jâbir et la science grecque|publisher=Institut Français d'Archéologie Orientale|location=Cairo|oclc=468740510|isbn=978-3-487-09115-0}}
			*{{cite book|ref= Needham|author1=Needham, Joseph |author2=Ho Ping-Yü |author3=Lu Gwei-Djen |author4=Sivin, Nathan | year=1980 | title=Science and Civilization in China|volume= 5: Chemistry and Chemical Technology, Part IV: ]al discovery and invention: apparatus, theories and gifts |place=Cambridge, England | publisher= Cambridge University Press|isbn=978-0521086905}}
			* {{cite book|last1=Nomanul Haq|first1=Syed|author-link=Syed Nomanul Haq|year=1994|title=Names, Natures and Things: The Alchemist Jābir ibn Ḥayyān and his Kitāb al-Aḥjār (Book of Stones)|location=Dordrecht|publisher=Kluwer|isbn=9789401118989|url=https://books.google.com/books?id=rydrCQAAQBAJ}}
			* {{cite journal|last1=Ruska|first1=Julius|author1-link=Julius Ruska|year=1923a|title=Sal ammoniacus, Nušādir und Salmiak|journal=Sitzungsberichte der Heidelberger Akademie der Wissenschaften, Philosophisch-Historische Klasse|volume=14|issue=5|doi=10.11588/diglit.38046}}
			* {{cite journal|last1=Ruska|first1=Julius|author1-link=Julius Ruska|year=1928|title=Der Salmiak in der Geschichte der Alchemie|journal=Zeitschrift für angewandte Chemie|volume=41|issue=50|pages=1321–1324|doi=10.1002/ange.19280415006|bibcode=1928AngCh..41.1321R }}
			* {{cite book|last1=Sezgin|first1=Fuat|author-link=Fuat Sezgin|year=1971|title=Geschichte des arabischen Schrifttums, Band IV: Alchimie, Chemie, Botanik, Agrikultur bis ca. 430 H.|location=Leiden|publisher=Brill|pages=132–269|isbn=9789004020092}}
			* {{cite journal <!-- Citation bot bypass-->|last1=Stapleton|first1=Henry E.|author1-link=Henry Ernest Stapleton|last2=Azo|first2=R.F.|last3=Hidayat Husain|first3=M.|year=1927|title=Chemistry in Iraq and Persia in the Tenth Century A.D.|journal=Memoirs of the Asiatic Society of Bengal|volume=VIII|issue=6|pages=317–418|oclc=706947607|url=http://www.southasiaarchive.com/Content/sarf.100203/231270}}
			* {{cite journal|ref=Sutton|pmid=18499318|year=2008|last1=Sutton|first1=M. A|title=Ammonia in the environment: From ancient times to the present|journal=Environmental Pollution|volume=156|issue=3|pages=583–604|last2=Erisman|first2=J. W|last3=Dentener|first3=F|last4=Möller|first4=D|doi=10.1016/j.envpol.2008.03.013|bibcode=2008EPoll.156..583S }}
			==External links==
			{{Commons category|Ammonium chloride}}
			* Calculators: , and of aqueous ammonium chloride
			*
			{{Ammonium salts}}
			{{Urologicals}}
			{{Authority control}}
			{{portal bar|Food}}
			]
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			]