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| Names | |
|---|---|
| IUPAC name
Ammonium chloride
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Other names
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.031.976 |
| EC Number |
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| KEGG | |
PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 3077 |
CompTox Dashboard (EPA)
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| Properties | |
| ClH4N | |
| Molar mass | 53.49 g·mol−1 |
| Appearance | White or colorless crystalline solid, hygroscopic |
| Odor | Odorless |
| Density | 1.519 g/cm3[1] |
| Melting point | 338 °C (640 °F) |
| Decomposes at 337.6 °C at 1 atm[2] ΔdecompH | |
| 244 g/L (−15 °C) 294 g/L (0 °C) 383.0 g/L (25 °C) 454.4 g/L (40 °C) 740.8 g/L (100 °C)[4] | |
Solubility product (Ksp)
|
30.9 (395 g/L)[5] |
| Solubility | Soluble in liquid ammonia, hydrazine, Slightly soluble in acetone Insoluble in diethyl ether, ethyl acetate[2] |
| Solubility in methanol | 32 g/kg (17 °C) 33.5 g/kg (19 °C) 35.4 g/kg (25 °C)[2] |
| Solubility in ethanol | 6 g/L (19 °C)[6] |
| Solubility in glycerol | 97 g/kg[2] |
| Solubility in sulfur dioxide | 0.09 g/kg (0 °C) 0.031 g/kg (25 °C)[2] |
| Solubility in acetic acid | 0.67 g/kg (16.6 °C)[2] |
| Vapor pressure | 133.3 Pa (160.4 °C)[7] 6.5 kPa (250 °C) 33.5 kPa (300 °C)[6] |
| Acidity (pKa) | 9.24 |
| -36.7·10−6 cm3/mol[8] | |
Refractive index (nD)
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1.642 (20 °C)[2] |
| Structure | |
| CsCl, cP2[9] | |
| Pm3m, No. 221 | |
a = 0.3876 nm
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Formula units (Z)
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1 |
| Thermochemistry | |
Heat capacity (C)
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84.1 J/mol·K[6] |
Std molar
entropy (S⦵298) |
94.56 J/mol·K[6] |
Std enthalpy of
formation (ΔfH⦵298) |
−314.43 kJ/mol[6] |
Gibbs free energy (ΔfG⦵)
|
−202.97 kJ/mol[6] |
| Pharmacology | |
| B05XA04 (WHO) G04BA01 (WHO) | |
| Hazards | |
| GHS labelling: | |
 [7]
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| Warning | |
| H302, H319[7] | |
| P305+P351+P338[7] | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
|
1650 mg/kg (rats, oral) |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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none[10] |
REL (Recommended)
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TWA 10 mg/m3 ST 20 mg/m3 (as fume)[10] |
IDLH (Immediate danger)
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N.D.[10] |
| Safety data sheet (SDS) | ICSC 1051 |
| Related compounds | |
Other anions
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Ammonium fluoride Ammonium bromide Ammonium iodide |
Other cations
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Sodium chloride Potassium chloride Hydroxylammonium chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ammonium chloride is an inorganic chemical compound with the chemical formula NH4Cl, also written as [NH4]Cl. It is an ammonium salt of hydrogen chloride. It consists of ammonium cations [NH4]+ and chloride anions Cl−. 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.
- ^ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.46. ISBN 1-4398-5511-0.
- ^ a b c d e f g ammonium chloride Archived 23 July 2015 at the Wayback Machine. Chemister.ru (2007-03-19). Retrieved on 2018-01-23.
- ^ Cite error: The named reference
Wiberg&Hollemanwas invoked but never defined (see the help page). - ^ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). D. van Nostrand Company.
Results here are multiplied by water's density at temperature of solution for unit conversion. - ^ "Solubility Products of Selected Compounds". Salt Lake Metals. Archived from the original on 21 October 2015. Retrieved 11 June 2014.
- ^ a b c d e f Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 978-0-07-049439-8.
- ^ a b c d Sigma-Aldrich Co., Ammonium chloride. Retrieved on 2014-06-11.
- ^ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.131. ISBN 1-4398-5511-0.
- ^ Breñosa, A.G; Rodríguez, F; Moreno, M (1993). "Phase transition temperatures and thermal hysteresis in NH4Cl1−xBrx (x≤0.05) crystals determined through charge transfer spectra of Cu2+(II) centres". Solid State Communications. 85 (2): 135. Bibcode:1993SSCom..85..135B. doi:10.1016/0038-1098(93)90362-Q.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0029". National Institute for Occupational Safety and Health (NIOSH).