Ammonium chloride

Ammonium chloride
Unit cell of ammonium chloride
Crystalline ammonium chloride
Names
IUPAC name
Ammonium chloride
Other names
  • Sal ammoniac
  • Salmiac
  • Nushadir salt
  • Sal armagnac
  • Ammonium Muriate
  • Amchlor
  • Salt armoniack
  • Salmiak
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.031.976 Edit this at Wikidata
EC Number
  • 235-186-4
KEGG
RTECS number
  • BP4550000
UNII
UN number 3077
  • InChI=1S/ClH.H3N/h1H;1H3 checkY
    Key: NLXLAEXVIDQMFP-UHFFFAOYSA-N checkY
  • InChI=1/ClH.H3N/h1H;1H3
    Key: NLXLAEXVIDQMFP-UHFFFAOYAI
  • [Cl-].[NH4+]
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]
ΔdecompHo = 176.1 kJ/mol[3]
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]
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]
1.642 (20 °C)[2]
Structure
CsCl, cP2[9]
Pm3m, No. 221
a = 0.3876 nm
1
Thermochemistry
84.1 J/mol·K[6]
94.56 J/mol·K[6]
−314.43 kJ/mol[6]
−202.97 kJ/mol[6]
Pharmacology
B05XA04 (WHO) G04BA01 (WHO)
Hazards
GHS labelling:
GHS07: Exclamation mark[7]
Warning
H302, H319[7]
P305+P351+P338[7]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1650 mg/kg (rats, oral)
NIOSH (US health exposure limits):
PEL (Permissible)
none[10]
REL (Recommended)
TWA 10 mg/m3 ST 20 mg/m3 (as fume)[10]
IDLH (Immediate danger)
N.D.[10]
Safety data sheet (SDS) ICSC 1051
Related compounds
Other anions
Ammonium fluoride
Ammonium bromide
Ammonium iodide
Other cations
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.

  1. ^ 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.
  2. ^ 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.
  3. ^ Cite error: The named reference Wiberg&Holleman was invoked but never defined (see the help page).
  4. ^ 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.
  5. ^ "Solubility Products of Selected Compounds". Salt Lake Metals. Archived from the original on 21 October 2015. Retrieved 11 June 2014.
  6. ^ a b c d e f Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 978-0-07-049439-8.
  7. ^ a b c d Sigma-Aldrich Co., Ammonium chloride. Retrieved on 2014-06-11.
  8. ^ 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.
  9. ^ 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.
  10. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0029". National Institute for Occupational Safety and Health (NIOSH).