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Template:Chembox SublimationConditionsTemplate:Chembox SolubilityProduct
Ammonium chloride
NH4Cl.png
Ammoniumchlorid Kristalle.jpg
IUPAC name Ammonium chloride
Other names Sal ammoniac, Salmiac, Nushadir salt, Sal armagnac, Salt armoniack, Salmiak
Identifiers
CAS number 12125-02-9
PubChem 25517
EC number 235-186-4
KEGG D01139
ChEBI CHEBI:31206
RTECS number BP4550000
SMILES [Cl-].[NH4+]
Properties
Molecular formula H4ClN
Molar mass 53.49 g mol-1
Appearance White solid, hygroscopic
Odor Odorless
Density 1.519 g/cm3[2]
Melting point

338 °C, 611 K, 640 °F

Boiling point

520 °C, 793 K, 968 °F

Solubility in water 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)[3]
Solubility Soluble in liquid ammonia, hydrazine,
Slightly soluble in acetone
Insoluble in diethyl ether, ethyl acetate[4]
Solubility in methanol 32 g/kg (17 °C)
33.5 g/kg (19 °C)
35.4 g/kg (25 °C)[4]
Solubility in ethanol 6 g/L (19 °C)[5]
Solubility in glycerol 97 g/kg[4]
Solubility in sulfur dioxide 0.09 g/kg (0 °C)
0.031 g/kg (25 °C)[4]
Solubility in acetic acid 0.67 g/kg (16.6 °C)[4]
Vapor pressure 133.3 Pa (160.4 °C)
6.5 kPa (250 °C)
33.5 kPa (300 °C)[5]
Acidity (pKa) 9.24
-36.7·10−6 cm3/mol[6]
Refractive index (nD) 1.642 (20 °C)[4]
Structure
Crystal structure CsCl, cP2[7]
Space group Pm3m, No. 221
Lattice constant a = 0.3876 nm
Thermochemistry
Std enthalpy of
formation
ΔfHo298
−314.43 kJ/mol[5]
Standard molar
entropy
So298
94.56 J/mol·K[5]
Specific heat capacity, C 84.1 J/mol·K[5]
Pharmacology
ATC code
Hazards
NFPA 704

NFPA 704.svg

0
2
0
 
Flash point Non-flammable
U.S. Permissible
exposure limit (PEL)
none[8]
Related compounds
Other anions Ammonium fluoride
Ammonium bromide
Ammonium iodide
Other cations Sodium chloride
Potassium chloride
Hydroxylammonium chloride
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

Ammonium chloride is a chemical compound composed of ammonium and chloride ions. It is a colorless crystalline compound. It is used in soldering. It is also used as an electrolyte in the Leclanche cell, a type of primary cell. Ammonium chloride can be deprotonated by strong bases such as sodium hydroxide to produce ammonia gas.It is sublime compound.

Related pages

References

  1. "Solubility Products of Selected Compounds". Salt Lake Metals. http://www.saltlakemetals.com/SolubilityProducts.htm. Retrieved 2014-06-11. 
  2. Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.46. ISBN 1439855110 . 
  3. 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.
  4. 4.0 4.1 4.2 4.3 4.4 4.5 4.6 ammonium chloride. Chemister.ru (2007-03-19). Retrieved on 2018-01-23.
  5. 5.0 5.1 5.2 5.3 5.4 Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc.. ISBN 978-0-07-049439-8 . 
  6. Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.131. ISBN 1439855110 . 
  7. 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. doi:10.1016/0038-1098(93)90362-Q . 
  8. "NIOSH Pocket Guide to Chemical Hazards #0029". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0029.html. 



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