Sodium chloride
Appearance
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| Names | |||
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| IUPAC name
Sodium chloride | |||
| Ither names
Common salt Halite | |||
| Identifiers | |||
3D model (JSmol) |
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| 3534976 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| EC Nummer | 231-598-3 | ||
| Gmelin Reference | 13673 | ||
| KEGG | |||
| MeSH | Sodium+chloride | ||
PubChem CID |
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| RTECS nummer | VZ4725000 | ||
| UNII | |||
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| Properties | |||
| NaCl | |||
| Molar mass | 58.44 g mol−1 | ||
| Appearance | Colorless crystals | ||
| Odour | Odorless | ||
| Density | 2.165 g cm−3 | ||
| Meltin pynt | 801 °C (1,474 °F; 1,074 K) | ||
| Bylin pynt | 1,413 °C (2,575 °F; 1,686 K) | ||
| 359 g L−1 | |||
| Solubility in ammonia | 21.5 g L−1 | ||
| Solubility in methanol | 14.9 g L−1 | ||
| Refractive index (nD) | 1.5442 (at 589 nm) | ||
| Structur | |||
| Cubic (see text), cF8 | |||
| Space group | Fm3m, No. 225 | ||
a = 564.02 pm | |||
| Octahedral (Na+) Octahedral (Cl−) | |||
| Thermochemistry | |||
| Speceefic heat capacity, C | 36.79 J K−1 mol−1 | ||
| Staundart molar entropy S |
72.11 J K−1 mol−1 | ||
| Std enthalpy o formation ΔfH |
−411.12 kJ mol−1 | ||
| Hazards | |||
| NFPA 704 | |||
| Lethal dose or concentration (LD, LC): | |||
LD50 (Median dose) |
3000–8000 mg/kg (oral in rats, mice, rabbits)[1] | ||
| Relatit compoonds | |||
Ither anions |
Sodium fluoride Sodium bromide Sodium iodide | ||
Ither cations |
Lithium chloride Potassium chloride Rubidium chloride Caesium chloride | ||
Except whaur itherwise notit, data are gien for materials in thair staundart state (at 25 °C [77 °F], 100 kPa). | |||
| Infobox references | |||
Sodium chloride, forby kent as saut, common saut, table saut or halite, is an ionic compound wi the formula NaCl, representin equal proportions o sodium an chlorine.[2] Sodium chloride is the saut maist responsible for the salinity o the ocean an o the extracellular fluid of mony multicellular organisms. As the major ingredient in edible saut, it is commonly uised as a condiment an fuid preservative.
References
[eedit | eedit soorce]- ↑ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. p. 369. ISBN 1-903996-65-1.CS1 maint: multiple names: authors leet (link)
- ↑ "Salt: A Common Ionic Compound". Retrieved 6 September 2023.
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