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| Names | |||
|---|---|---|---|
| IUPAC name Sodium thiocyanate | |||
| Other names Sodium rhodanide Sodium sulfocyanate Sodium rhodanate Thiocyanic acid, sodium salt | |||
| Identifiers | |||
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3D model (JSmol) | |||
| 3594965 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider |
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| ECHA InfoCard | 100.007.960 | ||
| EC Number |
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| 1249825 | |||
| RTECS number |
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| UNII | |||
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| Properties | |||
| NaSCN | |||
| Molar mass | 81.072 g/mol | ||
| Appearance | deliquescent colorless crystals | ||
| Density | 1.735 g/cm3 | ||
| Melting point | 287 °C (549 °F; 560 K) | ||
| Boiling point | 307 °C (585 °F; 580 K) decomposes | ||
| 139 g/100 mL (21 °C) 225 g/100 mL (100 °C) | |||
| Solubility | soluble inacetone,alcohols,ammonia,SO2 | ||
| Acidity (pKa) | −1.28 | ||
Refractive index (nD) | 1.545 | ||
| Structure | |||
| orthorhombic | |||
| Hazards | |||
| GHS labelling: | |||
  | |||
| Danger | |||
| H302,H312,H332,H412 | |||
| P261,P264,P270,P271,P273,P280,P301+P312,P302+P352,P304+P312,P304+P340,P305+P351+P338,P310,P312,P322,P330,P337+P313,P363,P501 | |||
| NFPA 704 (fire diamond) | |||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose) | 764 mg/kg (oral, rat)[1] | ||
| Safety data sheet (SDS) | ICSC 0675 | ||
| Related compounds | |||
Otheranions | Sodium cyanate Sodium cyanide | ||
Othercations | Lithium thiocyanate Potassium thiocyanate Ammonium thiocyanate | ||
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |||
Sodium thiocyanate (sometimes calledsodium sulphocyanide) is thechemical compound with the formula NaSCN. This colorlessdeliquescentsalt is one of the main sources of thethiocyanateanion. As such, it is used as a precursor for thesynthesis of pharmaceuticals and otherspecialty chemicals.[2] Thiocyanate salts are typically prepared by the reaction ofcyanide with elementalsulfur:
Sodium thiocyanate crystallizes in anorthorhombic cell. Each Na+ center is surrounded by three sulfur and three nitrogen ligands provided by the triatomic thiocyanate anion.[3] It is commonly used in thelaboratory as atest for the presence ofFe3+ ions.
Sodium thiocyanate is employed to convertalkyl halides into the corresponding alkylthiocyanates. Treatment ofisopropyl bromide with sodium thiocyanate in a hot ethanolic solution affords isopropyl thiocyanate.[4] Protonation of sodium thiocyanate affordsisothiocyanic acid, S=C=NH (pKa = −1.28).[5] Isothiocyanic acid, typically generated in situ from sodium thiocyanate, adds toanilines to afford2-aminobenzothiazoles.[6]
Closely related reagents includeammonium thiocyanate andpotassium thiocyanate, which has twice the solubility in water.Silver thiocyanate may be used as well; the precipitation of insoluble silver halides help simplifyworkup.
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