| Sodium ferrocyanide[1] | |
|---|---|
 |
|
| IUPAC name |
Tetrasodium [hexacyanoferrate(II)]
|
| Other names | Yellow prussiate of soda (YPS), Tetrasodium hexacyanoferrate, Gelbnatron, Ferrocyannatrium |
| Identifiers | |
| CAS number | 13601-19-9 |
| PubChem | 26129 |
| EC number | 237-081-9 |
| Properties | |
| Molecular formula | Na4Fe(CN)6 |
| Molar mass | 303.91 g/mol |
| Appearance | Yellow crystals |
| Density | 1.458 g/cm3 |
| Melting point |
435 °C (decomposes) |
| Solubility in water | 18 g/100 mL |
| Structure | |
| Crystal structure | monoclinic |
| Related compounds | |
| Other anions | Sodium ferricyanide (Red prussiate of soda) |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
| Infobox references | |
Sodium ferrocyanide, also known as tetrasodium hexacyanoferrate or sodium hexacyanoferrate (II), is a coordination compound of formula Na4Fe(CN)6 that forms semitransparent yellow crystals at room temperature and decomposes at its boiling point. It is soluble in water and insoluble in alcohol. Despite the presence of the cyanide ligands, sodium ferrocyanide is not especially toxic (acceptable daily intake 0-0.025 mg/(kg body weight)[2]) because the cyanides are tightly bound to the metal, although it can react with acid or photodecompose to release hydrogen cyanide gas.
In its hydrous form, Na4Fe(CN)6•10H2O (sodium ferrocyanide decahydrate), it is generally known as yellow prussiate of soda.
Uses
As yellow prussiate of soda, it is added to road and food grade salt as an anticaking agent.[2] When combined with iron, it converts to a deep blue pigment, which is the main component of prussian blue.[3] In photography, it is used for bleaching, toning, and fixing. It is used as a stabilizer for the coating on welding rods. In the petroleum industry, it is used for removal of mercaptans.
References
- ^ Sodium ferrocyanide MSDS
- ^ a b "Toxicological evaluation of some food additives including anticaking agents, antimicrobials, antioxidants, emulsifiers and thickening agents". World Health Organization, Geneva. 1974. http://www.inchem.org/documents/jecfa/jecmono/v05je02.htm. Retrieved 18 May 2009.
- ^ "Prussian blue". Encyclopædia Britannica. http://www.britannica.com/EBchecked/topic/480982/Prussian-blue. Retrieved 18 May. 2009.
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