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Potassium Ferricyanide 99% (1kg)
Potassium Ferricyanide 99% (1kg)
Potassium ferricyanide is the chemical compound with the formula K3[Fe(CN)6]. This bright red salt contains the octahedrally coordinated [Fe(CN)6]3− ion. It is soluble in water and its solution shows some green-yellow fluorescence. It was discovered in 1822 by Leopold Gmelin,[3][4] and was initially used in the production of ultramarine dyes.
Chemical Properties
| Properties | |
|---|---|
| K3[Fe(CN)6] | |
| Molar mass | 329.24 g/mol |
| Appearance | deep red crystals, sometimes small pellets, orange to dark red powder |
| Density | 1.89 g/cm3, solid |
| Melting point | 300 °C (572 °F; 573 K) |
| Boiling point | decomposes |
| 330 g/L (“cold water”) 464 g/L (20 °C) 775 g/L (“hot water”)[1] |
|
| Solubility | slightly soluble in alcohol soluble in acid soluble in water |
| +2290.0·10−6 cm3/mol | |
Chemical Structure Potassium Ferricyanide 99% (1kg)
Safety and storage
Keep it in dry and cool place at r.t.
Description Potassium Ferricyanide 99% (1kg)
Applications
The compound is also used to harden iron and steel, in electroplating, dyeing wool, as a laboratory reagent, and as a mild oxidizing agent in organic chemistry.
Blueprinting and photography
The compound has widespread use in blueprint drawing and in photography (Cyanotype process). Several photographic print toning processes involve the use of potassium ferricyanide.
Potassium ferricyanide was used as an oxidizing agent to remove silver from color negatives and positives during processing, a process called bleaching. Because potassium ferricyanide bleaches are environmentally unfriendly, short-lived, and capable of releasing hydrogen cyanide gas if mixed with high concentrations and volumes of acid, bleaches using ferric EDTA have been used in color processing since the 1972 introduction of the Kodak C-41 process. In color lithography, potassium ferricyanide is used to reduce the size of color dots without reducing their number, as a kind of manual color correction called dot etching. It is also used in black-and-white photography with sodium thiosulfate (hypo) to reduce the density of a negative or gelatin silver print where the mixture is known as Farmer’s reducer; this can help offset problems from overexposure of the negative, or brighten the highlights in the print.[6]
Reagent in organic synthesis
Potassium ferricyanide is a used as an oxidant in organic chemistry.[7][8] It is an oxidant for catalyst regeneration in Sharpless dihydroxylations.[9][10]
Sensors and indicators
Potassium ferricyanide is also one of two compounds present in ferroxyl indicator solution (along with phenolphthalein) that turns blue (Prussian blue) in the presence of Fe2+ ions, and which can therefore be used to detect metal oxidation that will lead to rust. It is possible to calculate the number of moles of Fe2+ ions by using a colorimeter, because of the very intense color of Prussian blue.
In physiology experiments potassium ferricyanide provides a means increasing a solution’s redox potential (E°’ ~ 436 mV at pH 7). As such, it can oxidize reduced cytochrome c (E°’ ~ 247 mV at pH 7) in isolated mitochondria. Sodium dithionite is usually used as a reducing chemical in such experiments (E°’ ~ −420 mV at pH 7).
Potassum ferricyanide is used to determine the ferric reducing power potential of a sample (extract, chemical compound, etc.).[11] Such a measurement is used to determine of the antioxidant property of a sample.
Potassium ferricyanide is a component of amperometric biosensors as an electron transfer agent replacing an enzyme’s natural electron transfer agent such as oxygen as with the enzyme glucose oxidase. It is an ingredient in commercially available blood glucose meters for use by diabetics.