Potassium thiocyanate

Potassium thiocyanate
Other names Potassium sulfocyanate Potassium isothiocyanate Potassium thiocyanide
Identifiers
CAS number	333-20-0 Y
PubChem	516872
ChemSpider	9150 Y
UNII	TM7213864A Y
ChEBI	CHEBI:30951 Y
RTECS number	XL1925000
Jmol-3D images	Image 1
SMILES C(#N)[S-].[K+]
InChI InChI=1S/CHNS.K/c2-1-3;/h3H;/q;+1/p-1 Y Key: ZNNZYHKDIALBAK-UHFFFAOYSA-M Y InChI=1/CHNS.K/c2-1-3;/h3H;/q;+1/p-1 Key: ZNNZYHKDIALBAK-REWHXWOFAT
Properties
Molecular formula	KSCN
Molar mass	97.181 g mol−1
Appearance	Colorless deliquescent crystals
Odor	Odorless
Density	1.886 g/cm3
Melting point	173.2 °C, 446 K, 344 °F
Boiling point	500 °C (decomp)
Solubility in water	177 g/100 mL (0 °C) 217 g/100 mL (20 °C)
Solubility in acetone	21.0 g/100 mL
Hazards
MSDS	ICSC 1088
EU Index	615-004-00-3
EU classification	Harmful (Xn)
R-phrases	R20/21/22 R32 R52/53
S-phrases	(S2) S13 S61
NFPA 704	0 3 0
LD50	854 mg/kg
Related compounds
Other anions	Potassium cyanate Potassium cyanide
Other cations	Sodium thiocyanate Ammonium thiocyanate
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Potassium thiocyanate is the chemical compound with the molecular formula KSCN. It is an important salt of the thiocyanate anion, one of the pseudohalides. The compound has a low melting point relative to most other inorganic salts.

Use in chemical synthesis

Aqueous KSCN reacts almost quantitatively with Pb(NO₃)₂ to give Pb(SCN)₂, which has been used to convert acyl chlorides to thiocyanates.^[1]

KSCN converts ethylene carbonate to ethylenesulfide.^[2] For this purpose, the KSCN is first melted under vacuum to remove water. In a related reaction, KSCN converts cyclohexene oxide to the corresponding episulfide.^[3]

C₆H₁₀O + KSCN → C₆H₁₀S + KOCN

KSCN is also the starting product for the synthesis of carbonyl sulfide.

Other uses

Dilute aqueous KSCN is occasionally used for moderately realistic blood effects in film and theater. It can be painted onto a surface or kept as a colorless solution. When in contact with ferric chloride solution (or other solutions containing Fe³⁺), the product of the reaction is a solution with a blood red colour, due to the formation of the thiocyanatoiron complex ion. Thus this chemical is often used to create the effect of 'stigmata'. Because both solutions are colorless, they can be placed separately on each hand. When the hands are brought into contact, the solutions react and the effect looks remarkably like stigmata.^{[citation needed]}

Similarly, this reaction is used as a test for Fe³⁺ in the laboratory.

References

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