The Full Wiki

More info on Potassium thiocyanate

Potassium thiocyanate: Wikis

Advertisements
  

Note: Many of our articles have direct quotes from sources you can cite, within the Wikipedia article! This article doesn't yet, but we're working on it! See more info or our list of citable articles.

Encyclopedia

From Wikipedia, the free encyclopedia

Potassium thiocyanate
Identifiers
CAS number 333-20-0 Yes check.svgY
PubChem 10931372
RTECS number XL1925000
Properties
Molecular formula CKNS
Molar mass 97.18 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
NFPA 704.svg
0
3
0
LD50 854 mg/kg
Related compounds
Other anions Potassium cyanate
Potassium cyanide
Other cations Sodium thiocyanate
Ammonium thiocyanate
 Yes check.svgY (what is this?)  (verify)
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 blood red solution, 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

  1. ^ Smith, P. A. S.; Kan, R. O. (1973), "2a-Thiohomophthalimide", Org. Synth., http://www.orgsyn.org/orgsyn/orgsyn/prepContent.asp?prep=cv5p1051 ; Coll. Vol. 5: 1051 
  2. ^ Searles, S.; Lutz, E. F.; Hays, H. R.; Mortensen, H. E. (1973), "Ethylenesulfide", Org. Synth., http://www.orgsyn.org/orgsyn/orgsyn/prepContent.asp?prep=cv5p0562 ; Coll. Vol. 5: 562 
  3. ^ van Tamelen, E. E. (1963), "Cyclohexenesulfide", Org. Synth., http://www.orgsyn.org/orgsyn/orgsyn/prepContent.asp?prep=cv4p0232 ; Coll. Vol. 4: 232 
Advertisements

Advertisements






Got something to say? Make a comment.
Your name
Your email address
Message