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  Home > JCE Print > Journal of Chemical Education > Issues > 1999  > September  >
In the Laboratory
Spectrophotometric Determination of Thiocyanate in Human Saliva
Markku Lahti
Department of Chemistry, University of Turku, FIN-20014 Turku, Finland

Juhani Vilpo
Department of Clinical Chemistry, Tampere University Hospital and University of Tampere Medical School, P.O. Box 2000, FIN-30521 Tampere, Finland

Jari Hovinen
Wallac Oy, P.O. Box 10 FIN-20101 Turku, Finland

Cover
September 1999
Vol. 76 No. 9
p. 1281
Abstract
The equilibrium constant between iron(III) ion and thiocyanate ion to form a thiocyanatoiron(III) ion can be conveniently measured with visible spectrophotometry because the FeSCN+2 solutions are deep blood-red. Hence this reaction is often used when teaching chemical equilibrium to students of general chemistry. The same reaction can be exploited in the qualitative and quantitative analysis of SCN- ions in solution. The experiment can be easily made more attractive to students when the thiocyanate ion concentration measured is from human saliva. Here is described how qualitative and quantitative analysis of human saliva thiocyanate ion can be performed as a part of the laboratory exercise for the determination of chemical equilibrium between Fe+3 and SCN- ions. For qualitative analysis a few drops of saliva (each student is using his or her own saliva) is treated with a drop of acidic Fe(NO3)3 solution. The deep blood-red color of FeSCN+2 complex is clearly demonstrated. Then each student measures his or her saliva thiocyanate ion concentration with visible spectrophotometry.
More Information
*  Citation
 Lahti, Markku; Vilpo, Juhani; Hovinen, Jari. J. Chem. Educ. 1999 76 1281.
*  Keywords
 Analytical Chemistry; Laboratory Instruction; UV-Vis Spectroscopy; Undergraduate Research; Medicinal Chemistry
*  History
 Created:
Last Updated:		 July 30, 1999
June 23, 2005
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