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Thiocyanate complexes are not widely used commercially. Possibly the oldest application of thiocyanate complexes was the use of thiocyanate as a test for ferric ions in aqueous solution. [14] The reverse was also used: testing for the presence of thiocyanate by the addition of ferric salts. The 1:1 complex of thiocyanate and iron is deeply red.
In coordination chemistry, a stability constant (also called formation constant or binding constant) is an equilibrium constant for the formation of a complex in solution. It is a measure of the strength of the interaction between the reagents that come together to form the complex. There are two main kinds of complex: compounds formed by the ...
Within chemistry, a Job plot, otherwise known as the method of continuous variation or Job's method, is a method used in analytical chemistry to determine the stoichiometry of a binding event. The method is named after Paul Job and is also used in instrumental analysis and advanced chemical equilibrium texts and research articles.
An example of a low-spin iron(III) complex is [Fe(CN) 6] 3−. The cyanide ligands may easily be detached in [Fe(CN) 6 ] 3− , and hence this complex is poisonous, unlike the iron(II) complex [Fe(CN) 6 ] 4− found in Prussian blue, [ 16 ] which does not release hydrogen cyanide except when dilute acids are added. [ 17 ]
The resulting organolithium compound serves as a nucleophile in various reactions, for example, with trimethylsilyl chloride: [citation needed] (η 6-C 6 H 6)Cr(CO) 3 is a useful catalyst for the hydrogenation of 1,3-dienes. The product alkene results from 1,4-addition of hydrogen. The complex does not hydrogenate isolated double bonds ...
Thiocyanate [6] is known to be an important part in the biosynthesis of hypothiocyanite by a lactoperoxidase. [7] [8] [9] Thus the complete absence of thiocyanate or reduced thiocyanate [10] in the human body, (e.g., cystic fibrosis) is damaging to the human host defense system.
Ammonium thiocyanate is used in the manufacture of herbicides, thiourea, and transparent artificial resins; in matches; as a stabilizing agent in photography; in various rustproofing compositions; as an adjuvant in textile dyeing and printing; as a tracer in oil fields; in the separation of hafnium from zirconium (important for the production of hafnium-free zircalloy for use in nuclear fuel ...
For example, it will react with diluted sulfuric acid under heating forming potassium sulfate, ferric sulfate and hydrogen cyanide. 2 K 3 [Fe(CN) 6] + 6 H 2 SO 4 → 3 K 2 SO 4 + Fe 2 (SO 4) 3 + 12 HCN. This won't occour with concentrated sulfuric acid as hydrolysis to formic acid and dehydration to carbon monoxide will take place instead. [17]