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Potassium Ferrate

Potassium ferrate is paramagnetic, and is a rare example of an iron(VI) compound. It has attracted interest for applications in "green chemistry" because the by-products of its use, iron oxides, are environmentally innocuous. In contrast, some related oxidants such as chromate are considered environmentally hazardous. However, the main difficulty with the use of potassium ferrate is that it is often too reactive, as indicated by the fact that it decomposes in contact with water. Because the side products of its redox reactions are rust-like iron oxides, potassium ferrate has been described as a "green oxidant." It has been employed in waste-water treatment as an oxidant for organic contaminants and as a biocide. Conveniently, the resulting reaction product is iron(III) oxyhydroxide, an excellent flocculant. In organic synthesis, potassium ferrate oxidizes primary alcohols. It has also attracted attention as a potential cathode material in a "super iron battery."

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Potassium Ferrocyanide

Potassium ferrocyanide is a coordination compound. It can be used as an alternate nitrogen source for plants. It is often used as a gardening technique. Industrially, this complex is used in metal extraction and to make adhesives, computer electronics, fire retardants, cosmetics, dyes, nylon, paints, inks, plexiglass, pharmaceuticals, and rocket propellant. It is also used in low doses in some food preparation. It works as an anti-caking agent and it removes copper from red wine, as copper is used as a fungicide on grapes. In the laboratory, potassium ferrocyanide is used to determine the concentration of potassium permanganate, a compound often used in titrations based on redoxreactions.

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Potassium Iodide

reparation of Potassium Iodate which is obtained by the oxidation of Potassium Iodide with Potassium chlorate or Potassium bromate. It is useful in the treatment of radiation poisoning resulting from nuclear accidents and also as a nutritional supplement for iodine in poultry feeds

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Potassium Metaperiodate

POTASSIUM PERIODATE; Potassium m-Perioda; POTASSIUM M-PERIODATE; PotassiumPeriodateKIO4; POTASSIUM METAPERIODATE; Potassium periodate 99%; PotassiumMetaperiodateGr; potassium periodate, acs; Potassium metaperiodiate; POTASSIUM PERIODATE, META

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Potassium Methoxide

Potassium methoxide is commonly used as a catalyst for transesterification in the production of biodiesel.

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Potassium Perchlorate

Potassium perchlorate is an inorganic salt. Like other perchlorates, this salt is a strong oxidizer and potentially reacts with many organic substances. This usually obtained as a colorless, crystalline solid is a common oxidizer used in fireworks, ammunition percussion caps, and is used variously in propellants, flash compositions, stars, and sparklers. It has been used as a solid rocket propellant, although in that application it has mostly been replaced by the higher performance ammonium perchlorate. Potassium perchlorate can be used as an antithyroid agent used to treat hyperthyroidism, usually in combination with one other medication.

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Potassium Persulphate

Potassium persulphate is a compound. It is a food additive and it is used in organic chemistry as an oxidizing agent for instance in the Elbs persulfate oxidation, and in hair dye substances as whitening agent with hydrogen peroxide. It takes also an important role as initiator for emulsion polymerization.

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Potassium Tetraborate

Potassium tetraborate is an excellent solvent for metallic oxides at high temperatures.In the field of metallurgy, it is used in the preparation of special welding, soldering and brazing fluxes of stainless steel or various nonferrous metals to avoid the “glare” associated with sodium borate.

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Potassium Thiocyanate

Potassium thiocyanate is an important salt of the thiocyanate anion, one of the pseudohalides. Dilute aqueous potassium thiocyanate 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, 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. Similarly, this reaction is used as a test for Fe3+ in the laboratory.

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