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Ferric oxide, commonly called rust, is a very complicated material that contains iron(III). Iron(III) is found in many minerals and solids, e.g., oxide Fe 2 O 3 (hematite) and iron(III) oxide-hydroxide FeO(OH) are extremely insoluble reflecting their polymeric structure. Rust is a mixture of iron(III) oxide and oxide-hydroxide that usually ...
In chemistry, hypochlorite, or chloroxide is an anion with the chemical formula ClO −. It combines with a number of cations to form hypochlorite salts. Common examples include sodium hypochlorite (household bleach ) and calcium hypochlorite (a component of bleaching powder, swimming pool "chlorine"). [ 1 ]
Iron(III) chloride forms a 1:2 adduct with Lewis bases such as triphenylphosphine oxide; e.g., FeCl 3 (OP(C 6 H 5) 3) 2. The related 1:2 complex FeCl 3 (OEt 2) 2, where Et = C 2 H 5), has been crystallized from ether solution. [14] Iron(III) chloride also reacts with tetraethylammonium chloride to give the yellow salt of the tetrachloroferrate ...
Ferrate(VI) salts are formed by oxidizing iron in an aqueous medium with strong oxidizing agents under alkaline conditions, or in the solid state by heating a mixture of iron filings and powdered potassium nitrate. [2] For example, ferrates are produced by heating iron(III) hydroxide with sodium hypochlorite in alkaline solution: [3] 2 Fe(OH) 3 ...
In the wet oxidation method, K 2 FeO 4 is prepared by oxidizing an alkaline solution of an iron(III) salt. Generally, this method employs either ferrous (Fe II) or ferric (Fe III) salts as the source of iron ions, calcium, sodium hypochlorite (Ca(ClO) 2, NaClO), sodium thiosulfate (Na 2 S 2 O 3) or chlorine (Cl 2) as oxidizing agents and, finally, sodium hydroxide, sodium carbonate (NaOH, NaCO ...
The formation of Fe(III)-EDTA (FeY) − can be described as follows: FeSO 4 ∙7H 2 O + K 2 H 2 Y + 1/4 O 2 → K[FeY(H 2 O)]. H 2 O + KHSO 4 + 5.5 H 2 O (1) [8]. Iron chelate has also been used as a bait in the chemical control of slugs, snails and slaters in agriculture in Australia and New Zealand.
The iron compounds produced on the largest scale in industry are iron(II) sulfate (FeSO 4 ·7H 2 O) and iron(III) chloride (FeCl 3). The former is one of the most readily available sources of iron(II), but is less stable to aerial oxidation than Mohr's salt ((NH 4) 2 Fe(SO 4) 2 ·6H 2 O). Iron(II) compounds tend to be oxidized to iron(III ...
The chloride ions cause the mercury thiocyanate salt to dissociate and the thiocyanate ion to bind Fe(III), which absorbs intensely at 450 nm. This absorption allows for the measurement of the concentration of the iron complex. This value allows one to calculate the concentration of chloride. [8]