Ferrous bromide oxide

Henry prepared sodium and potassium bromides by boiling ferrous bromide respectively with potassium or sodium carbonate until the precipitate is brown the clear liquid was then filtered and evaporated. J. Knobloch recommended treating a mixture of ferrous bromide with milk of lime, and then with potassium sulphate if potassium bromide is desired, or with Glauber s salt if sodium bromide is to be made. The mixture is then to be boiled, the precipitated iron oxide filtered off, and the soln. evaporated, for cubic crystals of potassium bromide. This is the principle of the method employed for manufacturing potassium bromide on a large scale ... 

Both the aqueous and alcoholic solutions of ferrous bromide absorb nitric oxide,2 the limit of absorption being reached with one molecule of NO to each atom of iron. The compound FeBr2.NO has not been isolated. 

Iron(If) bromide, FeBr2 (ferrous bromide), is a pale yellow/brown hygroscopic solid soluble in water and donor organic solvents. It may be prepared from iron and bromine at 200 °C, or iron and HBr in methanol, hydrobromination of iron(III) oxide at 200-350 °C, or dehydration of [FeBr2(H20)4]. The anhydrous compound is readily purified from FeBr3 by sublimation under nitrogen or in vacuo. It... 

Ferrous Sulfdte Titration. For deterrnination of nitric acid in mixed acid or for nitrates that are free from interferences, ferrous sulfate titration, the nitrometer method, and Devarda s method give excellent results. The deterrnination of nitric acid and nitrates in mixed acid is based on the oxidation of ferrous sulfate [7720-78-7] by nitric acid and may be subject to interference by other materials that reduce nitric acid or oxidize ferrous sulfate. Small amounts of sodium chloride, potassium bromide, or potassium iodide may be tolerated without serious interference, as can nitrous acid up to 50% of the total amount of nitric acid present. Strong oxidizing agents, eg, chlorates, iodates, and bromates, interfere by oxidizing the standardized ferrous sulfate. 

For ammonium bromide, another method involving reaction of an aqueous bromine solution and Hon filings has been used. The solution of ferrous and ferric bromide thus formed then reacts with ammonia to precipitate hydrated oxides of Hon. Ammonium bromide can be recovered by crystallization from the concentrated Hquor. 

Bromide ndIodide. The spectrophotometric determination of trace bromide concentration is based on the bromide catalysis of iodine oxidation to iodate by permanganate in acidic solution. Iodide can also be measured spectrophotometricaHy by selective oxidation to iodine by potassium peroxymonosulfate (KHSO ). The iodine reacts with colorless leucocrystal violet to produce the highly colored leucocrystal violet dye. Greater than 200 mg/L of chloride interferes with the color development. Trace concentrations of iodide are determined by its abiUty to cataly2e ceric ion reduction by arsenous acid. The reduction reaction is stopped at a specific time by the addition of ferrous ammonium sulfate. The ferrous ion is oxidi2ed to ferric ion, which then reacts with thiocyanate to produce a deep red complex. 

They also tried soln. of cupric chloride in acetic acid, formic acid, acetone, and methyl and ethyl alcohols. With 0-37, 0-62, and 0-925 litre of soln. with a mol of cupric bromide, 0-515, 0-120, and 0-000 litre of nitric oxide were respectively absorbed. They also tried soln. of cupric bromide in ethyl alcohol. E. Peligot found that nitric oxide is absorbed by aq. soln. of stannous salts (vide infra) and chromous salts. According to G. Chesneau, a soln. of ckromous chloride absorbs nitric oxide in the ratio CrCl2 NO=3 1, and the blue liquid becomes dark red. When heated, the nitric oxide is not expelled as in the case of ferrous salts, but the liquid becomes greenish-brown, and the nitric oxide is reduced to ammonia or hydroxylamine. The action of nitric oxide on soln. of chromous salts was also studied by V. Kohlschiitter, and J. Sand and O. Burger. 

Table II summarizes the data obtained by three analytical methods oxidation of iodide ion at pH 9, bromide ion at pH 2, and ferrous ion at pH 2. Data are reported for seven experiments conducted over a period of several days. Six aliquots were taken from each ozone solution, so that each value reported in the first three...

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