Ferrous bromide iodide

Incompal. Alcohol, arsenites, bromides, iodides, hydrochloric acid, charcoal organic substances generally ferrous or mercurous salts, hypophosphites, hyposulfites, sulfites, peroxides, oxalates. 

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. 

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. 

Elemental composition K 28.22%, Cl 25.59%, and 0 46.19%. An aqueous solution is analyzed for potassium by AA, ICP, and other methods (see Potassium). Perchlorate ion may be analyzed by ion chromatography or a liquid-membrane electrode. Iodide, bromide, chlorate, and cyanide ions interfere in the electrode measurement. Alternatively, perchlorate ion may be measured by redox titration. Its solution in 0.5M H2SO4 is treated with a measured excess standard ferrous ammonium sulfate. The excess iron(II) solution is immediately titrated with a standard solution of potassium dichromate. Diphenylamine sulfuric acid may be used as an indicator to detect the end point ... 

Now that we have run through the two simple processes. Its time to move onto something a little more advanced. To review what we have learned so far, look at the two similarities between the two procedures we have done. In the first procedure we made ferrous chloride by electrolyzing a salt solution using an iron anode. In the second procedure we used a copper anode, and got cupric chloride. Now, you should remember that if we replaced the copper anode with zinc for example, we would get zinc chloride. Note Any metal can be used with the exception of lead, platinum, and a few others we need not discuss at this point. If you want, try it with aluminum, zinc, nickel, chromium, or magnesium to get the respective chlorides. Note The sodium chloride can be replaced with sodium bromide, or sodium iodide to make the corresponding bromides and iodides. 

Sodium chloride Sodium bromide Sodium iodide Sodium sulphate Sodium silicate Potassium sulphate Lithium chloride Calcium carbonate Calcium sulphate Magnesium sulphate Manganous carbonate Ferrous carbonate. Aluminium phosphate Ammonium nitrate Organic matter... 

Ammonium iodide, NH4I.—The iodide is formed by methods analogous to those applicable to the bromide.3 It is also a product of the decomposition of nitrogen iodide in presence of water or ammonium hydroxide.4 It is best prepared by addition of alcohol to an aqueous solution of potassium iodide and ammonium sulphate in equimolecular proportions, potassium sulphate crystallizing and ammonium iodide remaining dissolved.5 It can also be prepared by the interaction of ferrous iodide and ammonium carbonate, and by that of ammonium hydroxide and iodine in presence of hydrogen peroxide 6... 

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...

If the driving potential for the ozone against bromide at pH 2.0 is inadequate or more time is needed for the reaction, a slight excess of ozone may be present when the iodide is added for the titration. When chloride is added to the ozone solution at pH 2.0, the ozone odor persists in a closed reaction vessel for an hour, as discussed by Yeatts and Taube 16). After the chloride has been added at pH 0.0, there is a greater excess of iodine than that calculated from the ferrous-ferric system ozone may have been present at the time of the iodine addition. 

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