Barium iodide nitrate

D.ll Write the formula for the ionic compound formed from (a) zinc and fluoride ions (b) barium and nitrate ions (c) silver and iodide ions (d) lithium and nitride ions (e) chromium(IIl) and sulfide ions. 

Uranyl Iodide, UOglj, is prepared by adding barium iodide in slight excess to an ethereal solution of uranyl nitrate. It separates in red crystals which are deliquescent and unstable, losing iodine in the air, and in aqueous solution forming hydriodic acid and free iodine. ... 

Describe the effect on pH (increase, decrease, or no change) that results from each of the following additions (a) potassium acetate to an acetic acid solution (b) ammonium nitrate to an ammonia solution (c) sodium formate (HCOONa) to a formic acid (HCOOH) solution (d) potassium chloride to a hydrochloric acid solution (e) barium iodide to a hy-droiodic acid solution. 

Ammonium nitrate Ammonium nitrite Ammonium oxalate Ammonium salicylate Ammonium sulfate Ammonium sulfide Ammonium sulfite Ammonium thiosulfate Amyl acetate Amyl alcohol Amyl chloride Amyl mercaptan Amyl naphthalene Amyl nitrate Amyl nitrite Amyl phenol Aniline hydrdochloride Aniline sulfate Aniline sulfite Animal fats Animal oils Anthraquinone Antimony sulfate Antimony tribromide Antimony trichloride Antimony trioxide Aqua regia Arsenic oxide Arsenic trichloride Arsenic trioxide Arsenic trisulfide Ascorbic acid Barium carbonate Barium chlorate Barium chloride, aqueous Barium cyanide Barium hydroxide Barium iodide Barium nitrate Barium oxide Barium peroxide Barium salts Beet sugar liquors Benzaldehyde Benzene... 

The anions that are involved in secondary inorganic chemical analysis are, in general, carbonate, chloride, iodide, nitrate(V), sulfate(IV) and sulfate(VI). Students may be familiar with the carbonate ion from lower secondary science the reactions of the remaining anions have been introduced in the tests for gases or ionic precipitation (iodide). Silver nitrate(V) solution, barium chloride/nitrate(V) solution, lead(II) nitrate(V) solution and dilute acids are generally used to test for anions. 

Impurities in bromine may be deterrnined quantitatively (54). Weighing the residue after evaporation of a bromine sample yields the total nonvolatile matter. After removing the bromine, chloride ion may be deterrnined by titration with mercuric nitrate, and iodide ion by titration with thiosulfate water and organic compounds may be detected by infrared spectroscopy sulfur may be deterrnined turbidimetricaHy as barium sulfate and heavy metals may be deterrnined colorimetricaHy after conversion to sulfides. 

Students usually identify the existence of anions such as carbonate, iodide and sul-fate(VI) by adding a barium/silver(I)/lead(II) solution to the unknown, followed by a dilute acid or vice-versa in qualitative analysis practical work sessions and examinations. Mat r students had difficulty understanding the roles of the bar-ium/silver(I)/lead(II) solution and the dilute acid in the tests for anions. For example, 20% believed that the addition of aqueous barium nitrate(V) followed by dilute nitric(V) acid was to test for sulfate(VI) only. Another 25% believed that to test for a carbonate, acid had to be added directly to the unknown sample, while 20% believed that the addition of barium nitrate(V) invalidated the test for carbonates. When the students were asked the purpose of adding dilute nitric(V) acid following die addition of silver nitrate(V) solution (in one question) and lead(II) nitrate(V in another question) to the unknown solutions, 22% and 35%, respectively, indicated... 

Major constituents (greater than 5 mg/L) Minor constituents (O.Ol-lO.Omg/L) Selected trace constituents (less than 0.1 mg/L) Bicarbonate, calcium, carbonic acid, chloride, magnesium, silicon, sodium, sulfate Boron, carbonate, fluoride, iron, nitrate, potassium, strontium Aluminum, arsenic, barium, bromide, cadmium, chromium, cobalt, copper, gold, iodide, lead, Uthium, manganese, molybdenum, nickel, phosphate, radium, selenium, silver, tin, titanium, uranium, vanadium, zinc, zirconium... 

In one of J. S. Stas processes, the iodine was dissolved in a soln. of potassium iodide. The soln. was diluted with water until a precipitate began to form, and then three-fourths of the amount of water required to precipitate all the iodine were added. The separated iodine was washed free from potassium iodide by decantation, the crystals, after draining, were dried over calcium nitrate in vacuo, and then distilled twice from barium oxide. In another process, J. S. Stas purified the iodine by first treating the iodide with ammonia which converts about 95 per cent, of it into the explosive nitrogen iodide. The washed nitrogen iodide decomposes quietly when warmed with an excess of water. J. S. Stas thus describes the procedure ... 

The exceptional character o fluorine.—Fluorine has a little more individuality, so to speak, than the other three members of the family (1) There are no compounds of oxygen and fluorine (2) Chlorine, bromine, and iodine or the haloid acids show no signs of the remarkable effect of hydrofluoric acid and of fluorine on silicon (3) The solubilities of the sulphates, nitrates, and chlorides of barium, strontium, calcium, and magnesium decrease with increasing at. wt. of the metal, while the solubilities of the hydroxides increase the solubilities of the iodides, bromides, and chlorides... 

The detection and determination ot the perchlorates.—The perchlorates give no precipitates with silver nitrate or barium chloride soln. cone. soln. give a white crystalline precipitate with potassium chloride. Unlike all the other oxy-acids of chlorine, a soln. of indigo is not decolorized by perchloric acid, even after the addition of hydrochloric acid and they do not give the explosive chlorine dioxide when warmed with sulphuric acid unlike the chlorates, the perchlorates are not reduced by the copper-zinc couple, or sulphur dioxide. Perchloric acid can be titrated with —iV-alkali, using phenolphthalein as indicator. The perchlorates can be converted into chlorides by heat and the chlorides determined volumetrically or gravimetrically they can be reduced to chloride by titanous sulphate 28 and titration of the excess of titanous sulphate with standard permanganate they can be fused with zinc chloride and the amount of chlorine liberated can be measured in terms of the iodine set free from a soln. of potassium iodide and they can be... 

Experiments showed that minute amounts of mercury vapour in the atmosphere are sufficient to discolour a blue iodide-starch paper, e.g. on heating a mixture of 0.2 g of barium nitrate with 0.8 mg of mercury to a temperature of 80°C there is immediate discoloration of the paper. 

Anhydrous hydrazine dssolves many salts, thus, 100 parts of solvent at 12-5°-13° dissolve 12-2 parts of sodium chloride 8 5, of potassium chloride 56-4, of potassium bromide 135-7, of potassium iodide 26-6, of sodium nitrate 21-7, of potassium nitrate and 814, of barium nitrate. The hydrazine seemed to unite with sodium chloride with a warm soln. of ammonium chloride, ammonia is evolved, and in the cold, there seems to be a state of equilibrium a complex salt seems to be formed with lead nitrate. An aq. soln. of hydrazine hydrate also dissolves a number of salts, potassium bromide and iodide, ammonium sulphate, potassium cyanide, barium nitrate, magnesium sulphate, etc. According to T. W. B. Welsh and H. J. Broderson, the solubility of the metal haloids seems to... 

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