Barium nitrate

Barium nitrate, Ba(N03)2, is a colorless, crystalline material with a melting point of 865 K. Ba( NO2) 2 and O2 are producedin the low-temperature region, and Ba(N02) 2 decomposes to produce BaO, N O, and NO. in the high-temperature region according to  

The gaseous products, O2, NO, and NO2, all act as oxidizer components when barium nittate is mixed with fuel components. The decomposition process is endothermic, hence barium nittate cannot be burned without fuel components. 

Barium nitrate is a white, crystalline, nonhygroscopic material with a melting point of approximately 592°C. It is commonly used as the principal oxidizer in green flame compositions, gold sparklers, and in photoflash mixtures in combination with potassium perchlorate. At high reaction temperatures, barium nitrate decomposes according to 

This reaction corresponds to 30.6% available oxygen. At lower reaction temperatures, barium nitrate produces nitrogen oxides (NO and NO2) instead of nitrogen gas, as does strontium nitrate.  

Mixtures containing barium nitrate as the sole oxidizer are typically characterized by higher ignition temperatures relative to potassium nitrate and potassium chlorate compositions. The higher melting point and decomposition temperature of barium nitrate are primarily responsible for these higher ignition values. 

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Dissolve 15-0 g. of A.R. barium nitrate and 130 g. of A.R. cupric nitrate trihydrate in 450 ml. of water at 80°. Prepare a solution of sodium chromate by dissolving 89 g. of recrystallised sodium dichromate dihydrate in 200 ml. of water and adding 112 5 ml. of cone, ammonia solution (sp. gr. 0-90). Add the warm solution (80°) of nitrates in a thin stream, with stirring, to the sodium chromate solution (at 25°). Collect the orange precipitate by suction Bltration, wash it with two 50 ml. portions of 5fiter, drain well, and dry at 75-80° for 12 hours powder finely. 

Nantokite, see Copper(I) chloride Natron, see Sodium carbonate Naumannite, see Silver selenide Neutral verdigris, see Copper(H) acetate Nitre (niter), see Potassium nitrate Nitric oxide, see Nitrogen(II) oxide Nitrobarite, see Barium nitrate Nitromagnesite, see Magnesium nitrate 6-water Nitroprusside, see Sodium pentacyanonitrosylfer-rate(II) 2-water... 

Chromium Chromate. Chromium chromate treatment baths are acidic and made up from sources of hexavalent chromium and complex fluoride, fluorosiHcate, fluorozirconate, fluorotitanate, and siHcofluorides. Optional additional components added to accelerate coating rate are free fluoride, ferricyanide, and other metal salts such as barium nitrate. Conversion coating on aluminum precedes by the following reactions (2,3,17) ... 

Aluminum nitrate nonahydrate is prepared by dissolving aluminum or aluminum hydroxide in dilute nitric acid, and crystaUi2ing the product from the resulting aqueous solution. It is made commercially from aluminous materials such as bauxite. Iron compounds may be extracted from the solution with naphthenic acids (21) before hydrate precipitation. In the laboratory it is prepared from aluminum sulfate and barium nitrate. 

Barium nitrate is prepared by reaction of BaCO and nitric acid, filtration and evaporative crystallization, or by dissolving sodium nitrate in a saturated solution of barium chloride, with subsequent precipitation of barium nitrate. The precipitate is centrifuged, washed, and dried. Barium nitrate is used in pyrotechnic green flares, tracer buUets, primers, and in detonators. These make use of its property of easy decomposition as well as its characteristic green flame. A small amount is used as a source of barium oxide in enamels. 

Barium nitrite [13465-94-6] Ba(N02)2, crystallines from aqueous solution as barium nitrite monohydrate [7787-38-4], Ba(N02)2 H2O, which has yellowish hexagonal crystals, sp gr 3.173, solubihty 54.8 g Ba(NO2)2/100 g H2O at 0°C, 319 g at 100°C. The monohydrate loses its water of crystallization at 116°C. Anhydrous barium nitrite, sp gr 3.234, melts at 267°C and decomposes at 270 °C into BaO, NO, and N2. Barium nitrite may be prepared by crystallization from a solution of equivalent quantities of barium chloride and sodium nitrite, by thermal decomposition of barium nitrate in an atmosphere of NO, or by treating barium hydroxide or barium carbonate with the gaseous oxidiation products of ammonia. It has been used in diazotization reactions. 

The thermate mixture, composed of thermite and various additives, is used in igniter compositions for magnesium bombs. A number of such compositions have been developed. Three of these were Therm-8, Thermate-TH2 (formerly Therm-8-2), and Thermate-TH3 (formerly Therm-64-C). Therm-8 was the precursor of later, improved igniting formulations TH2 differs from Therm-8 in that TH2 contains no sulfur and slightly less thermite. TH3 was found to be superior to the others and thus adopted for use in the incendiary magnesium bomb. The wt % composition of TH3 is thermite, 68.7 barium nitrate, 29.0 sulfur, 2.0 and as a binder, oil, 0.3. 

Barium nitrate [10022-31-8] M 261.4, m 593"(dec). Crystd twice from water (4mL/g) and dried overnight at 110°. POISONOUS. 

Aluminium nitrate Ammonium persulphate Barium nitrate/peroxide Calcium nitrate/peroxide Cupric nitrate... 

Find the ionic strength of (i) 0.05 molal sodium sulfate (Na,SO ) solution, and (ii) 0.25 molal nitric acid (HNO,) and 0.4 molal barium nitrate (Ba(NO,) ) together ill one solution. 

Barium nitrate is added to a solution of0.025 M sodium fluoride. 

The procedure may be illustrated by the following simple experiment, which is a modification of the Gay Lussac-Stas method. The sodium chloride solution is added to the silver solution in the presence of free nitric acid and a small quantity of pure barium nitrate (the latter to assist coagulation of the precipitate). 

Barium sulphate exhibits a marked tendency to carry down other salts (see co-precipitation, Section 11.5). Whether the results will be low or high will depend upon the nature of the co-precipitated salt. Thus barium chloride and barium nitrate are readily co-precipitated. These salts will be an addition to the true weight of the barium sulphate, hence the results will be high, since the chloride is unchanged upon ignition and the nitrate will yield barium oxide. The error due to the chloride will be considerably reduced by the very slow addition of hot dilute barium chloride solution to the hot sulphate solution, which is constantly stirred that due to the nitrate cannot be avoided, and hence nitrate ion must always be removed by evaporation with a large excess of hydrochloric acid before precipitation. Chlorate has a similar effect to nitrate, and is similarly removed. 

TNT-Coated Barium Nitrate. 30g of TNT in ale soln is added to 270g of Ba nitrate in an ale slurry under agitation. The temp of the mixt is maintained at 80° and stirring is contd until most of the ale is evapd, The coated material is spread in a thin layer and air dried overnight. The Ba nitrate thus coated with 10% TNT is reduced to an intimate mixt by hand rolling and blending before use... 

Nitrate (as barium nitrate), max percent see footnote 1 see footnote 1 0.1... 

Tracer Compositions Containing Barium Nitrate , PATR 1254 (1943) 10) D. Hart,... 

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