Barium nitrate, reaction with

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. 

Barium sulphide has the usual dangerous reactions of sulphides (detonations with potassium chlorate and nitrate, combustion with phosphorus pentoxide). It catalyses the explosive combustion of dichlorine oxide. 

A pyrotechnic mixture of aluminium powder with potassium perchlorate, barium nitrate, potassium nitrate and water exploded after 24 h storage under water. Tests revealed the exothermic interaction of finely divided aluminium with nitrate and water to produce ammonia and aluminium hydroxide. Under the conditions prevailing in the stored mixture, the reaction would be expected to accelerate, finally involving the perchlorate as oxidant and causing ignition of the mixture. 

An aqueous solution of periodic acid, free from metal ions, may be prepared through the conversion of potassium metaperiodate to the slightly soluble barium dimesoperiodate, Ba2l207, which, through reaction with an equivalent amount of sulfuric acid, yields pure periodic acid.107 Hudson found that nitrate as an impurity in periodic acid gives rise to erroneous results in this field.239 ... 

Barium acetate converts to barium carbonate when heated in air at elevated temperatures. Reaction with sulfuric acid gives harium sulfate with hydrochloric acid and nitric acid, the chloride and nitrate salts are obtained after evaporation of the solutions. It undergoes double decomposition reactions with salts of several metals. For example, it forms ferrous acetate when treated with ferrous sulfate solution and mercurous acetate when mixed with mercurous nitrate solution acidified with nitric acid. It reacts with oxahc acid forming barium oxalate. 

Barium nitrate is prepared by the reaction of barium carbonate or barium sulfide with nitric acid ... 

Barium sulfide undergoes double decomposition reactions with hydrochloric acid and nitric acid, giving barium chloride and barium nitrate, respectively, when the solution is evaporated. 

The nitrates are considerably endothermic in their decomposition and therefore deliver less heat than chlorates or perchlorates, but they can be used with less fear of accidental ignition. Barium nitrate is often selected for white-light mixtures. The barium oxide (BaO) product formed upon reaction is a good, broad-range molecular emitter in the vapor phase (the boiling point of BaO is ca. 2000°C), and condensed particles of BaO found in the cooler parts of the flame are also good emitters of incandescent light. 

Sulphates and Chlorides. On shaking 2 gm. of zinc oxide with 20 re. of water and filtering, the acidulated filtrate should show no reaction on the addition of barium nitrate Hohilioiu and should acquire at most a. slight opalescent turbidity on the addition of silver nitrate solution. 

A mixture of lOg of iodine, 8.6g of potassium chlorate and 30ml of water are placed in a 100-ml Kjeldahl flask. One millilter of concentrated nitric acid is added and the mouth of the flask covered with an inverted beaker. The flask is now placed in a water bath at about 60°C when the evolution of chlorine just begins it is immediately withdrawn. The vigorous reaction that follows may be moderated somewhat by momentary immersion of the flask in cold water. When the reaction subsides, gentle heat is applied until the iodine has dissolved and the excess chlorine has been driven off. The liquid is washed into a beaker with 60ml of hot water and heated on the steam bath to dissolve any solid that may have formed. A solution of 10.5g of barium nitrate in 100ml of hot water is slowly added and the mixture is cooled in ice. The product is filtered off and washed several times with a little cold water. 

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