Barium nitrate, reaction with potassium

Strongly exothermal reaction with potassium nitrate, barium carbonate... 

Barium sulphate is not a strong oxidant yet it can give rise to a very violent thermite reaction when it is heated in the presence of a very electropositive metal. This applies to aluminium for which an accident was described. In addition, there was an accident which involved a mixture of this sulphate with red phosphorus although the latter had been previously treated with potassium nitrate and calcium silicide. 

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 ... 

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 The flask is now placed in a water bath at about 60°C when the evolution of chlorine just begins it is immediately withdrawn.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. 

When two solutions are mixed, an insoluble substance sometimes forms that is, a solid forms and separates from the solution. Such a reaction is called a precipitation reaction and the solid that forms is called a precipitate. For example, a precipitation reaction occurs when an aqueous solution of potassium chromate, K2Cr04(aq), which is yellow, is mixed with a colorless aqueous solution containing barium nitrate, Ba(N03)2(aq). As shown in Fig. 4.12, when these solutions are mixed, a yellow solid forms. What is the equation that describes this chemical change To write the equation we must know the identities of the reactants and products. The reactants have already been described K2Cr04(aq) and Ba(N03)2(tf<7). Is there some way we can predict the identities of the products In particular, what is the yellow solid ... 

In this section we will consider the types of equations used to represent reactions in solution. For example, when we mix aqueous potassium chromate with aqueous barium nitrate, a reaction occurs to form a precipitate (BaCr04) and dissolved potassium nitrate. So far we have written the molecular equation for this reaction ... 

Explosive reaction with chlorosulfuric acid, hydroiodic acid, magnesium perchlorate, chromyl chloride. Forms sensitive explosive mixtures with metal halogenates (e.g., chlorates, bromates, or iodates of barium, calcium, magnesium, potassium, sodium, zinc), ammonium nitrate, mercury(1) nitrate, silver nitrate, sodium nitrate, potassium permanganate. Violent reaction or ignition with alkalies + heat, fluorine, chlorine, liquid bromine, antimony pentachloride. Reacts with hot alkalies or hydroiodic acid to form... 

It has been involved in many industrial explosions. Explodes on contact with aluminum + barium nitrate + potassium nitrate + water. Forms explosive mixtures with aluminum powder + titanium dioxide, ethylene glycol (240°C), cotton lint (245°C), furfural (270°C), lactose, metal powders (e.g., aluminum, iron, magnesium, molybdenum, nickel, tantalum, titanium), sulfur, titanium hydride. Reaction with ethanol + heat forms the explosive ethyl perchlorate. Violent reaction or ignition under the proper conditions with aluminum + aluminum fluoride, barium chromate + mngsten or titanium, boron + magnesium + silicone rubber, ferrocenium diammine-tetrakis(thiocyanato-N) chromate(l —), potassium hexacyanocobaltate(3—), A1 +... 

The ammonium nitrate which is produced by above reaction is quite hygroscopic. Therefore if a composition which contains ammonium perchlorate comes in contact with another composition which contains potassium nitrate such as black powder, a wet layer of ammonium nitrate occurs between the two compositions and causes misfire. With barium nitrate this double decomposition does not occur, and a mixture of barium nitrate and ammonium perchlorate is allowed in the preparation of firework compositions. 

For the reaction of potassium sulfate with barium nitrate, the net ionic equation shows that aqueous barium and sulfate ions join to form solid, insoluble barium sulfate. 

Samples of dry solid potassium sulfate, K2SO4, and dry solid barium nitrate, Ba(N03)2, can be mixed with no appreciable reaction occurring for several years. But if aqueous solutions of the two are mixed, a reaction occurs rapidly, forming a white precipitate of barium sulfate. 

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