Alkaline-earth metal nitrates

The standard X-ray diffraction patterns for 57 compounds have been collected. The data comprise Miller indices, interplanar spacings, and lattice constants for inorganic compounds, solid solutions of alkali-metal halides and of alkaline-earth metal nitrates. ... 

The ruthenium catalyst without promoter almost is inactive, and the outlet ammonia concentration of 4% Ru/C catalyst Is only 0.13% under the conditions of 430°C, 10.0MPa and 10,000h For single promoter of Ru/C catalyst with the alkali metal, alkaline earth metal nitrate acts as the precursors of promoter respectively, the alkali metal and alkaline earth metal nitrate can Increase the activity of the ruthenium catalyst In different extent. The order of the Influence, alkali metal nitrates are CsNOs > RbNOa > KNO3 > NaNOa and that of alkali earth metal nitrate is Ba(N03)2 > Sr(N03)2 > Mg(N03)2 > Ca(N03)2. In the selected eight kinds of promoters, Ba(N03)2 and CsNOa are the most effective and the outlet ammonia concentration are 13.38% and 9.89% at 430°C, 10.0MPa and 10,000h respectively. 

For the most part it is true to say that the chemistry of the alkali and alkaline earth metal compounds is not that of the metal ion but rather that of the anion with which the ion is associated. Where appropriate, therefore, the chemistry of these compounds will be discussed in other sections, for example nitrates with Group V compounds, sulphates with Group VI compounds, and only a few compounds will be discussed here. 

Strontium has a valence of +2 and forms compounds that resemble the compounds of the other alkaline-earth metals (see Barium compounds Calcium compounds). Although many strontium compounds are known, there are only a few that have commercial importance and, of these, strontium carbonate [1633-05-2] SrCO, and strontium nitrate [10042-76-9], Sr(N03)2, are made in the largest quantities. The mineral celestite [7759-02-6], SrSO, is the raw material from which the carbonate or the nitrate is made. 

Alkali and alkaline earth metals, e.g. sodium, potassium lithium, magnesium, calcium, powdered aluminium Anhydrous ammonia Ammonium nitrate... 

Heating with the following solids, their fusions, or vapours (a) oxides, peroxides, hydroxides, nitrates, nitrites, sulphides, cyanides, hexacyano-ferrate(III), and hexacyanoferrate(II) of the alkali and alkaline-earth metals (except oxides and hydroxides of calcium and strontium) (b) molten lead, silver, copper, zinc, bismuth, tin, or gold, or mixtures which form these metals upon reduction (c) phosphorus, arsenic, antimony, or silicon, or mixtures which form these elements upon reduction, particularly phosphates, arsenates,... 

The intensity of a flare is largely determined by its temp, which in turn depends on the stability of the reaction products. In order to generate grey body radiation which encompasses the spectral sensitivity of the human eye (0.4— 0.74pm), 3000°K should be exceeded. Whereas this is possible using nitrates and perchlorates with alkaline earth metals as well as Zr, Ti and Hf (Ref 34) (H, C, B, Si and P form oxides which dissociate at high temps), in practice Mg and A1 are found to be best in terms of heat output, cost, and transparency to visible radiation... 

The alkaline earth metals can be detected in burning compounds by the colors that they give to flames. Calcium burns orange-red, strontium crimson, and barium yellow-green. Fireworks are often made from their salts (typically nitrates and chlorates, because the anions then provide an additional supply of oxygen) together with magnesium powder. 

To prepare alkali- or alkaline earth-modified zeolites or mesoporous moleeular sieves, identieal general methodologies are used. Thus, alkaline earth eation-exehanged zeolites are prepared by exehange of the zeolite in the sodium form in aqueous solution of alkaline earth metal salts, followed by washing and ealeination. Alkaline earth metal oxides loaded in zeolites are also prepared by impregnation of alkaline earth metal salts sueh as nitrates, aeetates, or ethoxides followed by ealeination (70,215,216). 

Sulphates of the alkali and alkaline earth metals, when heated with sulphur, are converted into sulphide, polysulphide and thiosulphate, with simultaneous formation of sulphur dioxide many other sulphates, e.g. those of copper, mercury, silver and lead, yield only sulphide.7 Other salts of the metals behave in a similar- manner, undergoing transformation into sulphides, the change being effected more readily with the salts of the heavy metals, many of which indeed react slowly with sulphur even at 100° C. in the presence of water.8 At 150° to 200° C. mercuric, stannic and ferric salts in aqueous solution are quantitatively reduced by sulphur mercurous, cupric, bismuth and lead salts arc slowly but quantitatively precipitated as sulphides. Nitrates, permanganates and iodates cause oxidation of the sulphur to sulphuric acid. 

For solutions containing sulphuric acid or a sulphate the reagent commonly applied is barium chloride, both when the test is to be qualitative and when quantitative. Precipitation is effected by the gradual addition of barium chloride to the boiling solution containing a little hydrochloric acid, but for the production of pure barium sulphate, and therefore in order to ensure accuracy, certain precautions must be observed.4 Nitrates, perchlorates, phosphates, tervalent metals and large quantities of salts of the alkali metals (particularly potassium) and of the alkaline earth metals are to be avoided, as they cause the precipitated barium sulphate to be rendered impure by occlusion of otherwise soluble substances.5 Such impurities may be accounted for partly by... 

Catactines, Expls patented in 1888 by Chandelon for use in grains or compressed. They consisted of mixts of one of the organic picrates or chloropicrates with sulfur, carbon and an oxygen carrier, such as a nitrate or chlorate of alkaline or alkaline-earth metals Refs 1 )Cundill(l889) in MP 5, 306(1892) 2) Daniel(1902), 118... 

As already known (Addison Logan 1964), anhydrous nitrates exhibit oxidizing properties. Their oxidizing activity increases from ionic nitrates with alkali and alkaline earth metal cations to covalent nitrates with transient metal cations. Oxidation reactions result in the formation of nitrogen-containing oxides. Depending on the kind of nitrate salt and on the reaction conditions, one of these oxides can be predominant. Organic substrates can evidently serve as reductant. 

Derivatisation-electron capture gas chromatography has been used to determine pg L 1 quantities of nitrite in water without interference from halides, nitrate, phosphate, sulphate, bicarbonate, ammonium and alkali metals and alkaline earth metals [792],... 

Although anhydrous nitrates of the alkali and alkaline earth metals have been known and widely used for a long time, the anhydrous nitrates of many other metals have been prepared only relatively recently. (See Figure 5.2.) The existence of some is still in doubt. Methods for preparing these nitrates have been described by Addison and Logan.6 These authors, as well as Hardy and Field,8 have also written extensive reviews of nitrate chemistry. Since not much has changed since they were written, only a brief summary of factors relevant to thermal decomposition is provided here. 

Copper(II) forms the most stable complexes with PEI. It is separable from other elements at lower pH values (5p). In contrast to the elements mentioned above, alkali and alkaline earth metals are not retained at any pH value by PEI. Neutral salts (e.g. sodium chloride or nitrate) influence the complexation of PEI (Fig. 4) [53]. 

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