Strontium sulphide

In some of the furnace reactions in which none of the substances are melted, as, for example, in the reduction of strontium sulphate to strontium sulphide by means of charcoal (see Preparation 20), the process probably takes place by virtue of a certain amount of gas which is continuously regenerated. A little... 

One of the most important sources of strontium is the mineral celestite, SrS04. By reduction with charcoal this can be converted into strontium sulphide,... 

Since copper sulphide is a far more insoluble substance than copper oxide, it follows that the few Cu++ ions from the latter unite with the S ions from the strontium sulphide to form copper sulphide, which precipitates continuously, while the... 

How could strontium chloride be prepared from strontium sulphide ... 

Give some other method by which strontium hydroxide could be obtained from strontium sulphide without the use of copper oxide. 

Strontium chloride might be prepared by treating strontium sulphide, the intermediate product in the last preparation, with hydrochloric acid, but, to avoid the hydrogen sulphide nuisance,... 

A few metallic sulphides are decomposed by water. The majority, however, are stable in the presence of water, and this fact is made use of in routine methods of qualitative analysis. Water decomposes strontium sulphide, yielding a mixture of hydroxide and hydrosulphide, which can be readily separated on account of their widely differing solubilities,10 the latter substance being the more soluble ... 

Hence, by extracting strontium sulphide with hot water and cooling the clear filtrate, pure crystalline strontium hydroxide is obtained. 

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,... 

Z 1 Niobium 1 Nitrate 1 Osmium 73 a. I Perchlorate Phenols u a o Platinum o 0. 1 5 u 1 Rhodium 1 Rubidium Ruthenium Scandium 1 Selenium Silver I Sodium 1 Strontium 1 Sulphate Sulphides, organic Sulphur dioxide 1 Tantalum 1 Tellurium 1 Thallium Thorium e H 1 Titanium a u ab a 1- I Uranium 1 Vanadium 1 Yttrium 1 Zinc Zirconium... 

Lead peroxide is even more active than the oxide. It reacts violently with sulphur and sulphides. When it is ground up with sulphur, the mixture combusts. With hydrogen sulphide, the reaction is very exothermic and causes peroxide to incandesce and hydrogen sulphide to combust. Finally, it reacts violently with calcium, strontium and barium sulphides on heating. 

Precipitation, in removing traces of impurities by precipitation it is necessary to include a material to act as a collector of the precipitated substance so as to facilitate its removal by filtration or decantation. Aqueous hydrofluoric acid can be freed from lead by adding 1ml of 10% strontium chloride per 100ml of acid, lead being co-precipitated as lead fluoride with the strontium fluoride. If the acid is decanted from the precipitate and the process repeated, the final lead content in the acid is less than 0.003 ppm. Similarly, lead can be precipitated from a nearly saturated sodium carbonate solution by adding 10% strontium chloride dropwise (l-2ml per 100ml), then filtering. (If the sodium carbonate is required as a solid, the solution can be evaporated to dryness in a platinum dish.) Removal of lead from potassium chloride uses precipitation as lead sulphide, followed, after filtration, by evaporation and recrystallisation of the potassium chloride. 

Chloride of Strontium ie in long, six-sided needles, deliquescent in moist air, and soluble in three-qnarter parts of cold water. It imparts an intense crimson color to flame. In alcohol it is also soluble. When heated, the chloride melts and becomes speedily anhydrous. Ignited in air, it loses chlorine and absorbs oxygen. The chloride of strontium is most easily prepared by dissolving the sulphide la water, and decomposing with hydrochloric acid. The symbol for the salt is SrCl, 6 HO. 

More rarely use is made for the same purpose of other substances such as strontium and calcium chromates, lead oxychloride (Cassel yellow), lead protoxide, arsenic sulphide (orpiment), stannic sulphide (mosaic gold), potassium cobaltinitrite (cobalt yellow), etc. 

C. Kubierschky 6 prepared a series of oxythiophosphates with only part of the oxygen of the normal phosphates replaced by sulphur. He said that acids decompose all thiophosphates hydrogen sulphide is evolved, and, in some cases, sulphur separates. Monothiophosphates give white precipitates with calcium, barium, and strontium salts, the dithiophosphates with barium and strontium salts, and the trithiophosphates with barium salts only. All thiophosphates yield precipitates with cadmium, copper, silver, and mercurous salts, which decompose after a time,... 

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