1911 Encyclopædia Britannica/Sulphur
SULPHUR [symbol S, atomic weight 32·07 (O＝16)], a non-metallic chemical element, known from very remote times and regarded by the alchemists, on account of its inflammable nature, as the principle of combustion; it is also known as brimstone (q.v.). The element occurs widely and abundantly distributed in nature both in the free state and in combination. Free or native sulphur, known also as “virgin sulphur,” occurs in connexion with volcanoes and in certain stratified rocks in several modes, viz. as crystals, and as stalactitic, encrusting, reniform, massive, earthy and occasionally pulverulent forms as “sulphur meal.” It seems rather doubtful whether the unstable monoclinic modification of sulphur (β-sulphur) is ever found in a native state.
The crystals belong to the orthorhombic system, and have usually a pyramidal habit (fig.), but may be spheroidal or tabular. Twins are rare. The cleavage is imperfect, but there is a well-marked conchoidal fracture. The hardness ranges from about 1 to 2, and the sp.gr. from 1·9 to 2·1. Crystals of sulphur are transparent or translucent and highly refractive with strong birefringence; they have a resinous or slightly adamantine lustre, and present the characteristic sulphur-yellow colour. Impurities render the mineral grey, greenish or reddish, bituminous matter being often present in the massive varieties. Sulphur containing selenium, such as occurs in the isle of Vulcano in the Lipari Isles, may be orange-red; and a similar colour is seen in sulphur which contains arsenic sulphide, such as that from La Solfatara near Naples. The presence of tellurium in native sulphur is rare, but is known in certain specimens from Japan.
Volcanic sulphur usually occurs as a sublimate around or on the walls of the vents, and has probably been formed in many cases by the interaction of sulphur dioxide and hydrogen sulphide. Sublimed sulphur also results from the spontaneous combustion of coal seams containing pyrites. Deposits of sulphur are frequently formed by the decomposition of hydrogen sulphide, on exposure to the atmosphere: hence natural sulphureous waters, especially hot springs, readily deposit sulphur. The reduction of sulphates to sulphides by means of organic matter, probably through the agency of sulphur-bacteria, may also indirectly furnish sulphur, and hence it is frequently found in deposits of gypsum. Free sulphur may also result from the decomposition or pyrites, as in pyritic shales and lignites, or from the alteration of galena: thus crystals of sulphur occur, with angle site, in cavities in galena at Monteponi near Iglesias in Sardinia; whilst the pyrites of Rio Tinto in Spain sometimes yield sulphur on weathering. It should be noted that the oxidation of sulphur itself by atmospheric influence may give rise to sulphuric acid, which in the presence of limestone will form gypsum: thus the sulphur-deposits of Sicily suffer alteration of this kind, and have their outcrop marked by a pale earthy gypseous rock called briscale.
Some of the most important deposits of sulphur in the world are worked in Sicily, chiefly in the provinces of Caltanisetta and Girgenti, as at Racalmuto and Cattolica; and to a less extent in the provinces of Catania, Palermo (Lercara) and Trapani (Gibellina). The sulphur occurs in Miocene marls and limestone, associated with gypsum, Celestine, aragonite and Calcite. It was formerly believed that the sulphur had a volcanic origin, but it is now generally held that it has either been reduced from gypsum by organic agencies, or more probably deposited from sulphur-bearing waters. Liquid occasionally enclosed in the sulphur and gypsum has been found by O. Silvestri and by C. A. H. Sjogren to contain salts like those of sulphur-springs. An important zone of sulphur-bearing Miocene rocks occurs on the east side of the Apennines, constituting a great part of the province of Forli and part of Pesaro. Cesena and Perticara are well-known localities in this district, the latter yielding crystals coated with asphalt. Sulphur is occasionally found crystallized in Carrara marble; and the mineral occurs also in Calabria. Fine crystals occur at Conil near Cadiz; whilst in the province of Teruel in Aragon, sulphur in a compact form replaces fresh-water shells and plant-remains, suggesting its origin from sulphur-springs. Nodular forms of sulphur occur in Miocene marls near Radoboj in Croatia, and near Swoszowic, south of Cracow. Russia possesses large deposits of sulphur in Daghestan in Transcaucasia, and in the Transcaspian steppes. Important deposits of sulphur are worked at several localities in Japan, especially at the Kosaka mine in the province of Rikuchiu, and at Yatsukoda-yama, in the province of Mutsu. Sulphur is worked in Chile and Peru. A complete list of localities for sulphur would include all the volcanic regions of the world. In the United States, sulphur occurs in the following states, in many of which the mineral has been worked: Louisiana (q.v.), Utah, Colorado, California, Nevada, Alaska, Idaho, Texas and Wyoming. The Rabbit Hole sulphur-mines are in Nevada, and a great deposit in Utah occurs at Cove Creek, Beaver county. In the British Islands native sulphur is only a mineralogical rarity, but it occurs in the Carboniferous Limestone of Oughterard in Co. Galway, Ireland.[1]
In combination the element chiefly occurs as metallic sulphides and sulphates. The former are of great commercial importance, being, in most cases, valuable ores, e.g. copper pyrites (copper), galena (lead), blende (zinc), cinnabar (mercury), &c. Of the sulphates we notice gypsum and anhydrite (calcium), barytes (barium) and kieserite (magnesium). Gaseous compounds, e.g. sulphur dioxide and sulphuretted hydrogen, are present in volcanic exhalations (see Volcano) and in m-any mineral waters. The element also occurs in the animal and vegetable kingdoms. It is present in hair and wool, and in albuminous bodies; and is also a constituent of certain vegetable oils, such as the oils of garlic and mustard. There is, in addition, a series of bacteria which decompose sulphureous compounds and utilize the element thus liberated in their protoplasm (see Bacteriology).
Extraction.—As quarried or mined free sulphur is always contaminated with limestone, gypsum, clay, &c.; the principle underlying its extraction from these impurities isone of simple liquation, i.e. the element is melted, either by the heat of its own combustion or other means, and runs off from the earthy residue.
In the simplest and crudest method, as practised in Sicily, a mass of the ore is placed in a hole in the ground and fired; after a time the heat melts a part of the sulphur which runs down to the bottom of the hole and is then ladled out. This exceptionally wasteful process, in which only one-third of the sulphur is recovered, has been improved by conducting the fusion in a sort of kiln. A semicircular or semi-elliptical pit (calcarone) about 33 ft. in diameter and 8 ft. deep is dug into the slope of a hill, and the sides are coated with a wall of stone. The sole consists of two halves slanting against each other, the line of intersection forming a descending gutter which runs to the outlet. This outlet having been closed by small stones and sulphate of lime cement, the pit is filled with sulphur ore, Which is heaped up considerably beyond the edge of the pit and covered with a layer of burnt-out ore. In building up the heap a number of narrow vertical passages are left to afford a draught for the fire. The ore is kindled from above and the fire so regulated (by making or unmaking air-holes in the covering) that, by the heat produced by the combustion of the least sufficient quantity of sulphur, the rest is liquefied. The molten sulphur accumulates on the sole, whence it is from time to time run out into a square stone receptacle, from which it is ladled into damp poplar-wood moulds and so brought into the shape of truncated cones weighing 110 to 130 ℔ each. These cakes are sent out into commerce. A calcarone with a capacity of 28,256 cub. ft. burns for about two months, and yields about 200 tons of sulphur. The yield is about 50%. The immense volumes of sulphurous acid evolved give rise to many complaints; all the minor pits suspend work during the summer to avoid destruction of the crops. A calcarone that is to be used all the year round must be at least 220 yds. from any inhabited place and T10 yds. from any held under cultivation.
More efficient is the Gill kiln which uses coke as a fuel. The kiln consists of two (or more) connected cells which are both charged with the ore. The first cell is heated and the products of combustion are led into the second cell where they give up part of their heat to the contained ore, so that by the time the first cell is exhausted the mass in the second cell is at a sufficiently high temperature to ignite spontaneously when air is admitted. Other methods have been employed, but with varying commercial success. For example, in the Gritti and Orlando processes the ore is charged into retorts and the fusion effected by superheated steam, the sulphur being run off as usual; or as was suggested by R. E. Bollman in 1867 the ore may be extracted by carbon bisulphide.
Crude sulphur, as obtained from kilns, contains about 3% of earthy impurities, and consequently needs refining. The fol owing apparatus (invented originally by 1 ichel of Marsei les and improved subsequently by others) enables the manufacturer to produce either of two forms of “ refined ” sulphur which commerce demands. It consists of a large stone chamber which communicates directly with two slightly slanting tubular retorts of iron. The retorts are charged with molten sulphur from an up er reservoir, which is kept at the requisite temperature by means ofithe lost heat of the retort tires. The chamber has a safety value at the top of its vault, which is so balanced that the least surplus pressure from within sends it up. The first puff of sulphur vapour which enters the chamber takes tire and converts the air of the chamber into a mixture of nitrogen and sulphur dioxide. The next following instalments of vapour, getting diffused throughout a large mass of relatively coldgas. condense into a kind of “ snow, ” known in commerce and valued as “ Bowers of sulphur" (jlores sulphur is). By conducting the distillation slowly, so that the temperature within the chamber remains at a sufficiently low degree, it is possible to obtain the whole of the product in the form of “flowers.” If compact (“roll ”) sulphur is wanted the distillation is made to go on at the quickest admissible rate. The temperature of the interior of the chamber soon rises to more than the fusing-point of sulphur (113° C.), and the distillate accumulates at the bottom as a liquid, which is tapped off from time to time to be cast into the customary form of rods.
The Louisiana deposits are worked by a process devised by Herman Frasch in 1891. It consists in sinking a bore-hole, after the manner of a petroleum well, and letting in four pipes centrally arranged, the outer pipe being 10 in. in diameter, the next 6 in., the next 3 in. and the innermost 1 in. The operation consists in forcing down the 3-in. pipe superheated steam at 330° F. to melt the sulphur. Compressed air is now driven down the I-in. pipe and bubbles into the melted sulphur and water; the specific gravity of which is greatly diminished, so that it rises to the surface through the outer pipes; it is then run off to settling tanks. The sulphur so obtained is 98% pure.
In some places sulphur is extracted from iron pyrites by one of two methods. The pyrites is subjected to dry distillation from out of iron or fire-clay tubular retorts at a bright red heat. One-third of the sulphur is volatilized—3FeS2＝Fe3S4+2S-and obtained as a distillate. The second method is analogous to the calcarone method of liquation: the ore is placed in a limekiln-like furnace over a mass of kindled fuel to start a partial combustion of the mineral, and the process is so regulated that, by the heat generated, the unburnt part is decomposed with elimination of sulphur, which collects in the molten state on an inverted roof-shaped sole below the furnace and is thence conducted into a cistern. Such pyrites sulphur is usually contaminated with arsenic, and consequently is of less value than Sicilian sulphur, which is characteristically free from this impurity.
Large quantities are also recovered from alkali waste (see Alkali Manufacture); another source is the spent oxide of gas manufacture see Gas.
The substance known as “milk of sulphur” (lac sulphuris) is very finely divided sulphur produced by the following, or some analogous, chemical process. One part of quicklime is slaked with 6 parts of water, and the paste produced diluted with 24 parts of water: 2·3 parts of flowers of sulphur are added; and the whole is boiled for about an hour or longer, when the sulphur dissolves. The mixed solution of poiysulphides and thiosulphate of calcium thus produced is clarified, diluted largely, and then mixed with enough of pure dilute hydrochloric acid to roduce a feebly alkaline mixture when sulphur is precipitated. The addition of more acid would produce an additional supply of sulphur (by the action of the H2S2On on the dissolved H2S); but this thiosulphate sulphur is yellow and compact, while the polysulphide part has the desired qualities, forming an extremely line, almost white, powder. The precipitate is washed, collected, and dried at a very moderate heat.
Properties.-Sulphur exists in several allotropic modifications, but before considering these systematically we will deal with the properties of ordinary (or rhombic) sulphur. Commercial sulphur forms yellow crystals which melt at 113° and boil at 444·53° C. under ordinary pressure (H. L. Callendar, Chem. News, 1891, 63, p. 1); just above the boiling point the vapour is orange-yellow, but on continued heating it darkens, being deep red at 500°; at higher temperatures it lightens, becoming straw-yellow at 650°. These colour changes are connected with a dissociation of the molecules. At 524° Dumas deduced the structure S5 from vapour-density determinations, whilst for the range 860° to 10400, Sainte-Claire Deville and Troost deduced the formula Sz. Biltz (Ben, 1888, 21, p. 2013; 1901, 34, p. 2490) showed that the vapour density decreased with the temperature, and also depended on the pressure. G. Preuner and W. Schupp (Zeit. phys. Chem., 1909, 69, p. 157), in a study of the dissociation isotherms over 300°–850°, detected molecules of S8, S6 and S2, whilst S1 appears to exist below pressures of 30 mm. Boiling and freezing-point determinations of the molecular weight in solution indicate the formula S8. The density of solid sulphur is 2·062 to 2·070, and the specific heat 0·1712; it is a bad conductor of electricity and becomes negatively electrified on friction. It ignites in air at 363° and in oxygen at 275–280° (H. Moissan, Compt. rend., 1903, 137, p. 547), burning with a characteristic blue flame and forming much sulphur dioxide, recognized by its pungent odour. At the same time a little trioxide is formed, and, according to Hempel (Ber., 1890, 23, p. 1455), half the sulphur is converted into this oxide if the combustion be carried out in oxygen at a pressure of 40 to 50 atmospheres. Sulphur also combines directly with most of the elements to form sulphides. The atomic weight was determined by Berzelius, Erdmann and Marchand, Dumas and Stas. Thomsen (Zeit. phys. Chem., 1894, 13, p. 726) obtained the value 32·0606.
Allotropic Modifications.—Sulphur assumes crystalline, amorphous and (possibly) colloidal forms. Historically the most important are the rhombic (Sα) and mono clinic (Sβ)) forms, discussed by E. Mitscherlich in 1822 (see Ann. chim. phys., 1823, 24, p. 264). The transformations of these two forms are discussed in Chemistry: Physical. Rhombic sulphur may be obtained artificially by slowly crystallizing a solution of sulphur in carbon bi sulphide, or, better, by exposing pyridine saturated with sulphuretted hydrogen to atmospheric oxidation (Ahrens, Ber., 1890, 23, p. 2708). It is insoluble in water,[2] but readily soluble in carbon bi sulphide, sulphur chloride and oil of turpentine. The common mono clinic variety is obtained by allowing a crust to form over molten sulphur by partially cooling it, and then breaking the crust and pouring off the still liquid portion, whereupon the interior of the vessel will be found coated with long needles of this variety. Like S., it is soluble in carbon bi sulphide. Three other mono clinic forms have been described. By acting upon a solution of sodium hyposulphite with potassium bisulphate, Gernez (Compt. rend., 1884, 98, p. 144) obtained a form which he termed nacré (or pearly) sulphur; the same modification was obtained by Sabatier (ibid., 1885, 100, p. 1346) on shaking hydrogen per sulphide with alcohol or ether. It is readily transformed into rhombic sulphur. Another form, mixed with the variety just described, is obtained by adding 3 to 4 volumes of alcohol to a solution of ammonium sulphide saturated with sulphur and exposing the mixture to air at about 5°. Engel’s monoclinic form (Compt. rend., 1891, 112, p. 866) is obtained by mixing a solution of sodium hyposulphite with double its volume of hydrochloric acid, filtering and extracting with chloroform; the extract yielding the variety on evaporation. A triclinic form is claimed to be obtained by Friedel (Bull. soc. chim., 1879, 32, p. 14) on subliming ordinary sulphur. Amorphous sulphur or Sγ, exists in two forms, one soluble in carbon bi sulphide, the other insoluble. Milk of sulphur (see above), obtained by decomposing a poly sulphide with an acid, contains both forms. The insoluble variety may also be obtained by decomposing sulphur chloride with water and by other reactions. It gradually transforms itself int' rhombic sulphur.
The colloidal sulphur, Sδ, described by Debus as a product of the interaction of sulphuretted hydrogen and sulphur dioxide in aqueous solution, is regarded by Spring (Rec. hav. chim., 1906, 25, p. 253) as a hydrate of the formula S8-H20. The “blue sulphur,” described by Orloli, has been investigated by Paterno and Mazzucchelli (Abs. Journ. Chem. Soc., 1907, 451).
Molten Sulphur.—Several interesting phenomena are witnessed when sulphur is heated above its melting point. The solid melts to a pale yellow liquid which on continued heating gradually darkens and becomes more viscous, the maximum viscosity occurring at 180°, the product being dark red in colour. This change is associated with a change in the spectrum (N. Lockyer). On continuing the heating, the viscosity diminishes while the colour remains the same. If the viscous variety be rapidly cooled, or the more highly heated mass be poured into water, an elastic substance is obtained, termed plastic sulphur. This substance, however, on standing becomes brittle. The character of molten sulphur has been mainly elucidated by the researches of A. Smith and his collaborators. Smith (Abs. Journ. Chem. Soc., 1907, ii. 2o, 451, 757) regards molten sulphur as a mixture of two isomers Si and SH in dynamic equilibrium, SA being light in colour and mobile, and Su dark and viscous. At low temperatures S, predominates, but as the temperature is raised Sa increases; the transformation, however, is retarded by some gzses, e.g. sulphur dioxide and hydrochloric acid, and accelerated by others, e.g. ammonia. The solid derived from Si is crystalline and soluble in carbon bi sulphide, that from Sa is amorphous and insoluble. As to the formation of precipitated sulphur, Smith considers that the element first separates in the liquid Sa condition, which is transformed into S, and finally into Sa; the insoluble (in carbon bi sulphide) forms arise when little of the S, r has been transformed; whilst the soluble consist mainly of Sa. Similar views are adopted by H. Erdmann (/inn., 1998, 362, p. 133), but he regards S, i as the polymer S3, analogous to ozone 03; Smith, however, regards S, as SB.
Compounds.
Sulphuretted hydrogen, H2S, a compound first examined by C. Scheele, may be obtained by heating sulphur in a current of hydrogen, combination taking place between 200° C. and 358° C., and being complete at the latter temperature, dissociation taking place above this temperature (M. Bodenstein, Zeit. phys. Chem., 1899, 29, p. 315); by heating some metallic sulphides in a current of hydrogen; by the action of acids on various metallic sulphides (ferrous sulphide and dilute sulphuric acid being most generally employed); by the action of sulphur on heated paraffin wax or vaseline, or by heating a solution of magnesium sulphydrate. It is also produced during the putrefaction of organic substances containing sulphur and is found among the products obtained in the destructive distillation of coal. To obtain pure sulphuretted hydrogen the method generally adopted consists in decomposing precipitated antimony sulphide with concentrated hydrochloric acid. As an alternative, H. Moissan (Comp. fend., 1903, 137, p. 363) Condenses the gas by means of liquid air and fraction ates the product. Sulphuretted hydrogen is a colourless gas possessing an extremely offensive odour. It acts as a strong poison. It burns with a pale blue flame, forming sulphur dioxide and water. It is moderately soluble in water, the solution possessing a faintly acid reaction. This solution is not very stable, since on exposure to air it slowly oxidizes and becomes turbid owing to the gradual precipitation of sulphur. The gas is much more soluble in alcohol. It forms a hydrate of composition HQS-7H2O. (De Forcrand, Compt. fend., 1888, IO6, p. 1357.) The gas may be liquefied by a pressure of about I7 atmospheres, the liquid so obtained boiling at -61-8° C.; and by further cooling it yields a solid, the melting point of which is given by various observers as -82° to -86°'C. (see Ladenburg, Bef., 1900, 33, p. 637). It is decomposed by the halogens, with liberation of sulphur. Concentrated sulphuric acid also decomposes it: H2504-{-H¢»S=2H2O+SO2+S. It combines with many metals to form sulphides, and also decomposes many metallic salts with consequent production of sulphides, a property which renders it extremely useful in chemical analysis. It is frequently used as a reducing agent: in acid solutions it reduces ferric to ferrous salts, arsenates to arsenites, permanganate's to manganous salts, &c., whilst in alkaline solution it converts many organic nitro compounds into the corresponding amino derivatives. Oxidizing agents rapidly attack sulphuretted hydrogen, the primary products of the reaction being- water and sulphur.
By the action of dilute hydrochloric acid on metallic poly sulphides, an oily product is obtained which C. L. Berthollet considered to be H3S5. L. Thénard, on the other hand, favoured the formula HQSQ. It was also examined by W. Ramsay (Journ. Chem. Soc., 1874, 12, p. 857). Hofmann, who obtained it by saturating an alcoholic solution of ammonium sulphide with sulphur and mixing the product with anialcoholic solution of strychnine, considered the resulting product to be HZS3; while P. Sabatier by fractionating the crude product in vacuo obtained an oil which boiled between 60° and 85° C. and possessed the composition H4S5.
Several halogen compounds of sulphur are known, the most stable of which is sulphur fluoride, SF5, which was first prepared by H. Moissan and Lebeau (Compt. fend., 1900, 130, p. 865) by fractionally distilling the product formed in the direct action -of fiuorine on sulphur. It is tasteless, colourless and odourless gas, which is exceedingly stable and inert. It may be condensed and yields a solid which melts at -55° C. Sulphuretted hydrogen decomposes it with formation of hydrofluoric acid and liberation of sulphur. Sulphur chloride, S2Cl2, is obtained as a by-product in the manufacture of carbon tetrachloride from carbon bi sulphide and chlorine, and may also be prepared on the small scale by distilling sul hur in a chlorine gas, or by the action of sulp-hur on sulphuryl ciiloride in the presence of aluminium chloride (O. Ruff). It is an amber coloured, fuming liquid possessing a very unpleasant irritating smell. It boils at 139° C. and is solid at -80° C. It is soluble in carbon bi sulphide and in benzene. It is gradually decomposed by water: 2S¢Cl2 + 3H2O = 4HCl + QS + HZSQO3, the thiosulphuric acid produced in the primary reaction radually decomposing into water, sulphur and sulphur dioxide. Sulphur chloride dissolves sulphur with great readiness and is consequently used largely for vulcanizing rubber; it also dissolves chlorine. The chloride SCl2 according to the investigations of 0. Ruff and Fischer (Bern, 1903, 36, p. 418) did not' appear to exist, but E. Beckmann (Zeit. phys. Chem., 1909, 42, p. 1839) obtained it by distilling the product of the interaction of chlorine and S2Cl2 at low pressures. The tetrachloride, SCl4, isformed by saturating S¢Cl2 with chlorine at -"22° C. (Michaelis, Ann., 1873, 170, p. 1). It is a yellowish-brown liquid which dissociates rapidly with rise of temperature. On cooling it solidifies to a crystalline mass which fuses at -80° C. (Ruff, ibid.). Water decomposes it violently with formation of hydrochloric and sulphurous acids. Sulphur bromide, S2Br2, is a dark red liquid which boils with decomposition at about 200° C. The products obtained by the action of iodincon sulphur are probably mixtures, although E. Mclvor (Chem. News, 1902, 86, p. 5) obtained a substance of composition S312 (which in all probability is a chemical individual) as a reddish-coloured powder by the action of sulpliuretted hydrogen on a solution of iodine trichloride.
Four oxides of sulphur are known, namely sulphur dioxide, SO2, sulphur trioxide, SCs, sulphur sesquioxide, SQO3, and per sulphuric an hydride, S-:O-1. The dioxide has been known since the earliest times and is found as a naturally occurring product, in the gaseous exhalations of volcanoes and in solution in some volcanic springs. It was first collected in the pure condition by ]. Priestley in 1775 and its composition determined somewhat later by A. L. Lavoisier. It is formed when sulphur is burned in air or in oxygen, or when many metallic sulphides are roasted. It may also be obtained by heating carbon, sulphur and many metals with concentrated sulphuric acid: C + 2H2SO4 = ZSOQ -{- C02 -|- 2H2O; S -l- 2H2S04= 3502 -I-2H2O; Cu +2H¢S04 = S02 + CuSO4 -}- 2H2O; and by decomposing a sulphite, a thiosulphate or a thionic acid with a dilute mineral acid. It is a colourless gas which possesses a characteristic suffocating odour. It does not burn, neither does it support combustion. It is readily soluble in alcohol and in water, the solution in water possessing a strongly acid reaction. It is easily liquefied, the liquid boiling at -8° C., and it becomes crystalline at -72-7° C. (Walden, Zeit. phys. Chem., 1902, 43, p. 432). Walden (ibid.) has shown that certain salts dissolve in liquid sulphur dioxide forming additive compounds, two of which have been prepared in the case of potassium iodide: a yellow crystalline solid of composition, Kl-I4-SO2, and a red solid of composition, Ki-4S02. It is decomposed by the influence of strong light or when strongly heated. It combines directly with chlorine to form sulphuryl chloride and also with many metallic peroxides, converting them into sulphates. In the presence of water it frequently acts as a bleaching agent, the bleaching process in this case being one of reduction. It is frequently used as an “ antichlor, " since in presence of water it has the power of converting chlorine into hydrochloric acid: S02 -}- C12 + 2H¢O = 2HCl + HZSO4. In many cases it acts as a reducing agent (when used in the presence of acids); thus, permanganate's are reduced to manganous salts, iodates are reduced with liberation of iodine, &c., 2KMnO.; +5502 + 2H2O=K2SO4 -4- 2MnSO4 + ZHZSO4; 2Kl03+ 5501 + 4H¢O = Ig + QKHSO4 -l- 3H2S04. It is prepared on the industrial scale for the manufacture of sulphuric acid, for the preparation of sodium sulphate by the Hargreaves process, and for use as a bleaching-disinfecting agent and as a preservative. When compressed it is also used largely as a refrigerating agent, and in virtue of its property of neither burning nor supporting combustion it is also used as a fire extinct or. The solution of the gas in water is used under the name of sulphurous acid. The free acid has not been isolated, since on evaporation the solution gradually loses sulphur dioxide. This solution possesses reducing properties, and gradually oxidizes to sulphuric acid on exposure. When heated in a sealed tube to 180° C. it is transformed into sulphuric acid, with liberation of sulphur. Numerous salts, termed sulphates, are known. Since the free acid would be dibasic, two series of salts exist, namely, the neutral and acid salts. The neutral alkaline salts are soluble in water and show an alkaline reaction, the other neutral salts being either insoluble or difficultly soluble in water. The acid salts have a neutral or slightly acid reaction. The sulphates are prepared by the action of sulphur dioxide on the oxides, hydroxides or carbonates of the metals, or by processes of precipitation. Sulphur-ous acid may have either of the constitutions /OH 0 OH
0:5 or , or be an equilibrium mixture of these
oH o H
two substances. Although the correct formula for the acid is not known, sulphates are known of both types. Sodium sulphite is almost certainly of the second and unsymmetrical type. Two ethyl sulphates are known, the first or symmetrical form being derived from sulphuryl chloride and alcohol, and the second and unsymmetrical from sodium sulphite and ethyl iodide; the junction of one ethyl group with a sulphur atom in the second salt follows because it yields ethyl sulphonic acid, also obtainable from ethyl mercaptan, C2H5SH. Two isomeric sodium potassium sulphates are known, and may be obtained by neutralizing acid sodium sulphite with potassium carbonate, and acid potassium sulphite with sodium carbonate; their formulae are: 02SK(0Na) and 02SNa(0K). There are various haloid derivatives of sulphurous acid. Thionyl fluoride, SOFZ, has been obtained as a fuming gas by decomposing arsenic fluoride with thionyl chloride (Moissan and Lebeau, Compt. fend., 1900, 130, p. 1436). It is decomposed by water into hydrofluoric and sulphurous acids. Thionyl chloride, S0Cl2, may be obtained by the action of phosphorus pentachloride on sodium sulphite; by the action of sulphur trioxide on sulphur dichloride at 7? -80° C. (Joum. Chem. Soc., 1903, p. 420); and by the action o chlorine monoxide on sulphur at low temperature. It is a colourless, highly refracting liquid, boiling at 78°; it fumes on exposure to moist air. Water decomposes it into hydrochloric and sulphurous acids. 0n treatment with potassium bromide it yields thionyl bromide, S0Br2, an orange-yellow liquid which boils at 68° C. (40 mm.) (Hartoz and Sims, Chem. News, 1893, 67, p. 82).
Sulphur trioxide, 503, mentioned by Basil Valentine in the 15th century, was obtained by N. Lemery in 1675 by distilling green vitriol. It may be prepared by distilling fuming sulphuric acid, or concentrated sulphuric acid over phosphorus pent oxide, or by the direct union of sulphur dioxide with oxygen in the presence of a catalyst, such as platinized asbestos (see SULPHURIC Ac11>). This oxide exists in two forms. The a- form is readily fusible and melts at 14-8° C. It corresponds to the simple molecular complex S03. The B- variety is in fusible, but on heating to 50° C. is transformed into the a- form. It corresponds to the molecular complex (S0;)2. /Vhen perfectly dry this oxide has no caustic properties; it combines rapidly, however, with water to form sulphuric acid, with the development of much heat. It combines directly with concentrated sulphuric acid to form pyrosulphuric acid, H2520-, It reacts most energetically with many organic compounds, removing the elements of water in many cases and leaving a carbonized mass. It combines directly with many elements and compounds and frequently acts as energetic oxidizing agent. It finds considerable application in the colour industry.
Sulphuryl fiuoride, SOZFQ, formed by the action of fiuorine on sulphur dioxide (H. Moissan, Compt. fend. 132, p. 374), is an exceedingly stable colourless gas at ordinary temperatures, becoming solid at about -120° C. Sulphuryl chloride, SOQCI2, first obtained in 1838 by Regnault (Ann. chim. phys., 1838, (2), 69, 170), b the action of chlorine on a mixture of ethylene and sulpfiur dioxide, may also be obtained by the direct union of sulphur dioxide and chlorine (€SD€C1&lly IQ the presence of a little camphor); and by heating chlorsulphonic ac1d 1n the presence of a catalyst, such as mercuric sulphate (liawlewski, Bef., I?Q7, 30 p 765); QSQZCLQH =5(), Cl, + HQSO4. it is a colourless fummg liquid which boils at 699 C. and which is readily decomposed by water into sulphuric and hydrochloric acids. Fluorsulphonic acid, SOQF-OH, is a mobile liquid obtained by the HCUOH of an excess of hydrofluoric acid on well-cooled sulphur trioxide. It boils at 162-6° and is decomposed violently bv water. Chlorsulphonic acid, S0¢Cl~0H, first prepared by A. Williamson (1f'0€~ R022 S06-, 1856, 7, p. II) by the direct union of sulphur trioxide with hydrochloric acid gas, may also be obtained by distilling concentrated sulphuric acid with phosphorus oxychloride: 2H2$04-ljPQCla=2S02Cl-0H-l-HCl-1-HP03. It is a colourless fummg liquid which boils at 152-153° C. When heated under pressure it decomposes, forming sulphuric acid, sulphuryl chloride, &c. (Ruff, Bef., 1901, 34, p. 3509). It is decomposed by water with explosive violence. Disulphuryl chloride, S205Cl2, corresponding to pyrosulphuric acid, is obtained by the action of sulphur trioxide on sulphur dichloride, phosphorus oxychloride, sulphuryl chloride or dry sodium chloride:6S03 -l-2P0Cl3 = P205 -I-3S205Cl2; SZCI2 + 5503 = S205Cl2 'l' 5502; S03 'ff' S02Cl2 = S205Cl2; + = S20;, Cl2+Na2S0.i. It may also be obtained by distilling chlorsulphonic acid with phosphorus pentachloride: 2S02Cl-OH -l-PCl5 = S205Cl2 +POCl;i --2HCl. It is a colourless, oily, fuming liquid which is decomposed by water into sulphuric and hydrochloric acids. An oxychloride of composition S203Cl4 has been described. Sulphur sesquioxide, S203, is formed by adding well-dried flowers of sulphur to melted sulphurtrioxide at about 12-15° C. The sulphur dissolves in the form of blue drops which sink in the liquid and finally solidify in blue-green crystalline crusts. It is unstable at ordinary temperatures and rapidly decomposes into its generators on warming. It is readily decomposed by water with formation of sulphurous, sulphuric and thiosulphuric acids, with simultaneous liberation of sulphur. Hyposulphurous acid, H2S204, was first really obtained by Berthollet in 1789 when he showed that iron left in contact with an aqueous solution of sulphur dioxide dissolved without any evolution of gas, whilst C. F. Schonbein subsequently showed the solution possessed reducing properties. P. Schutzenberger (Compt. fend., 1869, 69, p. 169) obtained the sodium salt by the action of zinc on a concentrated solution of sodium bisulphite: Zn -|- 4NaHS03 = Na2S204 + ZnS03 + Na2S03 + 2H20, the salt -being separated from the sulphates formed by fractional precipitation. A solution of the free acid may be prepared by adding oxalic acid to the solution of the sodium salt. This solution is yellow in colour, and is very unstable decomposing at ordinary temperature into sulphur and sulphur dioxide. A pure zinc salt has been prepared by Nabl (Monatr, 1899, 20, p. 679) by acting with zinc on a solution of sulphur dioxide in absolute alcohol, whilst H. Moissan (Compt. fend., 1902, 135, p. 647) has also obtained salts by the action of dry sulphur dioxide on various metallic hydrides. Considerable controversy arose as to the constitution of the salts of this acid, the formula of sodium salt, for example, being written as NaHS02 and Na2S204; but the investigations of C. Bernthsen (Ann., 1881, 208, p. 142; 1882, 211, p. 285; Bef., 1900, 33, p. 126) seem to decide definitely in favour of the latter (see also T S. Price, Joum. Chem. Soc.; also Buchercr and Schwalbe, Zeit. angew. Chem 1904, 17, p. 1447). Although this acid appears to be derived from an oxide S203, it is not certain that the known sesquioxide is its an hydride.
Persulphuric an hydride, S201, is a thick viscous liquid obtained by the action of the silent discharge upon a mixture of sulphur trioxide and oxygen. It solidifies at about 0° C. to a mass of long needles, and is very volatile. It is decomposed readily into sulphur trioxide and oxygen when heated. Water decomposes it with formation of sulphuric acid and oxygen: 25201 + 4H20 = 4H2S04 + 02. Persulphuric acid, HS04, the acid corresponding to 5207, has not been obtained in the free state, but its salts were first prepared in 1891 by H. Marshall (]oum. Chem. Soc., 1891, p. 771) by electrolysing solutions of the alkaline bi sulphates. The potassium salt, after recrystallization from warm water, separates in large tabular crystals. Its aqueous solution gradually decomposes with evolution of oxygen, behaves as a strong oxidant, and liberates iodine from potassium iodide. Solutions of per sulphates in the cold give no precipitate with barium chloride, but when warmed barium sulphate is precipitated with simultaneous liberation of chlorine 1 KQSQOS + BaCl¢ = BaS04 + K¢S04 + Cl2. The conductivity measurements of G. Bredig point to the salt possessing the double formula. Thiosulphuric acid, formerly called hypo sulphurous acid, HQSQO3, cannot be preserved in the free state, since it gradually decomposes with evolution of sulphur dioxide and liberation of sulphur: HQSZO3 = S+S02-l-H20. The salts of the acid, however, are stable, the sodium salt in particular being largely used for photographic purposes under the name of “ hypo." This salt may be prepare by digesting flowers of sulphur with sodium sulphite solution or by boiling sulphur with milk of lime. In this latter reaction the deep yellow solution obtained is exposed to air when the calcium poly sulphide formed is gradually converted into thiosulphate by oxidation, and the calcium salt thus formed is converted into the sodium salt by sodium carbonate or sulphate. The thiosulphates are readily decomposed b mineral acids with liberation of sulphur dioxide and precipitation of, sulphur: Na2S203 -1- 2HCl = 2NaCl S -l' 502 H2Q- ThQY form many double salts and give a dark violet coloration with ferric Chloride solution, this colour, however, gradually disappearing on standing, sulphur being precipitated. The acid is considered t0 possess the structure 02S(SH) (OH). SiHC€ S0dl{m 'fh105Phat€ f€aCtS with ethyl bromide to give sodium ethyl th1osulphate, wh1ch on treatment with barium chloride gives presumably barium €¥hYl thiosulphate. This salt, on standing, decomposes into barium dithionate, BaS205, and diethyl disulphide, (C2Hf»)252» Wh1Ch Points to the presence of the SH group in the molecule. I The zhionic acids are a group of sulphuf-C0f1t21f1§ U§ acids 0f §§ 9e"? formula H2S, .O¢, where »=2, 3. 4. 5 and Possibly 64, DI* 19“'§ acid, I-125206, prepared by ]. Gay-Lussac in 1819, is usua y obtaine in the form of its barium salt by suspending freshly precipitated hydrated manganese dioxide in water and passing sulphur dioxide into the mixture until all is dissolved; the barium salt is then precipitated by the careful addition of barium hydroxide. Much manganese sulphate is formed during the reaction, and H. C. Carpenter (Journ. Chem. Soc., 1902, 81, p. 1) showed that this can be almost entirely avoided by replacing the manganese oxide by hydrated ferric oxide, the reaction proceeding according to the equation: 2Fe(OH)3 + 3SO2＝FeS2O6 + FeSO3 + 3H2O. He points out that the available oxygen in the oxides may react either as SO2 + H2O + O＝H2SO4 or as 2SO2 + H2O + O＝H2S2O6; and that in the case of ferric oxide 96 % of the theoretical yield of dithionate is obtained, whilst manganese oxide only gives about 75%. A solution of the free acid may be obtained by decomposing the barium salt with dilute sulphuric acid and concentrating the solution in vacuo until it attains a density of about 1·35 (approximately), further concentration leading to its decomposition into sulphur dioxide and sulphuric acid. The dithionates are all soluble in water and when boiled with hydrochloric acid decompose with evolution of sulphur dioxide and formation of a sulphate. Trithionic acid, H2S3O6, is obtained in the form of its potassium salt by the action of sulphur dioxide on a solution of potassium thiosulphate: 2K2S2O3 + 3SO2＝2K2S3O6 + S; or by warming a solution of silver potassium thiosulphate: KAgS2O3＝Ag2S + K2S3O6; whilst the sodium salt may be prepared by adding iodine to a mixture of sodium thiosulphate and sulphite: Na2S03 + Na2S2O2 + I2＝Na2S2O6 + 2NaI. The salts are unstable; and a solution of the free acid (obtained by the addition of hydrofluosilicic acid to the potassium salt) on concentration in vacuo decomposes rapidly: H2S3O6＝H2SO4 + S + SO2. Tetrathionic acid, H2S4O4, is obtained in the form of its barium salt by digesting barium thiosulphate with iodine: 2Ba2S2O2 + I2＝BaS4O6 + 2BaI, the barium iodide formed being removed by alcohol; or in the form of sodium salt by the action of iodine on sodium thiosulphate. The free acid is obtained (in dilute aqueous solution) by the addition of dilute sulphuric acid to an aqueous solution of the barium salt. It is only stable in dilute aqueous solution, for on concentration the acid decomposes with formation of sulphuric acid, sulphur dioxide and sulphur.
Wackenroder’s solution (Debus, Journ. Chem. Soc., 1888, 53, p. 278) is prepared by passing sulphuretted hydrogen gas into a nearly saturated aqueous solution of sulphur dioxide at about 0° C. The solution is then allowed to stand for 48 hours and the process repeated many times until the sulphur dioxide is all decomposed. The reactions taking place are complicated, and the solution contains ultimately small drops of sulphur in suspension, a colloidal sulphur (which Spring (Rec. trav. shim., 1906, 25, p. 253) considers to be a hydrate of sulphur of composition S8·H2O), sulphuric acid, traces of trithionic acid, terra-and pentathionic acids and probably hexathionic acid. The solution obtained may be evaporated in vacuo until it attains a density of 1·46 when, if partially saturated with potassium hydroxide and filtered, it yields crystals of potassium pentathionate, K2S5O4·3H2o. The formation of the pentathionic acid may be represented most simply as follows: 5SO2 + 5H2S＝H2S5O5 + 5S + 4H2O. The aqueous solution of the acid is fairly stable at ordinary temperatures. The pentathionates give a brown colour on the addition of ammoniacal solutions of silver nitrate and ultimately a black precipitate. Hexathionic acid, H2S5O6, is probably present in the mother liquors from which potassium pentathionate is prepared The solution on the addition of ammoniacal silver nitrate behaves similarly to that of potassium pentathionate, but differs from it in giving an immediate precipitate of sulphur with ammonia, whereas the solution of the pentathionate only gradually becomes turbid on standing.
The per-acids of sulphur were first obtained in 1898 by Caro (Zeit. angew. Chem., 1898, p. 845) who prepared mono per sulphuric acid by the action of sulphuric acid on a per sulphate. This acid may also be prepared by the electrolysis of concentrated sulphuric acid, and it is distinguishable from per sulphuric acid by the fact that it immediately liberates iodine from potassium iodide. It behaves as a strong oxidant and in aqueous solution is slowly hydrolysed. It most probably corresponds to the formula H2SO5.
See H. E. Armstrong and Lowry, Chem. News (1902), 85, p. 193; Lowry and West, Journ. Chem. Soc. (1900), 77, p. 950; H. E. Armstrong and Robertson, Proc. Roy. Soc., 50, p. 105; T. S. Price, Ber., 1902. 35, p. 291; Journ. Chem. Soc. (1906), p. 53; A. v. Baeyer and V. Villiger, Ber., passim.
Pharmacology.-The sources of all sulphur preparations used in medicine (except calx sulphurata) are native virgin sulphur and the sulphides of metals. Those contained in the British Pharmacopoeia are the following: (1) Sulphur sublimatum, Howers of sulphur (U.S.P.), which is insoluble in water. From it are made (a) confectio sulphuris; (b) unguentum sulphuris; (c) sulphur praecipitalum, milk of sulphur (U.S.P.) which has a sub-preparation trochiscus sulphur is each lozenge containing 5 grs. of precipitated sulphur and I gr. of potassium acid tartrate; (d) patassa sulphurata (liver of sulphur), a mixture of salts of which the chief are sulphides of potassium; (e) sulphuris iodidum (U.S.P.), which has a preparation unguentum sulphuris iodidi, strength 1 in 25. From the heating of native calcium sulphate and carbon is obtained calx sulphurata (U.S. and B.P.), or sulphurated lime, a greyish-white powder.
Therapeutics.—Externally, sulphur is of use in skin affections. Powdered, it has little effect upon the skin, but in ointment or used by fumigation it has local therapeutic properties. In scabies (itch) it is the best remedy, killing the male parasite, which remains on the surface of the skin. To get at the female and the ova prolonged soaking in soap and water is necessary, the epiderm being rubbed away and the ointment then applied. Precipitated sulphur is also useful in the treatment of acne, but sulphurated lime is more powerful in acne pustulosa and in the appearance of crops of boils. Internally, sulphur is a mild laxative, being converted in the intestine into sulphides. Milk of sulphur, the confection and the lozenge, is used for this purpose. Sulphur and sulphur waters such as those of Harrogate, Aix-la-Chapelle and Aix-les-Bains, have a powerful effect in congested conditions of the liver and intestines, haemorrhoid's, gout and gravel. Sulphur is of use in chronic bronchial affections, ridding the lungs of mucus and relieving cough. In chronic rheumatism sulphur waters taken internally and used as bgthfs are effectual. Sulphur in some part escapes unchanged in the faeces.
When sulphur is burned in air or oxygen, sulphur dioxide is produced, which is a powerful disinfectant, used to fumigate rooms which have been occupied by persons suffering from some infectious disease.
- ↑ References.—A very full article (“Zolfo”) by G. Aichino, of the Geological Survey of Italy, will be found in the Enciclopedia delle arte e industrie (Turin, 1898). This includes a full bibliography. See also J. F. Kemp in Rothwell’s Mineral Industry (1893), vol. ii.; Jules Brunfaut, De l’Exploitation des soufres (2nd ed., 1874); Georgio Spezia, Sull’ origine del solfo nei giacimenti solfiferi della Sicilia (Turin, 1892). For Japanese sulphur see T. Wada, Minerals of Japan (Tokyo, 1904).
- ↑ It is a common practice of keepers of dogs to place a piece of roll sulphur in the animal's water but this serves no useful purpose owing to this property.