TECHNICAL CHEMISTRY. T e c h n i c a1 C h e m i s t r y. Gas Lighting. By J. VAN EYNDHOVEN (Dingl. polyt. J., 229, 449).-It has been supposed that the gas flame is translucent. As, however, this appeared doubtful to the author, he determined to in- vestigate the subject. The experiments were made with the aid of an excellent photometer, the results being as follows :- The first experiments were madewith a bat's-wing burlier of 160 litres' gas consumption a t 8.3 mm. pressure. The result of ten observations proved that the lighting power of the flat side was equal to 11.58, that of the narrow edge 10.04 candles. After correction for barometer and thermometer, the actual lighting power for normal consumption of gas and candle is 11.81 and 10.18 candles: English spermaceti candles with a normal consumption of 120 grains were used.For a flame consuming 100 1. of gas per hour, the actual illuminating power on the flat side was 9.03, on the narrow edge 7-42 candles, m7it.h a gas pressure of 4 mm. The difference in both cases is 1.5 candles, or 1 7 to 18 per cent., a circumstance which proves that the flame is not translucent, a bat's-wing burner giving most light on its flat side. An argand burner will from a similar cause not give all its illumina- ting power. For a good street illumination, therefore, the slits of the burners and the direction of the road must be placed perpendicularly on one another. D. B. Some Peculiarities of the Vartry Water, and the Action of that Water on Boiler-plates. B,y C. R. C. 'YICHUORNE (Cheiri,. News, 38, 191).-The water of the River Vartry consists of organic matter of a peaty nature, and mineral matter, which consists chiefly of the chlorides of the alkalis and of the alkaline earths; nitrates and nitrites are also present, which, however, cannot be detected with- out evaporation, but as concentration by heat reduces the nitrates, the water was concentrated in a vacuum.This reduction, when it takes place in high pressure boilers, is a cause of the corrosion of the boiler plates, It was found that when iron was heated with nitrates in sealed glass tubes it became oxidised. E. W. P. Preservation of Potable Water. By H. SCHIFF (Deut. Chem. Ges. Ber., 11, 1528--1529).-Water containing 3 parts of salicylic acid in 10,000 was found to be fresh after remaining in a flask for three years.Sea-water to which phenol or, preferably, carbon bisulphide (1 part to 1,000) has been added, forms a good preservative fluid for specimens of marine fauna. w. c. w.86 ABSTRACTS OF CHEJIICAL PAPERS. Utilisation of Suint from Wool. By F. FISCHER (Dim$. polyt. J., 229, 446--449).-1t is known that raw wool contains about 90 per cent. of suint soluble in cold water, consisting of the potassium compounds of oleic, stearic, and acetic acids, a small amount of valeric acid, and many other organic substances, also of potassium chloride and sulphate, ammonium salts, and especially potassium carbonate, and sodium compounds. By lixiviating wool with water, a dark brown liquid of peculiar smell is obtained, of sp. gr. 1.069; I. litre of this required, for neutrali- sation, a quantity of normal acid corresponding with 3.98 grams of potassium carbonate.By neutralising 1 litre of liquor with hydrochloric acid and shaking up with benzene, only 916 milligrams of a yellow strongly smelling fat were obtained. By evaporating 1 litre and drying at 120°, 122.16 grams of a hygroscopic mass remained, which on igni- tion swelled up considerably, and evolved a, gas burning with a bright flame. By continued heating in the air, and extracting with water and evaporating, 72.16 grams of a white saline mass, and 2.98 grams of a residue consisting of sand, alumina, lime, and phosphoric acid re- sulted. By burning the suint dried at 120" in a stream of oxygen, 3.04 per cent. of hydrogen as water and 19.92 per cent. of carbon 8s carbonic acid were obtained.The organic compounds of potassium are hereby converted into potassium carbonate. A profitable recovery of the fat and the acetic acid is impossible, but the utilisation of the evaporated mass for gas and the production of potash can be recommended. For obtaining the potash present i r i the mass, the latter is in Germany merely heated strongly in rever- beratory furnaces, the gas formed being used as fuel. Analyses of the composition of the flue gases showed that carbon monoxide is, in spitc of the sooty nature of the flame, formed very rarely, and only when the mass is at its highest heat, in which case oxygen disappears. As soon as the evaporated liquors begin to burn, the heat evolved suffices to destroy all organic matter present.Thus with 1 kilo. of Westphalian coal 12 kilos. of liquom can be evaporated and ignited. The coke formed is solid. The following is the analysis of the coal dried a t 120" :- C. H. S. 0 (and N). Ash. 76.11 4.52 1-19 10.06 8-12 The raw potash taken from the furnace gave- Salts soluble in water. Insoluble. Organic matter. 92-05 4.92 3-03 The composition of the soluble salts was as follows:- K,C03. KC1. KZSO4. NasCO3. 85.34 6-15 2.98 5.02 = 99.49 p.c. W. Graff, in Lesum, works up this raw potash from six establishments for washing wool into pure potassium carbonate, bicarbonate, chloride, and sulphate. He employs about 10 to 12 workmen, the annual sale amounting to about 120,000 marks. D. B.TECHXICAL CHEMISTRY. 87 Ingredients. Analyses of Clays. (Dingl.polyt. J., 229, 451455).--Glaze- clay.-As a very durable, perfectly impervious glaze on refractory clay, e.g., for Bunzlau vessels, water pipes, &c., a very readily fusible clay 18 often used. Seger has analysed three specimens of t'hese earthy glazes with the following results :- A. 58-99 11.73 4.16 4-77 1.83 4.83 16-19 4.80 B. 64.49 14.35 4.38 4.13 1-53 3.69 3.12 3.31 C. 62.40 15.51 5-68 4.36 1-13 3.62 2.88 4.41 A is one from Naumburg 0. Q, used in Bunzlau for the manufacture of brown kitchen utensils and water pipes ; B from Camenz i. S., used for the same purpose, and C is a glaze from the clay pipe manufactory in Dommitzsch 0. Elbe. The pyrometric investigations showed that, according to Seger's quotients of refractoriness (ibid., 228, 2M), the Naumburg glaze was the most readily fusible, that of Dommitzsch the most difficultly fusible.Stoneware-cZa$.-This clay, obtained from Hohr, and representing the raw material used for the manufacture of the fine, compact, pearl-grey vessels a t that place, had the following composition : H20 and SiO,. A1,03. Fe203. CaO. MgO. Alkalis. CO2. organic matter. Si02. Al,O,. Fe203. CaO. MgO. K20and N%O. H,O. 70.12 21.43 0.77 0.00 0.39 2-62 4.92 By sulphuric acid. Wilkins has already pointed out the important influence which a large amount of silica in clay has on the lustre and the fineness of the salt-glaze ; an observation which confirms the ready acceptation of the salt-glaze and the peculiar compactness of the above mass. Porcelain Eurth of Linzoges.-These clays are not merely distin- guished by the fineness of their forms, but the mass itself possesses a purer, more agreeable coloration, and greater fineness and strong trans- parency than the greater number of the German productions. The following is the composition of the kaolin :- i I Si02 .................... Fe203.................... CaO .................... MgO .................... K,O .................... Na.20 .................... Loss by ignition .......... A120,. ................... 58 -39 27.52 0.36 1 -52 0 '41 1 -71 2 *58 7 -19 99 -68 32 222 7.49 - 4'40 J - 26 *17 20 '03 0 -36 1 -82 7 -19 Clay sub- stance decomposible sulphuric acid. bY 47 '09 36 *04 0 '64 3 *27 12 -9488 ABSTRACTS OF CHEMICAL PAPERS. Kot decom- posible Corresponding with- Clay substance ................55.88 Quartz:. ....................... 5.95 Felspar. ....................... 38.1 7 Compared with the composition of the German and Austrian kaolins (ihid., 228, 67), this substance is distinguished by an unusually high percentage of felspar, which explains also the fact that in S h e s the mass is not mixed with felspar but merely with sand. The porcelain from Limoges had the following composition :- Decompos- ible Ingredients. SiOa .................... CaO .................... MgO .................... K20 ..................... 8 1 2 0 3 . . .................. FezO,. ................... N+O .................... Loss by ignition .......... 66 -71 21 '58 0 '47 0 -61 0 -37 2.93 1 -62 5 -54 99-83 - 47 -27 5 '93 1 3'76 - - 19 '44 15 -65' 0 -47 1 -77 5 -54 Composition of the clay substance.45 -35 36 -50 1.09 4 *13 12.92 corresponding with clay substance = 43.04, quartz 26.46, and felspar 30.50. The mass contains therefore more sodium, lime, and magnesia than, e.g., the Berlin porcelain, a circumstance which explains its ready fusibility and greater transparency. The glaze from Limoges consists of- SiOp. A1203. Fe203. CaO. Ingredients in p. c.. ............... 74.99 14.80 0.37 1.09 Not decomposible by sulphuric acid. . 70.92 12.38 - 0.20 Decomposible by sulphuric acid .... 4.07 2.42 0.37 0.89 Ingredients in p. c.. ............... 0.36 4.31 3.49 0.65 Loss by MgO. K20. NasO. ignition. Not decomposible by sulphuric acid . . 0.36 7 4 7 Decomyosible by sulphuric acid .... - 0.68 - 0.60 liurstenu?aZd-gZaxe.-This glaze adheres in the form of sand to the lignite strata, and is used in the preparation of the lead and tin enamels for the fabrication of stoves.According to Seger, the mass dried a t 120" has the following composition :-TECHNICAL CHEMISTRY s 89 H,O and carbon- Si02. A1,03. Fe,O,. MgO. E@. aceous matter. Total.. . . . . . . . . . , . . 85.96 7.30 2.26 0.25 1.97 2.11, - Not decomposible by U HZSOa ....... . .. 80.03 2.69 - 1-08 substance.. . . . . . . 5.93 4.61 2.22 1.14 2.12 Eatable-cZay.-Pattison Muir has investigated a clay-substance from Mackenzie County, in South Island, near New Zealand, which is eaten by men and sheep in large quantities. It has the following compos’ , I t’ ion :- Decomposible clay Si02. Al,03. Fe,03. CaO. MgO. NaC1. n20. Organic. 61-25 17.97 5.72 1-91 0.87 3.69 7.31 1.77 (according to R.Biedermann in Noiizb. d. Ver. fur Fuh. zo?z Ziegel?z. 1878, 229). Gross~Zme?.ode-cZay.-This clay is highly refractory and possesses great cementing power. It is coloured light bluish-grey to white, is shiny, and breaks up in water to a fine slimy mass. The following is the composition of the clay dried a t 120’ :- SiO,. r 1. - Chemically Mechanically Loss by AI203. combined. added. MgO. CaO. Fe203. K20. S. ignition. 34.52 43.38 6.53 0.73 0.76 1.66 1.51 0.26 11-04 This gives a chemical composition: 4.89(A1203, 1.65 SiO,) + RO, and the quotient of refractoriness (according to Bischof) = 2.96. D. B. Blair’s Process for Iron Manufacture. By J . IRELAND (Dingl. polyt. J., 229, 458--461).-This paper gives a detailed account of the improvements which have been recently made in the working plant, also in the method of preparing iron sponge.A brief descrip- tion of the reduction furnaces is given; these consist of a group of three vertical retorts, each retort having a diameter of 914 mm., and being 8.53 m. high. The furnace is surrounded by an outer casing of brickwork, leaving a combustion chamber between the inside of it and the outside of the retorts. The retorts were heated externally by gas jets, the air for combustion being supplied through apertures immediately above the gas jets. I n 1876 Blair discovered, that by the addition of a small quantity of alkali to the carbonaceous matter mixed with the ore, the action of reduction was facilitated to a great extent, and ore which took about thirty hours to reduce without alkali, could be per- fectly reduced in six hours with it.The existing furnaces, however, could not be altered in any way to suit the new condition of quickened reduction. Blair therefore abandoned the whole principle of heating, and adopted a system by which a stream of hot carbonic oxide was passed through the mass of ore and carbonaceous matter. The author, however, made use of the above furnace by dividing the cast-iron pipe inserted in the top of each retort into a number of smaller ones, so as90 ABSTRACTS OF CHEMICAL PAPERS. to present as small a column of materials to the action of heat as pos- sible. He used a furnace of a height of 6.4 m., the retort, being about 3.2 m. high, with four inserted tubes. A fiirnace of this description, 1.52 m.diameter and 12.92 m. high, produces from 60 to 70 tons of iron, and costs about 12,000 marks. The cost of producing iron sponge will vary according to the locality in which'the work is carried on, but with the furnaces intro- duced by Blair, the cost will be about 22 marks per ton, exclusive of the ore. Where several of the furnaces are in operation, the cost is less. Where the oye is rich and pure, iron sponge made from it can be a t once made into tool steel, the quality of which cannot be equalled by that made from the best brands of Swedish bars. I n the case of ore which is not so rich, the best way of utilising the sponge made from it is to melt i t in a cupola furnace, transferring the molten mass to a Siemens-Martin furnace, wherein the mass is converted into steel.The pig metal obtained in this manner will coiitain about 1.5 per cent. carbon and 0.19 per cent. to 0.25 per cent. silicon. D. B. Phosphorus in Cleveland Ironstone and in Iron. By J. E. STEAD (Chew,. News, 38, 14-18 ; 29-31 and 39-42).--This paper may be divided into six sections: (1.) The compound or com- pounds in which phosphoric acid exists in the Cleveland ironstone. (2.) Method of eliminating phosphoric acid from iron ores. (3.) The compound in which phosphorus exists in Cleveland metal. (4.) The effect, physically and chemically considered, which phosphorus has on pig metal. (5.) Method of removing it from pig iron. (6.) Phos- phorus in bar iron. The following are the results of the analysis of the main Cleveland ironstone bed :- Iron in the Stone Siliceous Phosphoric Loss by calcined analysed.Iron. matter. acid. Moisture. calcination. stone. Main: p. c. p. c. p. c. p. c. p. c. p. c. (1st foot 26.53 18.30 1.46 8.50 27.39 36.50 2nd ,, 29.54 10.90 1.13 9-10 29.80 42.08 3rd ,, 29.14 10.68 1-13 9.50 29.80 41.50 4th ,, 28.41 11.98 1.41 9-80 28.80 39-92 5th ,, 29.97 9.00 1.17 10.00 30.83 43.31 6th ,, 30.42 8.82 0.89 10.00 31.51 44.40 7th ,, 29.70 9-00 0.80 10.10 31.78 43-53 8th ,, 29-85 9.29 0.91 9-80 30.90 45-20 9.00 28.50 42.40 C9th ,, 30.30 12.01. 1.16 Black hard. 4 7 inches 30.56 12-90 0.44 8.50 26.80 41.75 *s {; ,, 37-87 22.20 1-12 5-50 18.00 34.00 ,, 27-26 24.70 0.81 5-00 17.00 32.85 It will be seen from these analyses that no part of the stone is free from phosphoric acid.In the " Black Hard " bed, the author found this substance very variable in quantity, reaching as much as 3 per cent. in some cases, and only 0.25 per ceut. in others. d CJTECHNICAL CBEJIISTRT. 91 1. As to the form in which phosphoric acid exists in Cleveland ironstone, the author mentions that several years ago Pattinson inves- tigated this matter and concluded, judging from the non-action of ammonium sulphide on the stone, or rather on the compound contain- ing phosphoric acid in the stone, that no iron phosphate was present, and that the phosphoric acid must be in combination with lime ; and the results obtained by other methods of investigation employed by the author has confirmed this. It is the prevailing opinion that the source of all the phosphorus in the ironstone is the remains of small phosphatic animals ; but this theory cannot be regarded as trustworthy, first, because in some parts of the “ Black Hard ” bed, where no fossil remains could be detected, the phosphoric acid has been found in large quantity, and secondly, because in all cases, on analysis, the shells and fossil remains which were taken out of the stone, were proved to con- tain much less phosphoric acid than the surrounding ironstone.The following analyses of fossil wood taken from various mines in that disirict will throw some light upon this very obscure subject. Fossilised mood found in Cleveland ironstone- OH,. C. SiO,. (20%. SO3. S. MU. d1203. 3.00 9-60 0.50 0.75 0-GO 7-56 trace 8.25 COO and NiO. Co and Ni. Fe. FeO. MgO.P,05. CaO. 3.70 1-65 5.20 10.02 1.12 20.80 27.60 Several other samples gave similar results on analysis. There can be no doubt about the fact, that these samples were at one time parts of trees, which in their natural state would not, contain more than very minute quantities of phosphoric acid. The latter must have been in solution, and has in this state passed into the substance of the wood and been there deposited in the condition in which we find it. 2. Method of Removing Phosphoric Acid from Ores.- Jacob’s method, based on the treatment of the ores with sulphurous acid produced by burning sulphur pyrites and condensing the acid fumes in coke towers, gave satisfactory results only when the stone was reduced to a very fine powder, about 90 per cent. of phosphoric acid being removed thereby.Forbes’ method, based on the action of common salt on iron phosphate when fused, also gave unsatisfactory results, as did the last method referred to by the author, the action of sodium carbonate on phosphate of lime when fused with it. From this it would seem that Cleveland ironstone cannot be freed from phosphorus by any methods as yet proposed. With regard t o the smelting of ironstone, since we know that phosphate of lime heated with carbon aud iron oxides, or metallic iron, to a very high temperature, is decomposed, the phos- phorus combining with the iron, it is to be expected that nearly all of the phosphorus introduced in the charge at the top of the blast-furnace, will be found concentrated in the pig metal. Experiments showed that fluorspar is of no value in removing the phosphoric acid or preventing its passage into the metal when employed as a flux in smelting.Iro?z a i d Phosphorus.--By direct addition of phosphorus to iron heated in a crucible, the author obtained combinations containing between 6 mid92 ABSTRACTS OF CHEMICAL PBPERS. 27 per cent. of phosphorus, although Percy has stated that iron will not take up more than 8.4 per cent. of phosphorus when the two substances are heated together in the manner described. The fusion point appears to decrease with each addition of phosphorus, until a com- pound containing from 10 to 12 per cent. of phosphorus is produced, which is the most fusible ; after which each addition makes the com- pound less and less fusible. 3. The Co~npount7s in which Phosphwus exists in Clemdand Jfeta1.- Judging from the comparative fusibility of iron, it was thought that if separate compounds of iron and phosphorus existed in pig metal, these compounds would be more fusible than the bulk.Analyses of about 1 cwt. of Cleveland iron poured into a mould were made. After the mass had become viscous, extreme pressure was applied by means of a hydraulic ram, and the portions of metal last fluid expressed. The expressed metal was found to be n combination of phosphide of iron and unaltered pig metal in the proportion of 51.5 : 48.5 or 88.05 per cent. of iron and 11.95 per cent. of phosphorus ; or, calculated into chemical equivalents, they are in the ratio 1.57 iron to 0.385 phos- phorus or 4 equivalents of iron to 1 of phosphorus, and the formula may therefore be written Fe4P.It is very clear from these results that phosphide of iron does exist in a separate state in pigmetal intimately diffused throughout the mass. On immersing bar iron in dilute acid, such as hydrochloric acid or sulphuric acid, a black residue is observed adhering to the outside of the iron. In these residues, phosphides of different constitution were found, the iron and phosphorus being pre- sent as Fe3P4 and Fe3P,. This fact proves that iron containing phos- phorus contains two or more different phosphides, and that they exist in very varying proportions in different samples of iron. 4. The Efect which Phosphorzis has on Pig metal ( a ) . Physicnl Pro- perties.--Experiments have shown that, as a considerable quantity of iron is in combination with phosphorus in Cleveland iron, there is less iron remaining capable ut taking up silicon, than is the case where no phosphorus is present: consequently less silicon w7ill be required to give to the smaller proportion of iron t,he conditions necessary for the production of glazed iron.( b . ) ChemicaZ Properties.- When sulphur is added to fluid metal-which under ordinary circum- stances would assume a grey fracture when cooled and broken-the sulphurised iron when cold will present a mottled or white fracture. I n other words, sulphur prevents the separation of carbon as graphite. I n order to ascertain if phosphorus has a similar action, experiments were made which proved that the effect of phosphorus compared with that of sulphur is very small, and would not affect materially the quality of the iron or pig in this direction, even if increased in con- siderable quantity.5 . Methods of removi?Ag Phosphorus from Pig metal.-The action of oxide of iron as a purification method is well known, but it has fre- quently been supposed that oxide of iron, without the aid of mechanical power, has very little action, and that the work a puddler gives to the metal has some important action in removing phosphorus independent of the oxide of iron. By the results obtained from numerous experi- ments it has been clearly proved that mechanical power, whether itbe in the force of the refining blast, the motion of the puddler’s bar, or the revolving of the rotary puddling machine, is simply the meaiis by which the molten iron is brought into intimate contact with the fluid or semi-fluid oxide of iron, The removal of phosphoras depends entirely on this, and not on any mechanical force.It is further illustrated experimentally that, when the puddling process is con- ducted a t a very low temperature,or when the cinder is run out of the furnace before the phosphorus is removed, the puddled bar produced is high in phosphorus. i n the first case the temperature is not high enough to liquefy the necessary amount of cinder required for the purification of the metal, and as a consequence, there is left an impure iron ; whilst in the other, when the cinder is removed from the semi- purified iron the purifying agent being taken away, the removal of phosphorus is retarded and a pliosphuretted iron is produced.On the other hand, when a high temperature is maintained, a very excellent quality of bar is produced. 6. Iron Heated with Phosphoric Acid.-It is stated that pure iron at a red heat has no power to decompose phosphoric acid ; but, if the iron be heated to its fusion point, the acid is readily decomposed. Pure iron was fused with puddler’s tap-cinder, containing above 4 per cent. of phosphoric acid, in order to determine whether or not pure iron would decompose phosphoric acid when in combination with iron oxide : the button produced contained = 2.12 per cent. Pure iron was next fused with phosphate of iron, and the metal, after fusion, was found to contain 2.68 per cent. of phosphorus. The nature of the action between oxide and phosphide of iron was proved by experiments to be not physical but chemical.The button obtained weighed about 15 per cent. more than before such treatment. 6 . Phoqhorus in Bar-iron.-From the following results i t will be seen that a considerable amount of phosphorns is removed by simply heating and rolling iron containing i t ; and that it is oxidised and removed from the iron, whereby the quality of the bar is improved considerably. No. 2 ordinary bar-iron made from Cleveland pig was twice piled and rolled. No. 4 bar, produced after the second rolling, was excellent fibrous iron, and very soft, whereas, before the treatment, it was in great part crystalline and hard:- Phosphorus combined Phosphorus in Phosphorus. with iron. cinder. Total.p. c. p. c . p. c. 2. 0.243 0.087 0.33 3. 0.130 0.110 0.24 4. 0.071 0.149 0.22 The following is an analysis of three finished bars made from Cleveland iron, puddled in the Danks’ furnaces at the Tees Side Iron Works. It would be difficult to obtain better iron thaa this:- I. 11. 111. p. c. p. c. p. c. Carbon .. .. . . .. 0.080 0.110 0.160 Silicon .... .. .. 0.092 0.046 0.040 Phosphorus . . . . 0.110 0.060 0.073 Sulphur .... .... 0.012 0.016 0.01294 ABSTRACTS OF CHEMICAL PAPERS. Pliosphorus combined Phosphorus in Phosphorus. with iron. cinder. Total. p. c. p. c. p. c. 1. 0.057 0.063 0.1 10 2. 0.023 0.037 0.069 3. 0.034 0.039 0.073 I n the third portion of his paper the author describes some of the changes which take place when air is blown through phosphuretted metal, and censiders the value of manganese oxides, chlorine, bromine, iodine, and hydrogen as agents for removing phosphorus, leaving the question of ore purification as a yet unsolved problem, and one which will not be readily solved to the satisfaction of the practical iron manufacturer. When metal containing mangnnese, silicon, carbon, and phosphorus is acted upon while in the fluid state by a stream of air, there is every reason to believe that all the elements present, probably with the ex- ception of carbon, are oxidiscd in the ratio in which they exist in the metal, and this should give a very basic cinder.Such, however. is not the case: for almost instantly after the formation of cinder, the manganese, silicon, and phosphorus still present in the fluid mass are oxidised by the oxygen of the protoxide of iron, while the reduced iron, leaving the cinder, returns to the bath and is replaced by the oxide of manganese, silicon, and phosphorus.In consequence of the rapidity with which these reactions take place, the cindey drawn off from the metal is always more or less saturated with silica, phosphoric acid, and manganese oxide. la a Bessemer converter, when the temperature is low enough, there can be no doubt that a t first all ingredients are burnt just in the proportion in which they are present. Such, however, is tlie violent agitation to which the metal is subjected, that the cinder and iron are continually in intimate con- tact, and as a consequence, the cinder is very rapidly saturated with silica and phosphoric acid.In the Bessemer converter, after the saturation point has been reached, when the silica and phosphoric acid have both in combination with them the proper chemical proportion of oxide of iron, the still unoxidised silicon in the metal will continue to reduce the oxide in the cinder, and will replace i t by silica. It is clear that when this point has been attained, viz., the removal of a base and the substitution of an acid in a compound already saturated with acid (silica), silica must be in excess, and that, as this acid is much niore powerful than phosphoric acid, i t will take away the oxide of iron a t first in combination with it, by which reaction silicic acid arid iron phosphates are transformed into phosphoric acid and iron silicate. Experiments were.undertaken which afforded proof of the theory, that manganese is capable of reducing free phosphoric acid a t a comparatively low temperature. It was further shown that the attraction of silicon for oxygen is greater than the attraction of phos- phorus for that element, and that when free phosphoric acid is exposed to the action of silicon, as i t exists in fluid metal a t low temperatures, oxygen is withdrawn from the phosphoric acid, and combines with the siiicon to form silicic acid. The results of an experiment in which fluid iron containing little or no silicon or manganese, was pouredTECHSICAL CHEMISTRY. 95 upon solid phosphoric acid placed at the bottom of a red-hot crucible, clearly showed that the acid had suffered decomposition. As the question as to the point a t which oxide of iron becomes saturated with silica is very important, several experiments were made with the view of solving it. F o r this purpose cinder containing little more than a trace of phosphoric acid wils mixed with variable propor- tions of sand, and, after fusion, was agitated with fluid iron containing phosphorus.In each case the metal was tested for phosphorus after treatment, and if no diminution was detected, it was concluded that the cinder employed contained no free iron oxide. The results were as follows :- No. 1. No. 2. No. 3. No. 4. p. c . p. c. p. c. p. c. Protoxide of iron.. ...... 73.90 64*.50 55.50 47-68 Sesquioxide of iron. ..... 11.60 10.60 8.50 6.87 Silica.. ................ 10.50 20.40 31.00 40.00 Alumina, lime, &c. ......4-00 4.50 5.00 5.45 100.00 lOO.00 100.00 100.00 No. 5. No. 6. No. 7. No. 8. p. c. p. c . p. c. p. c. Protoxide of iron ........ 42.13 43.41 38.57 29.57 Sesquioxide of iron ...... 10.71 8.13 7.86 5.00 Silica .................. 44.00 46.00 51.00 62.50 Alumina, lime, &c. ...... 3.16 2.46 2.57 2.93 100*00 100*00 100~00 100.00 Metallic iron.. .......... 65.60 57.60 49.12 41.89 Ratio of iron to silica . . . . 1 to 0.16 0.35 0.63 0.95 Before treatment ........ 1.51 1.51 1.48 1.48 After treatment.. ........ 0.13 0.04 0.2.5 0.75 Phosphorus in metal- Metallic iron.. .......... 40.27 38.34 38.50 26.50 Ratio of iron to silica .... 1 to 1-06 1.20 1.44 2.36 Before treatment ........ 091 0.91 0.91 0.91 After treatment.. ........ 0.89 0.90 0.91 0.91 Phosphorus in metal- It will be seen that when the ratio of iron to silica in the cinder is as 1 to 1.06, the compound is incapable of oxidising phosphorus from fluid iron containing it.This ratio is almost exactly the same as that of the chemical equivalents of iron and silica, viz., as 56 t o 60. It will be noticed that there has not been so much phosphorus removed in No. 1 as in No. 2, in which the cinder was dot so pure as in the first case, This, however, was due to the very sluggish nature of the cinder, which prevented its intimate admixture with the metal. It was proved by experiment that, within certain limits of tempera- ture, it is impossible to drive off from cinder its phosphoric acid by96 ABSTR.4CTS OF CHEMICAL PAPERS. the addition of silica.The analysis of the cinder made after fusion showed that it tenaciously retains phosphoric acid, confirming the theory that the whole of the phosphorus rerrioved in the various pro- cesses in which oxide of iron is used for purifying iron, is contained in the cinder, and that none is vaporised and carried iip the stack with the waste products of combustion from the furnace grate. As t o the value of manganese oxides as agents for purifying iron from phosphorus, it is mentioned that the protoxide, retaining its oxygen with much greater tenacity than the sesquioxide, and being de- composed a t very high temperatures only, in presence of reducing agents, is without any direct action on the phxphorus existing in the fluid iron ; as, however, this oxide has a much greater attraction for silica than iron oxide, it plays a part of secondary importance in the cinders of the purifying processes by taking up the silica.By forcing per- oxide of manganese under the surface of molteii iron, i t is deprived of half its oxygen, which, acting upon the oxidisable impurities in the metal, removes them. When oxide of iron acts upon phosphorus, for each part of that element oxidised, 4.5 parts of pure iron are removed from the oxide, When manganese peroxide acts upon phosphorus the oxidation is effected by free oxygen, and therefore there is no gain by the separation of metal. I t would seem, therefore, that peroxide of manganese is of much less value than iron oxides. With regard to the value of fluorspar as an agent for removing phosphorus, the fol- lowing experiment was tried. The action of a mixture of fluid oxide of iron and fluorspar upon Cleveland iron was ascertained by fusing two-thirds of mill-tap and one-third of spar, and thoroughly well mixing up with molten iron, the result being the removal of the greater part of the phosphorus.AS to the use of chlorine, bromine, and iodine, it is mentioned that since all these elements form definite compounds with phosphorus, which are all decomposed when brought into contact with red-hot iron, tthe phosphorus combining with the iron, t,here would be no advantage derived from their use. Hydrogen also is incapable of removing phosphorus from iron, as iron will with- draw phosphorus from its combination with hydrogen. Water has been advocated as an agent for removing phosphorus, it being held that the hydrogen would combine with i t and pass off as phosphoretted hydrogen. An experiment was undertaken with the following re- sults :- Pig metal.Before. After. Phosphorus.. . . . . . . 1.48 p. c. 1-48 p. c. Analysis of gases evolved from molten Cleveland iron in water :- 79.69 12.48 4.87 1.74 1.22 None = 100 H. co. CH4. H28. CO2. r205. p. c. The metal lost half its sulphur by the operation. 111 concluding this paper the author remarks, that so far as our present knowledge goes, there is nothing to surpass, in point of cost and efficiency, the process of purifying by means of oxide of iron, D. B.TECHNICAL CHEMISTRY. 97 Manufacture of a Red Pigment from Iron Scrap. By R. and C. STEINAU (Chem. Cen.fr., 1878, 336).-This pigment is formed by exposing wrought-iron shearings to the alternate action of air and water, and heating the resulting hydrated oxide to redness with access of air.Black is obtained by using reducing agents, and brown by mixing the two pigments. Preparation of Rosemary-oil. By C. 0. CECH (DingLpoZyt. J., 229, 466).-In the island Lesina, the rosemary plant attains a height of 30 to 62 cm., and, where it is carefully cultivated, 125 cm., the stems having a diameter of 2 to 3 cm. The glands filled with the ethereal oil (Oleum rosmnrini) are situated on the under side of the leaves. The manufacture of this oil in Lesina is increasing daily. Alt>hough no positive data exist as to the production of this oil, it is nevertheless known that Lesina ten years ago sent out 30,000 fl.Austr. worth of it. Every third year the biennial sprouts of the rosemary shrub are clipt in the month of May, the branches being dried for a week in the sun, and then deprived of their leaves. The distillation of the oil is made in copper stills, placed close by the sea shore, and heated over an open fire. Before charging the still, the dried leaves are moistened with water. The oil volatilising with the vapours of water passes through a worm and is collected in bottles. After separating t h e water from the oil, the latter is filled into tin vessels and sent to Trieste. Rosemary-oil is mostly used in perfumery, but is also added in small quantity to olive-oil ; the latter suffers no loss in value for technical purposes by this treatment, whilst the high duty imposed on olive-oil is avoided.From Trieste 17,000 to 20,000 kilos. of rosemary-oil are annually brought into commerce at an average price of 2 fl. per kilo. In France and Spain an alcoholic extract has for some time been prepared from this oil and other perfumes, which was known under the name of aqua regime Hungariae. This preparation had its origin in Lesina. Besides rosemary-oil, the dried leaves of this phnt are sent into commerce as spices, and for use in the smoking of meat, and for the preparation of rosemary-wine and rosemary-vinegar. Inactive Glucose in Crude Cane-sugars. By U. GAYON (Compt. rend., 87, 407).-The optically inactive glucose contained in crude cane-sugar and in molasses has been supposed to consist of a mixture of dextroglucose and levoglucose in due proportions.The paper describes experiments which confirm this opinion, and exhibit a means of transforming, by fermentation induced by pure Jlucor cir- ciqLeZZoides, the glucose of molasses into alcohol, and consequently of extracting additional quantities of crystallisable sugar from it. Analyses of Lamp-black made from the Natural Hydro- carbon Gas of the Ohio Petroleum Region. By J. R. SANTOS (Chem. News, 38, 941.-There are two wells in Knox County, Ohio, near the junction of the Kokosing and Mohican rivers, yielding very large quantities of hrdrocarbon gas, which Nee, of Gambler, has J. M. T. D. B. R. R. YOL. xsx\-1, ?Lutilised in the manufacture of a lamp-black, which he calls " diamond black." In the building used, 1,800 burners are at work, consuming about 275,000 cubic feet of gas per 24 hours, being about one-fourth of the available supply.The following is the composition of t.he gas by volume :- CHd. CpH6. N. 0. CO. CO,. 81.4 12.2 4.8 0% 0.5 0.3 = 100.0 Hydrogen, although not mentioned, is, according t o Sadtler, present in small quantity. The lamp-black is a t present manufactured to tho extent of about 16 tons per annum. It is very fine and smooth, free from coarse or gritty paiticles, and of a deep blue colour. It is sold to makers of fine printing and lithographic ink in the Unitcti States. The following analysis was made :-Sp. gr. a t 17" after corn- plete expulsion of air, equals 1.729. The air-dried lamp-black lost by exposure at ordinary temperature over sulphuric acid 2.30 per cent.of moisture, and a furt,her loss of 0.40 per cent. was experienced by lieating to 100". Continued heating at 200" and then a t 300" under atmospheric pressure gave rise to no further loss, but a miniitc: amount of water was expelled by subsequently heating in a Sprengcl 1-acuum. I. Carbon.. . . 96.041 Hydrogen.. . . 0.736 11. ), . . . . 9G.011 ,, . . . . 0.747 The occluded gases, driven out by heating to low redness in a Sprengel vacuum, represented, on calculating weight from volume :- co. CO?. N. Vapour of water. 1.378 1.386 0.776 0.682 p.c. by weight. There was also expelled and condensed on the cooler part of tile tube 0.024 of a solid light-yellow hydrocarbon, soluble i u alcohol, fusible, and volatilising rapidly under atmospheric pressure betweeii 215" and 220" (impure naphthalene ?).Hence the composition of the lamp-black may be calculatcd as- The material dried at 200" gave in two combustions :- Ash C. H. N. CO. COZ. 3320. (FZO, + CuO). 95.057" 0.665" 0.776 1.378-f 1.386-f 0.682 0.056 = 100.000. The Part played by Coal-dust in producing Explosions in Coal Mines. By L. SlnioxrN (COW@ ye?td., 87, 195-197).- I~xplosions have been known to occur in coal mines which mere l ' r c ~ from explosive gases, and this is attributed to the presence in tlic galleries of the mine of finely-divided coal-dust, which, in the event of :i very slight explosion of fire-damp or of powder when blasting tlic coal, rapidly disengages its coal-gas and increases the force of the ex- plosion. A. J. C. D. B. * Including the C and 11 of 0.024 60lid hjdrocahoii.t. These gases were doubt lcjs l)ai*tlj foriiiecl froin solid carbon and O L * L ' ~ L L ~ E ~ osjgen b j the lieat applied in tlic \ LLLCIL~III~.Abnormal Solubility of certain Bodies in Soaps and Alka- line Resinates. By A. LIVACHE (Coinpt. rend., 88, 249).- Tbc soaps known in commerce as “ petroleum soaps’’ are made by adding to ordinary soap petroleum mixed with a certaiu proportion of Carnauba wax. On heating the soap, the petroleum easily distils out, leaving the soap unaltered; these soaps are entirely solnble in water. This lattsr property is due to the Carnauba wax which they contain, or rather to the melissic alcohol contained in that body, for petroleum done is quite insoluble in soap solution, but dissolves in melissic i~lcohot. Other bodies, such as wood-spirit, amyl alcohol, &c., act in like manner, very small quantities of these solvents sufficing to dis- solve as much as 50 per cent.of petroleum in soap. Turpentine oil arid other liquids, suspended in soap-solution, dissolve on addition of coal-tar oil dissolved in the same solution. c. w. w. Kallab’s New Bleaching Process for Animal Textile Fibres. (IJijLgZ. poZyt. J., 229, 89--92).-The following method has been used with success by the author for bleaching silk, and more especially wool with the use of indigo and Schutzenberger’s hyposulphurous acid, H2S02 (Dhzgl., 225. 383). The material to be bleachcd is cleaned in the usual manner (DhgZ., 225, 389) and brought in its moist s h t e iuto a bath of clean water at the ordinary temperature, to every 100 litre of which 0.5 to 1 gram of finely-powdered reddish- blue indigo has been added.After a short treatment in this bath, tlic material is taken ont, pressed, and taken to the bleaching bath. Thc latter consists of a solutioir of freshly-prepared sodium hyposulphite o t’ 1.0069 to 1.0283 sp. gr. ; to each litre of liquid 5 to 20 C.C. of 50 pe?. cent. acetic acid are added. The latter must be free from stroil:,. mineral acids. The operation is conducted in closed vessels. Thc mechanically adhering indigo is reduced to indigo-white, and taker1 u p in a dissolved state by the fibre, whilst the sulphurous acid give11 off simultaneously bleaches the latter. After 6 to 24 hours’ exposures in the bath, a sample is taken out.If the latter is quite white and shows a slight bluish tinge, the operation is finished; the whole is taken out of the bath, allowed to drain, and finally exposed t o the air. The indigo-white is reconverted into indigo blue, producing a per- fectly fast azurage of the fibre. If concentrated bleaching baths ai-c used, a subsequent treatment with 0.5 t o 1 per cent. solution of crgs- tallised soda may be recommended. Loose wool may be bleached in :L inore concentrated bath of 1.0356 to 1.0431 sp. gr., without the addi- tion of acetic acid. For yellow shades, it is preferable to use calcium hyposulphite instead of the sodium salt, a bath of 1 to 1.0283 sp. gr. bcing the most suitable. In this ease the previous treatmect with indigo is unnecessary. If the white shows a greenish tinge, the stufl’ is drawn through a water-bath acidulated with hydrochloric or sul- phnric acid.For silk, the bleaching liquid must be much weaker tlinn for wool. This process may also be employcd for bleachiiig l’csthers, bathing sponges, lines, hemp, cotton, wood, and straw. Advantages of only Partially Removing the Fat in Oil- 13y L. W ~ ~ I R ~ A C K (IlijiyZ. p07yf. J., 229, 167).-Whcn soiuc D. B. Seeds.100 ABSTRACTS OF CHEMICAL PAPERS. time ago the idea originated of extracting the fat from oil-seeds by means of carbon bisulphide instead of by pressure, it was generally feared that the residue could not be used as fodder, becanse at that time no satisfactory method had been found of completely removing the carbon bisulphide.Since it has been found possible in practice to completely remove the carbon bisulphide from the residue, the latter has been largely used as fodder, with advantage both as to the yield of milk and also with regard to the breeding and fattening of animals. I t was, however, regretted by farmers that during the last decade the extrac- tion of fat had become so perfect, that the residue was poor in f a t compared with that obtained by pressing. It nevertheless remains to be proved whether for fattening purposes an increased quantity of fat is needed, the mast itself being very nourishing. Trials made by Wolff, Funke, and Kreuzhage in this direction gave no material dif- ference, although it is stated that an increase in the quantity of fat undoubtedly has a more nutritious action, especially with regard to the fattening of animals, from the increased utilisation of the whole fodder in the formation of fat and flesh.For this reason manu- facturers have given up the idea of completely extracting the fat from oil-seed. Moreover, by extracting merely a large proportion of the fat, they are able to operate on a much larger quantity of seeds with the same plant. D. B. On Tanning and Mineral Tanning. By GOTTFRIEDSEY (Dingl. polyt. J., 229: 180--182).-The editor of the Halle aux Cuirs in Paris obtained some time ago samples of iron-tanned leathci. (Knapp’s patent, DingE., 227, 86 and 185) from Gottfriedsen, of Braunschweig ; these were forwarded to Muntz, who, after examining them, published his results in that Journal (January 10).He con- siders that real leather always consists of a chemical combination of the tissues of the skin with tannin, every mechanical or physical union being merely a false leather without real value for application. He therefore subjected iron-tanned leather to a treatment with sulphuric: acid, and concludes from the results obtained, that the ferric oxide is not present in a combined form, and, moreover, that iron-tanned leather is not leather at all, but is perfectly useless as such. According to his views, the oxide in iron-tanned upper leather is merely a solution of ferric oxide in fat. Howevei., by comparing mineral tanned leather with ordinary leather (tanned leatlier), he does not go further than the “ evident proof’’ that, the latter is a chemical combination, without giving any explanation as to what this evidence is.The authors, therefore, undertook to complete this investigation. They found that leather made with vegetable tannin was more easily decomposable than iron-tanned leather. The same was the case with tanned or chamois leather. D. B.TECHNICAL CHEMISTRY.T e c h n i c a1 C h e m i s t r y.Gas Lighting. By J. VAN EYNDHOVEN (Dingl. polyt. J., 229,449).-It has been supposed that the gas flame is translucent. As,however, this appeared doubtful to the author, he determined to in-vestigate the subject. The experiments were made with the aid of anexcellent photometer, the results being as follows :-The first experiments were madewith a bat's-wing burlier of 160 litres'gas consumption a t 8.3 mm.pressure. The result of ten observationsproved that the lighting power of the flat side was equal to 11.58, thatof the narrow edge 10.04 candles. After correction for barometerand thermometer, the actual lighting power for normal consumptionof gas and candle is 11.81 and 10.18 candles: English spermaceticandles with a normal consumption of 120 grains were used. For aflame consuming 100 1. of gas per hour, the actual illuminatingpower on the flat side was 9.03, on the narrow edge 7-42 candles, m7it.ha gas pressure of 4 mm. The difference in both cases is 1.5 candles,or 1 7 to 18 per cent., a circumstance which proves that the flame isnot translucent, a bat's-wing burner giving most light on its flat side.An argand burner will from a similar cause not give all its illumina-ting power.For a good street illumination, therefore, the slits of theburners and the direction of the road must be placed perpendicularlyon one another. D. B.Some Peculiarities of the Vartry Water, and the Action ofthat Water on Boiler-plates. B,y C. R. C. 'YICHUORNE (Cheiri,.News, 38, 191).-The water of the River Vartry consists of organicmatter of a peaty nature, and mineral matter, which consists chieflyof the chlorides of the alkalis and of the alkaline earths; nitratesand nitrites are also present, which, however, cannot be detected with-out evaporation, but as concentration by heat reduces the nitrates, thewater was concentrated in a vacuum. This reduction, when it takes placein high pressure boilers, is a cause of the corrosion of the boilerplates, It was found that when iron was heated with nitrates insealed glass tubes it became oxidised.E. W. P.Preservation of Potable Water. By H. SCHIFF (Deut. Chem.Ges. Ber., 11, 1528--1529).-Water containing 3 parts of salicylic acidin 10,000 was found to be fresh after remaining in a flask for threeyears. Sea-water to which phenol or, preferably, carbon bisulphide(1 part to 1,000) has been added, forms a good preservative fluid forspecimens of marine fauna. w. c. w86 ABSTRACTS OF CHEJIICAL PAPERS.Utilisation of Suint from Wool. By F. FISCHER (Dim$. polyt.J., 229, 446--449).-1t is known that raw wool contains about90 per cent. of suint soluble in cold water, consisting of the potassiumcompounds of oleic, stearic, and acetic acids, a small amount of valericacid, and many other organic substances, also of potassium chlorideand sulphate, ammonium salts, and especially potassium carbonate, andsodium compounds.By lixiviating wool with water, a dark brown liquid of peculiar smellis obtained, of sp.gr. 1.069; I. litre of this required, for neutrali-sation, a quantity of normal acid corresponding with 3.98 grams ofpotassium carbonate. By neutralising 1 litre of liquor with hydrochloricacid and shaking up with benzene, only 916 milligrams of a yellowstrongly smelling fat were obtained. By evaporating 1 litre and dryingat 120°, 122.16 grams of a hygroscopic mass remained, which on igni-tion swelled up considerably, and evolved a, gas burning with a brightflame. By continued heating in the air, and extracting with water andevaporating, 72.16 grams of a white saline mass, and 2.98 grams of aresidue consisting of sand, alumina, lime, and phosphoric acid re-sulted.By burning the suint dried at 120" in a stream of oxygen,3.04 per cent. of hydrogen as water and 19.92 per cent. of carbon 8scarbonic acid were obtained. The organic compounds of potassiumare hereby converted into potassium carbonate.A profitable recovery of the fat and the acetic acid is impossible,but the utilisation of the evaporated mass for gas and the productionof potash can be recommended. For obtaining the potash present i r ithe mass, the latter is in Germany merely heated strongly in rever-beratory furnaces, the gas formed being used as fuel.Analyses of thecomposition of the flue gases showed that carbon monoxide is, in spitc ofthe sooty nature of the flame, formed very rarely, and only when themass is at its highest heat, in which case oxygen disappears. As soonas the evaporated liquors begin to burn, the heat evolved suffices todestroy all organic matter present. Thus with 1 kilo. of Westphaliancoal 12 kilos. of liquom can be evaporated and ignited. The cokeformed is solid. The following is the analysis of the coal dried a t120" :-C. H. S. 0 (and N). Ash.76.11 4.52 1-19 10.06 8-12The raw potash taken from the furnace gave-Salts soluble in water. Insoluble. Organic matter.92-05 4.92 3-03The composition of the soluble salts was as follows:-K,C03.KC1. KZSO4. NasCO3.85.34 6-15 2.98 5.02 = 99.49 p.c.W. Graff, in Lesum, works up this raw potash from six establishmentsfor washing wool into pure potassium carbonate, bicarbonate, chloride,and sulphate. He employs about 10 to 12 workmen, the annual saleamounting to about 120,000 marks. D. BTECHXICAL CHEMISTRY. 87Ingredients.Analyses of Clays. (Dingl. polyt. J., 229, 451455).--Glaze-clay.-As a very durable, perfectly impervious glaze on refractory clay,e.g., for Bunzlau vessels, water pipes, &c., a very readily fusible clay18 often used. Seger has analysed three specimens of t'hese earthyglazes with the following results :-A. 58-99 11.73 4.16 4-77 1.83 4.83 16-19 4.80B. 64.49 14.35 4.38 4.13 1-53 3.69 3.12 3.31C.62.40 15.51 5-68 4.36 1-13 3.62 2.88 4.41A is one from Naumburg 0. Q, used in Bunzlau for the manufactureof brown kitchen utensils and water pipes ; B from Camenz i. S., usedfor the same purpose, and C is a glaze from the clay pipe manufactoryin Dommitzsch 0. Elbe.The pyrometric investigations showed that, according to Seger'squotients of refractoriness (ibid., 228, 2M), the Naumburg glazewas the most readily fusible, that of Dommitzsch the most difficultlyfusible.Stoneware-cZa$.-This clay, obtained from Hohr, and representing theraw material used for the manufacture of the fine, compact, pearl-greyvessels a t that place, had the following composition :H20 andSiO,. A1,03. Fe203. CaO. MgO. Alkalis. CO2. organic matter.Si02.Al,O,. Fe203. CaO. MgO. K20and N%O. H,O.70.12 21.43 0.77 0.00 0.39 2-62 4.92By sulphuric acid.Wilkins has already pointed out the important influence which alarge amount of silica in clay has on the lustre and the fineness of thesalt-glaze ; an observation which confirms the ready acceptation of thesalt-glaze and the peculiar compactness of the above mass.Porcelain Eurth of Linzoges.-These clays are not merely distin-guished by the fineness of their forms, but the mass itself possesses apurer, more agreeable coloration, and greater fineness and strong trans-parency than the greater number of the German productions. Thefollowing is the composition of the kaolin :-i ISi02 ....................Fe203. ...................CaO ....................MgO ....................K,O ....................Na.20 ....................Loss by ignition ..........A120,.................... 58 -3927.520.361 -520 '411 -712 *587 -1999 -6832 2227.49 -4'40 J -26 *1720 '030 -361 -827 -19Clay sub-stancedecomposiblesulphuricacid.bY47 '0936 *040 '643 *2712 -988 ABSTRACTS OF CHEMICAL PAPERS.Kot decom-posibleCorresponding with-Clay substance ................ 55.88Quartz:. ....................... 5.95Felspar. ....................... 38.1 7Compared with the composition of the German and Austrian kaolins(ihid., 228, 67), this substance is distinguished by an unusuallyhigh percentage of felspar, which explains also the fact that in S h e sthe mass is not mixed with felspar but merely with sand.The porcelain from Limoges had the following composition :-Decompos-ibleIngredients.SiOa ....................CaO ....................MgO ....................K20 .....................8 1 2 0 3 .. ..................FezO,. ...................N+O ....................Loss by ignition ..........66 -7121 '580 '470 -610 -372.931 -625 -5499-83-47 -275 '93 1 3'76--19 '4415 -65'0 -471 -775 -54Compositionof theclaysubstance.45 -3536 -501.094 *1312.92corresponding with clay substance = 43.04, quartz 26.46, and felspar30.50.The mass contains therefore more sodium, lime, and magnesia than,e.g., the Berlin porcelain, a circumstance which explains its readyfusibility and greater transparency.The glaze from Limoges consists of-SiOp.A1203. Fe203. CaO.Ingredients in p. c.. ............... 74.99 14.80 0.37 1.09Not decomposible by sulphuric acid. . 70.92 12.38 - 0.20Decomposible by sulphuric acid .... 4.07 2.42 0.37 0.89Ingredients in p. c.. ............... 0.36 4.31 3.49 0.65Loss byMgO. K20. NasO. ignition.Not decomposible by sulphuric acid . . 0.36 7 4 7Decomyosible by sulphuric acid .... - 0.68 - 0.60liurstenu?aZd-gZaxe.-This glaze adheres in the form of sand to thelignite strata, and is used in the preparation of the lead and tin enamelsfor the fabrication of stoves. According to Seger, the mass dried a t120" has the following composition :TECHNICAL CHEMISTRY s 89H,O and carbon-Si02. A1,03.Fe,O,. MgO. E@. aceous matter.Total.. . . . . . . . . . , . . 85.96 7.30 2.26 0.25 1.97 2.11,- Not decomposible by UHZSOa ....... . .. 80.03 2.69 - 1-08substance.. . . . . . . 5.93 4.61 2.22 1.14 2.12Eatable-cZay.-Pattison Muir has investigated a clay-substance fromMackenzie County, in South Island, near New Zealand, which iseaten by men and sheep in large quantities. It has the followingcompos’ , I t’ ion :-Decomposible claySi02. Al,03. Fe,03. CaO. MgO. NaC1. n20. Organic.61-25 17.97 5.72 1-91 0.87 3.69 7.31 1.77(according to R. Biedermann in Noiizb. d. Ver. fur Fuh. zo?z Ziegel?z.1878, 229).Gross~Zme?.ode-cZay.-This clay is highly refractory and possessesgreat cementing power. It is coloured light bluish-grey to white, isshiny, and breaks up in water to a fine slimy mass.The followingis the composition of the clay dried a t 120’ :-SiO,.r 1. - Chemically Mechanically Loss byAI203. combined. added. MgO. CaO. Fe203. K20. S. ignition.34.52 43.38 6.53 0.73 0.76 1.66 1.51 0.26 11-04This gives a chemical composition: 4.89(A1203, 1.65 SiO,) + RO,and the quotient of refractoriness (according to Bischof) = 2.96.D. B.Blair’s Process for Iron Manufacture. By J . IRELAND (Dingl.polyt. J., 229, 458--461).-This paper gives a detailed account ofthe improvements which have been recently made in the workingplant, also in the method of preparing iron sponge. A brief descrip-tion of the reduction furnaces is given; these consist of a group ofthree vertical retorts, each retort having a diameter of 914 mm., andbeing 8.53 m.high. The furnace is surrounded by an outer casing ofbrickwork, leaving a combustion chamber between the inside of it andthe outside of the retorts. The retorts were heated externally by gasjets, the air for combustion being supplied through apertures immediatelyabove the gas jets. I n 1876 Blair discovered, that by the addition ofa small quantity of alkali to the carbonaceous matter mixed with theore, the action of reduction was facilitated to a great extent, and orewhich took about thirty hours to reduce without alkali, could be per-fectly reduced in six hours with it. The existing furnaces, however,could not be altered in any way to suit the new condition of quickenedreduction.Blair therefore abandoned the whole principle of heating,and adopted a system by which a stream of hot carbonic oxide waspassed through the mass of ore and carbonaceous matter. The author,however, made use of the above furnace by dividing the cast-iron pipeinserted in the top of each retort into a number of smaller ones, so a90 ABSTRACTS OF CHEMICAL PAPERS.to present as small a column of materials to the action of heat as pos-sible. He used a furnace of a height of 6.4 m., the retort, being about3.2 m. high, with four inserted tubes. A fiirnace of this description,1.52 m. diameter and 12.92 m. high, produces from 60 to 70 tons ofiron, and costs about 12,000 marks.The cost of producing iron sponge will vary according to thelocality in which'the work is carried on, but with the furnaces intro-duced by Blair, the cost will be about 22 marks per ton, exclusive ofthe ore.Where several of the furnaces are in operation, the cost isless. Where the oye is rich and pure, iron sponge made from it canbe a t once made into tool steel, the quality of which cannot beequalled by that made from the best brands of Swedish bars. I n thecase of ore which is not so rich, the best way of utilising the spongemade from it is to melt i t in a cupola furnace, transferring the moltenmass to a Siemens-Martin furnace, wherein the mass is converted intosteel. The pig metal obtained in this manner will coiitain about 1.5per cent. carbon and 0.19 per cent. to 0.25 per cent. silicon.D. B.Phosphorus in Cleveland Ironstone and in Iron.By J. E.STEAD (Chew,. News, 38, 14-18 ; 29-31 and 39-42).--This papermay be divided into six sections: (1.) The compound or com-pounds in which phosphoric acid exists in the Cleveland ironstone.(2.) Method of eliminating phosphoric acid from iron ores. (3.) Thecompound in which phosphorus exists in Cleveland metal. (4.) Theeffect, physically and chemically considered, which phosphorus has onpig metal. (5.) Method of removing it from pig iron. (6.) Phos-phorus in bar iron. The following are the results of the analysis ofthe main Cleveland ironstone bed :-Iron in theStone Siliceous Phosphoric Loss by calcinedanalysed. Iron. matter. acid. Moisture. calcination. stone.Main: p. c. p. c. p. c. p. c. p. c.p. c.(1st foot 26.53 18.30 1.46 8.50 27.39 36.502nd ,, 29.54 10.90 1.13 9-10 29.80 42.083rd ,, 29.14 10.68 1-13 9.50 29.80 41.504th ,, 28.41 11.98 1.41 9-80 28.80 39-925th ,, 29.97 9.00 1.17 10.00 30.83 43.316th ,, 30.42 8.82 0.89 10.00 31.51 44.407th ,, 29.70 9-00 0.80 10.10 31.78 43-538th ,, 29-85 9.29 0.91 9-80 30.90 45-209.00 28.50 42.40 C9th ,, 30.30 12.01. 1.16Black hard.4 7 inches 30.56 12-90 0.44 8.50 26.80 41.75 *s {; ,, 37-87 22.20 1-12 5-50 18.00 34.00,, 27-26 24.70 0.81 5-00 17.00 32.85It will be seen from these analyses that no part of the stone is freefrom phosphoric acid. In the " Black Hard " bed, the author foundthis substance very variable in quantity, reaching as much as 3 percent. in some cases, and only 0.25 per ceut.in others.dCTECHNICAL CBEJIISTRT. 911. As to the form in which phosphoric acid exists in Clevelandironstone, the author mentions that several years ago Pattinson inves-tigated this matter and concluded, judging from the non-action ofammonium sulphide on the stone, or rather on the compound contain-ing phosphoric acid in the stone, that no iron phosphate was present,and that the phosphoric acid must be in combination with lime ; andthe results obtained by other methods of investigation employed bythe author has confirmed this. It is the prevailing opinion that thesource of all the phosphorus in the ironstone is the remains of smallphosphatic animals ; but this theory cannot be regarded as trustworthy,first, because in some parts of the “ Black Hard ” bed, where no fossilremains could be detected, the phosphoric acid has been found in largequantity, and secondly, because in all cases, on analysis, the shells andfossil remains which were taken out of the stone, were proved to con-tain much less phosphoric acid than the surrounding ironstone.Thefollowing analyses of fossil wood taken from various mines in thatdisirict will throw some light upon this very obscure subject.Fossilised mood found in Cleveland ironstone-OH,. C. SiO,. (20%. SO3. S. MU. d1203.3.00 9-60 0.50 0.75 0-GO 7-56 trace 8.25COO and NiO. Co and Ni. Fe. FeO. MgO. P,05. CaO.3.70 1-65 5.20 10.02 1.12 20.80 27.60Several other samples gave similar results on analysis. There canbe no doubt about the fact, that these samples were at one time partsof trees, which in their natural state would not, contain more than veryminute quantities of phosphoric acid.The latter must have been insolution, and has in this state passed into the substance of the woodand been there deposited in the condition in which we find it.2. Method of Removing Phosphoric Acid from Ores.- Jacob’s method,based on the treatment of the ores with sulphurous acid produced byburning sulphur pyrites and condensing the acid fumes in coke towers,gave satisfactory results only when the stone was reduced to a veryfine powder, about 90 per cent. of phosphoric acid being removedthereby. Forbes’ method, based on the action of common salt on ironphosphate when fused, also gave unsatisfactory results, as did the lastmethod referred to by the author, the action of sodium carbonate onphosphate of lime when fused with it.From this it would seem thatCleveland ironstone cannot be freed from phosphorus by any methodsas yet proposed. With regard t o the smelting of ironstone, since weknow that phosphate of lime heated with carbon aud iron oxides, ormetallic iron, to a very high temperature, is decomposed, the phos-phorus combining with the iron, it is to be expected that nearly all of thephosphorus introduced in the charge at the top of the blast-furnace, willbe found concentrated in the pig metal. Experiments showed thatfluorspar is of no value in removing the phosphoric acid or preventingits passage into the metal when employed as a flux in smelting.Iro?z a i d Phosphorus.--By direct addition of phosphorus to iron heatedin a crucible, the author obtained combinations containing between 6 mi92 ABSTRACTS OF CHEMICAL PBPERS.27 per cent.of phosphorus, although Percy has stated that iron will nottake up more than 8.4 per cent. of phosphorus when the two substancesare heated together in the manner described. The fusion pointappears to decrease with each addition of phosphorus, until a com-pound containing from 10 to 12 per cent. of phosphorus is produced,which is the most fusible ; after which each addition makes the com-pound less and less fusible.3. The Co~npount7s in which Phosphwus exists in Clemdand Jfeta1.-Judging from the comparative fusibility of iron, it was thought thatif separate compounds of iron and phosphorus existed in pig metal,these compounds would be more fusible than the bulk.Analyses ofabout 1 cwt. of Cleveland iron poured into a mould were made. Afterthe mass had become viscous, extreme pressure was applied by meansof a hydraulic ram, and the portions of metal last fluid expressed.The expressed metal was found to be n combination of phosphide ofiron and unaltered pig metal in the proportion of 51.5 : 48.5 or 88.05per cent. of iron and 11.95 per cent. of phosphorus ; or, calculated intochemical equivalents, they are in the ratio 1.57 iron to 0.385 phos-phorus or 4 equivalents of iron to 1 of phosphorus, and the formulamay therefore be written Fe4P. It is very clear from these results thatphosphide of iron does exist in a separate state in pigmetal intimatelydiffused throughout the mass.On immersing bar iron in dilute acid,such as hydrochloric acid or sulphuric acid, a black residue is observedadhering to the outside of the iron. In these residues, phosphides ofdifferent constitution were found, the iron and phosphorus being pre-sent as Fe3P4 and Fe3P,. This fact proves that iron containing phos-phorus contains two or more different phosphides, and that they existin very varying proportions in different samples of iron.4. The Efect which Phosphorzis has on Pig metal ( a ) . Physicnl Pro-perties.--Experiments have shown that, as a considerable quantity ofiron is in combination with phosphorus in Cleveland iron, there isless iron remaining capable ut taking up silicon, than is the casewhere no phosphorus is present: consequently less silicon w7ill berequired to give to the smaller proportion of iron t,he conditionsnecessary for the production of glazed iron.( b . ) ChemicaZ Properties.-When sulphur is added to fluid metal-which under ordinary circum-stances would assume a grey fracture when cooled and broken-thesulphurised iron when cold will present a mottled or white fracture.I n other words, sulphur prevents the separation of carbon as graphite.I n order to ascertain if phosphorus has a similar action, experimentswere made which proved that the effect of phosphorus compared withthat of sulphur is very small, and would not affect materially thequality of the iron or pig in this direction, even if increased in con-siderable quantity.5 .Methods of removi?Ag Phosphorus from Pig metal.-The action ofoxide of iron as a purification method is well known, but it has fre-quently been supposed that oxide of iron, without the aid of mechanicalpower, has very little action, and that the work a puddler gives to themetal has some important action in removing phosphorus independentof the oxide of iron. By the results obtained from numerous experi-ments it has been clearly proved that mechanical power, whether ibe in the force of the refining blast, the motion of the puddler’s bar,or the revolving of the rotary puddling machine, is simply the meaiisby which the molten iron is brought into intimate contact with thefluid or semi-fluid oxide of iron, The removal of phosphoras dependsentirely on this, and not on any mechanical force.It is furtherillustrated experimentally that, when the puddling process is con-ducted a t a very low temperature,or when the cinder is run out of thefurnace before the phosphorus is removed, the puddled bar producedis high in phosphorus. i n the first case the temperature is not highenough to liquefy the necessary amount of cinder required for thepurification of the metal, and as a consequence, there is left an impureiron ; whilst in the other, when the cinder is removed from the semi-purified iron the purifying agent being taken away, the removal ofphosphorus is retarded and a pliosphuretted iron is produced. On theother hand, when a high temperature is maintained, a very excellentquality of bar is produced.6.Iron Heated with Phosphoric Acid.-It is stated that pure iron at ared heat has no power to decompose phosphoric acid ; but, if the iron beheated to its fusion point, the acid is readily decomposed. Pure ironwas fused with puddler’s tap-cinder, containing above 4 per cent. ofphosphoric acid, in order to determine whether or not pure iron woulddecompose phosphoric acid when in combination with iron oxide : thebutton produced contained = 2.12 per cent. Pure iron was nextfused with phosphate of iron, and the metal, after fusion, was found tocontain 2.68 per cent. of phosphorus. The nature of the actionbetween oxide and phosphide of iron was proved by experiments tobe not physical but chemical.The button obtained weighed about15 per cent. more than before such treatment.6 . Phoqhorus in Bar-iron.-From the following results i t will beseen that a considerable amount of phosphorns is removed by simplyheating and rolling iron containing i t ; and that it is oxidised andremoved from the iron, whereby the quality of the bar is improvedconsiderably. No. 2 ordinary bar-iron made from Cleveland pig wastwice piled and rolled. No. 4 bar, produced after the second rolling,was excellent fibrous iron, and very soft, whereas, before the treatment,it was in great part crystalline and hard:-Phosphorus combined Phosphorus in Phosphorus.with iron. cinder. Total.p. c. p. c . p. c.2. 0.243 0.087 0.333.0.130 0.110 0.244. 0.071 0.149 0.22The following is an analysis of three finished bars made fromCleveland iron, puddled in the Danks’ furnaces at the Tees Side IronWorks. It would be difficult to obtain better iron thaa this:-I. 11. 111.p. c. p. c. p. c.Carbon .. .. . . .. 0.080 0.110 0.160Silicon .... .. .. 0.092 0.046 0.040Phosphorus . . . . 0.110 0.060 0.073Sulphur .... .... 0.012 0.016 0.0194 ABSTRACTS OF CHEMICAL PAPERS.Pliosphorus combined Phosphorus in Phosphorus.with iron. cinder. Total.p. c. p. c. p. c.1. 0.057 0.063 0.1 102. 0.023 0.037 0.0693. 0.034 0.039 0.073I n the third portion of his paper the author describes some of thechanges which take place when air is blown through phosphurettedmetal, and censiders the value of manganese oxides, chlorine, bromine,iodine, and hydrogen as agents for removing phosphorus, leaving thequestion of ore purification as a yet unsolved problem, and one whichwill not be readily solved to the satisfaction of the practical ironmanufacturer.When metal containing mangnnese, silicon, carbon, and phosphorusis acted upon while in the fluid state by a stream of air, there is everyreason to believe that all the elements present, probably with the ex-ception of carbon, are oxidiscd in the ratio in which they exist in themetal, and this should give a very basic cinder. Such, however.is notthe case: for almost instantly after the formation of cinder, themanganese, silicon, and phosphorus still present in the fluid massare oxidised by the oxygen of the protoxide of iron, while the reducediron, leaving the cinder, returns to the bath and is replaced by theoxide of manganese, silicon, and phosphorus.In consequence ofthe rapidity with which these reactions take place, the cindeydrawn off from the metal is always more or less saturated with silica,phosphoric acid, and manganese oxide. la a Bessemer converter,when the temperature is low enough, there can be no doubt that a tfirst all ingredients are burnt just in the proportion in which they arepresent. Such, however, is tlie violent agitation to which the metalis subjected, that the cinder and iron are continually in intimate con-tact, and as a consequence, the cinder is very rapidly saturated withsilica and phosphoric acid.In the Bessemer converter, after thesaturation point has been reached, when the silica and phosphoric acidhave both in combination with them the proper chemical proportion ofoxide of iron, the still unoxidised silicon in the metal will continue toreduce the oxide in the cinder, and will replace i t by silica. It isclear that when this point has been attained, viz., the removal of abase and the substitution of an acid in a compound already saturatedwith acid (silica), silica must be in excess, and that, as this acid ismuch niore powerful than phosphoric acid, i t will take away the oxideof iron a t first in combination with it, by which reaction silicic acidarid iron phosphates are transformed into phosphoric acid and ironsilicate.Experiments were. undertaken which afforded proof of thetheory, that manganese is capable of reducing free phosphoric acid a ta comparatively low temperature. It was further shown that theattraction of silicon for oxygen is greater than the attraction of phos-phorus for that element, and that when free phosphoric acid is exposedto the action of silicon, as i t exists in fluid metal a t low temperatures,oxygen is withdrawn from the phosphoric acid, and combines with thesiiicon to form silicic acid. The results of an experiment in whichfluid iron containing little or no silicon or manganese, was poureTECHSICAL CHEMISTRY. 95upon solid phosphoric acid placed at the bottom of a red-hot crucible,clearly showed that the acid had suffered decomposition.As the question as to the point a t which oxide of iron becomessaturated with silica is very important, several experiments were madewith the view of solving it.F o r this purpose cinder containing littlemore than a trace of phosphoric acid wils mixed with variable propor-tions of sand, and, after fusion, was agitated with fluid iron containingphosphorus. In each case the metal was tested for phosphorus aftertreatment, and if no diminution was detected, it was concluded thatthe cinder employed contained no free iron oxide. The results wereas follows :-No. 1. No. 2. No. 3. No. 4.p. c . p. c. p. c. p. c.Protoxide of iron.. ...... 73.90 64*.50 55.50 47-68Sesquioxide of iron. ..... 11.60 10.60 8.50 6.87Silica.. ................10.50 20.40 31.00 40.00Alumina, lime, &c. ...... 4-00 4.50 5.00 5.45100.00 lOO.00 100.00 100.00No. 5. No. 6. No. 7. No. 8.p. c. p. c . p. c. p. c.Protoxide of iron ........ 42.13 43.41 38.57 29.57Sesquioxide of iron ...... 10.71 8.13 7.86 5.00Silica .................. 44.00 46.00 51.00 62.50Alumina, lime, &c. ...... 3.16 2.46 2.57 2.93100*00 100*00 100~00 100.00Metallic iron.. .......... 65.60 57.60 49.12 41.89Ratio of iron to silica . . . . 1 to 0.16 0.35 0.63 0.95Before treatment ........ 1.51 1.51 1.48 1.48After treatment.. ........ 0.13 0.04 0.2.5 0.75Phosphorus in metal-Metallic iron.. .......... 40.27 38.34 38.50 26.50Ratio of iron to silica .... 1 to 1-06 1.20 1.44 2.36Before treatment ........ 091 0.91 0.91 0.91After treatment.......... 0.89 0.90 0.91 0.91Phosphorus in metal-It will be seen that when the ratio of iron to silica in the cinder isas 1 to 1.06, the compound is incapable of oxidising phosphorus fromfluid iron containing it. This ratio is almost exactly the same as thatof the chemical equivalents of iron and silica, viz., as 56 t o 60. Itwill be noticed that there has not been so much phosphorus removedin No. 1 as in No. 2, in which the cinder was dot so pure as in the firstcase, This, however, was due to the very sluggish nature of thecinder, which prevented its intimate admixture with the metal.It was proved by experiment that, within certain limits of tempera-ture, it is impossible to drive off from cinder its phosphoric acid b96 ABSTR.4CTS OF CHEMICAL PAPERS.the addition of silica.The analysis of the cinder made after fusionshowed that it tenaciously retains phosphoric acid, confirming thetheory that the whole of the phosphorus rerrioved in the various pro-cesses in which oxide of iron is used for purifying iron, is containedin the cinder, and that none is vaporised and carried iip the stackwith the waste products of combustion from the furnace grate.As t o the value of manganese oxides as agents for purifying ironfrom phosphorus, it is mentioned that the protoxide, retaining itsoxygen with much greater tenacity than the sesquioxide, and being de-composed a t very high temperatures only, in presence of reducing agents,is without any direct action on the phxphorus existing in the fluidiron ; as, however, this oxide has a much greater attraction for silicathan iron oxide, it plays a part of secondary importance in the cindersof the purifying processes by taking up the silica.By forcing per-oxide of manganese under the surface of molteii iron, i t is deprived ofhalf its oxygen, which, acting upon the oxidisable impurities in themetal, removes them. When oxide of iron acts upon phosphorus, foreach part of that element oxidised, 4.5 parts of pure iron are removedfrom the oxide, When manganese peroxide acts upon phosphorus theoxidation is effected by free oxygen, and therefore there is no gain bythe separation of metal. I t would seem, therefore, that peroxide ofmanganese is of much less value than iron oxides.With regard tothe value of fluorspar as an agent for removing phosphorus, the fol-lowing experiment was tried. The action of a mixture of fluid oxideof iron and fluorspar upon Cleveland iron was ascertained by fusingtwo-thirds of mill-tap and one-third of spar, and thoroughly wellmixing up with molten iron, the result being the removal of thegreater part of the phosphorus. AS to the use of chlorine, bromine,and iodine, it is mentioned that since all these elements form definitecompounds with phosphorus, which are all decomposed when broughtinto contact with red-hot iron, tthe phosphorus combining with theiron, t,here would be no advantage derived from their use. Hydrogenalso is incapable of removing phosphorus from iron, as iron will with-draw phosphorus from its combination with hydrogen. Water hasbeen advocated as an agent for removing phosphorus, it being heldthat the hydrogen would combine with i t and pass off as phosphorettedhydrogen. An experiment was undertaken with the following re-sults :-Pig metal. Before.After.Phosphorus.. . . . . . . 1.48 p. c. 1-48 p. c.Analysis of gases evolved from molten Cleveland iron in water :-79.69 12.48 4.87 1.74 1.22 None = 100H. co. CH4. H28. CO2. r205. p. c.The metal lost half its sulphur by the operation.111 concluding this paper the author remarks, that so far as ourpresent knowledge goes, there is nothing to surpass, in point of costand efficiency, the process of purifying by means of oxide of iron,D. BTECHNICAL CHEMISTRY.97Manufacture of a Red Pigment from Iron Scrap. By R. andC. STEINAU (Chem. Cen.fr., 1878, 336).-This pigment is formed byexposing wrought-iron shearings to the alternate action of air andwater, and heating the resulting hydrated oxide to redness with accessof air. Black is obtained by using reducing agents, and brown bymixing the two pigments.Preparation of Rosemary-oil. By C. 0. CECH (DingLpoZyt. J.,229, 466).-In the island Lesina, the rosemary plant attains aheight of 30 to 62 cm., and, where it is carefully cultivated, 125 cm.,the stems having a diameter of 2 to 3 cm. The glands filled with theethereal oil (Oleum rosmnrini) are situated on the under side of theleaves. The manufacture of this oil in Lesina is increasing daily.Alt>hough no positive data exist as to the production of this oil, it isnevertheless known that Lesina ten years ago sent out 30,000 fl.Austr.worth of it.Every third year the biennial sprouts of the rosemary shrub areclipt in the month of May, the branches being dried for a week in thesun, and then deprived of their leaves. The distillation of the oil ismade in copper stills, placed close by the sea shore, and heated overan open fire. Before charging the still, the dried leaves are moistenedwith water. The oil volatilising with the vapours of water passesthrough a worm and is collected in bottles. After separating t h ewater from the oil, the latter is filled into tin vessels and sent to Trieste.Rosemary-oil is mostly used in perfumery, but is also added in smallquantity to olive-oil ; the latter suffers no loss in value for technicalpurposes by this treatment, whilst the high duty imposed on olive-oil isavoided.From Trieste 17,000 to 20,000 kilos. of rosemary-oil areannually brought into commerce at an average price of 2 fl. per kilo.In France and Spain an alcoholic extract has for some time beenprepared from this oil and other perfumes, which was known underthe name of aqua regime Hungariae. This preparation had its originin Lesina.Besides rosemary-oil, the dried leaves of this phnt are sent intocommerce as spices, and for use in the smoking of meat, and forthe preparation of rosemary-wine and rosemary-vinegar.Inactive Glucose in Crude Cane-sugars. By U. GAYON(Compt. rend., 87, 407).-The optically inactive glucose containedin crude cane-sugar and in molasses has been supposed to consistof a mixture of dextroglucose and levoglucose in due proportions.Thepaper describes experiments which confirm this opinion, and exhibit ameans of transforming, by fermentation induced by pure Jlucor cir-ciqLeZZoides, the glucose of molasses into alcohol, and consequently ofextracting additional quantities of crystallisable sugar from it.Analyses of Lamp-black made from the Natural Hydro-carbon Gas of the Ohio Petroleum Region. By J. R. SANTOS(Chem. News, 38, 941.-There are two wells in Knox County,Ohio, near the junction of the Kokosing and Mohican rivers, yieldingvery large quantities of hrdrocarbon gas, which Nee, of Gambler, hasJ. M.T.D. B.R. R.YOL. xsx\-1, ?utilised in the manufacture of a lamp-black, which he calls " diamondblack." In the building used, 1,800 burners are at work, consumingabout 275,000 cubic feet of gas per 24 hours, being about one-fourthof the available supply. The following is the composition of t.he gasby volume :-CHd. CpH6. N. 0. CO. CO,.81.4 12.2 4.8 0% 0.5 0.3 = 100.0Hydrogen, although not mentioned, is, according t o Sadtler, presentin small quantity. The lamp-black is a t present manufactured to thoextent of about 16 tons per annum. It is very fine and smooth, freefrom coarse or gritty paiticles, and of a deep blue colour. It issold to makers of fine printing and lithographic ink in the UnitctiStates. The following analysis was made :-Sp. gr.a t 17" after corn-plete expulsion of air, equals 1.729. The air-dried lamp-black lost byexposure at ordinary temperature over sulphuric acid 2.30 per cent. ofmoisture, and a furt,her loss of 0.40 per cent. was experienced bylieating to 100". Continued heating at 200" and then a t 300" underatmospheric pressure gave rise to no further loss, but a miniitc:amount of water was expelled by subsequently heating in a Sprengcl1-acuum.I. Carbon.. . . 96.041 Hydrogen.. . . 0.73611. ), . . . . 9G.011 ,, . . . . 0.747The occluded gases, driven out by heating to low redness in aSprengel vacuum, represented, on calculating weight from volume :-co. CO?. N. Vapour of water.1.378 1.386 0.776 0.682 p.c. by weight.There was also expelled and condensed on the cooler part of tiletube 0.024 of a solid light-yellow hydrocarbon, soluble i u alcohol,fusible, and volatilising rapidly under atmospheric pressure betweeii215" and 220" (impure naphthalene ?).Hence the composition of the lamp-black may be calculatcd as-The material dried at 200" gave in two combustions :-AshC.H. N. CO. COZ. 3320. (FZO, + CuO).95.057" 0.665" 0.776 1.378-f 1.386-f 0.682 0.056 = 100.000.The Part played by Coal-dust in producing Explosionsin Coal Mines. By L. SlnioxrN (COW@ ye?td., 87, 195-197).-I~xplosions have been known to occur in coal mines which mere l ' r c ~from explosive gases, and this is attributed to the presence in tlicgalleries of the mine of finely-divided coal-dust, which, in the event of:i very slight explosion of fire-damp or of powder when blasting tliccoal, rapidly disengages its coal-gas and increases the force of the ex-plosion.A. J. C.D. B.* Including the C and 11 of 0.024 60lid hjdrocahoii.t. These gases were doubt lcjs l)ai*tlj foriiiecl froin solid carbon and O L * L ' ~ L L ~ E ~osjgen b j the lieat applied in tlic \ LLLCIL~III~Abnormal Solubility of certain Bodies in Soaps and Alka-line Resinates. By A. LIVACHE (Coinpt. rend., 88, 249).- Tbcsoaps known in commerce as “ petroleum soaps’’ are made by adding toordinary soap petroleum mixed with a certaiu proportion of Carnaubawax. On heating the soap, the petroleum easily distils out, leavingthe soap unaltered; these soaps are entirely solnble in water.Thislattsr property is due to the Carnauba wax which they contain, orrather to the melissic alcohol contained in that body, for petroleumdone is quite insoluble in soap solution, but dissolves in melissici~lcohot. Other bodies, such as wood-spirit, amyl alcohol, &c., act inlike manner, very small quantities of these solvents sufficing to dis-solve as much as 50 per cent. of petroleum in soap. Turpentine oilarid other liquids, suspended in soap-solution, dissolve on addition ofcoal-tar oil dissolved in the same solution. c. w. w.Kallab’s New Bleaching Process for Animal Textile Fibres.(IJijLgZ. poZyt. J., 229, 89--92).-The following method has been usedwith success by the author for bleaching silk, and more especiallywool with the use of indigo and Schutzenberger’s hyposulphurousacid, H2S02 (Dhzgl., 225.383). The material to be bleachcd iscleaned in the usual manner (DhgZ., 225, 389) and brought in itsmoist s h t e iuto a bath of clean water at the ordinary temperature, toevery 100 litre of which 0.5 to 1 gram of finely-powdered reddish-blue indigo has been added. After a short treatment in this bath, tlicmaterial is taken ont, pressed, and taken to the bleaching bath. Thclatter consists of a solutioir of freshly-prepared sodium hyposulphite o t’1.0069 to 1.0283 sp. gr. ; to each litre of liquid 5 to 20 C.C. of 50 pe?.cent. acetic acid are added. The latter must be free from stroil:,.mineral acids. The operation is conducted in closed vessels. Thcmechanically adhering indigo is reduced to indigo-white, and taker1u p in a dissolved state by the fibre, whilst the sulphurous acid give11off simultaneously bleaches the latter.After 6 to 24 hours’ exposuresin the bath, a sample is taken out. If the latter is quite white andshows a slight bluish tinge, the operation is finished; the whole istaken out of the bath, allowed to drain, and finally exposed t o the air.The indigo-white is reconverted into indigo blue, producing a per-fectly fast azurage of the fibre. If concentrated bleaching baths ai-cused, a subsequent treatment with 0.5 t o 1 per cent. solution of crgs-tallised soda may be recommended. Loose wool may be bleached in :Linore concentrated bath of 1.0356 to 1.0431 sp. gr., without the addi-tion of acetic acid. For yellow shades, it is preferable to use calciumhyposulphite instead of the sodium salt, a bath of 1 to 1.0283 sp. gr.bcing the most suitable. In this ease the previous treatmect withindigo is unnecessary. If the white shows a greenish tinge, the stufl’is drawn through a water-bath acidulated with hydrochloric or sul-phnric acid. For silk, the bleaching liquid must be much weakertlinn for wool. This process may also be employcd for bleachiiigl’csthers, bathing sponges, lines, hemp, cotton, wood, and straw.Advantages of only Partially Removing the Fat in Oil-13y L. W ~ ~ I R ~ A C K (IlijiyZ. p07yf. J., 229, 167).-Whcn soiucD. B.Seeds100 ABSTRACTS OF CHEMICAL PAPERS.time ago the idea originated of extracting the fat from oil-seeds bymeans of carbon bisulphide instead of by pressure, it was generallyfeared that the residue could not be used as fodder, becanse at thattime no satisfactory method had been found of completely removingthe carbon bisulphide. Since it has been found possible in practice tocompletely remove the carbon bisulphide from the residue, the latter hasbeen largely used as fodder, with advantage both as to the yield of milkand also with regard to the breeding and fattening of animals. I t was,however, regretted by farmers that during the last decade the extrac-tion of fat had become so perfect, that the residue was poor in f a tcompared with that obtained by pressing. It nevertheless remainsto be proved whether for fattening purposes an increased quantity offat is needed, the mast itself being very nourishing. Trials made byWolff, Funke, and Kreuzhage in this direction gave no material dif-ference, although it is stated that an increase in the quantity of fatundoubtedly has a more nutritious action, especially with regard tothe fattening of animals, from the increased utilisation of the wholefodder in the formation of fat and flesh. For this reason manu-facturers have given up the idea of completely extracting the fat fromoil-seed. Moreover, by extracting merely a large proportion of thefat, they are able to operate on a much larger quantity of seeds withthe same plant. D. B.On Tanning and Mineral Tanning. By GOTTFRIEDSEY(Dingl. polyt. J., 229: 180--182).-The editor of the Halle aux Cuirsin Paris obtained some time ago samples of iron-tanned leathci.(Knapp’s patent, DingE., 227, 86 and 185) from Gottfriedsen, ofBraunschweig ; these were forwarded to Muntz, who, after examiningthem, published his results in that Journal (January 10). He con-siders that real leather always consists of a chemical combination of thetissues of the skin with tannin, every mechanical or physical unionbeing merely a false leather without real value for application. Hetherefore subjected iron-tanned leather to a treatment with sulphuric:acid, and concludes from the results obtained, that the ferric oxide isnot present in a combined form, and, moreover, that iron-tannedleather is not leather at all, but is perfectly useless as such. Accordingto his views, the oxide in iron-tanned upper leather is merely a solutionof ferric oxide in fat. Howevei., by comparing mineral tanned leatherwith ordinary leather (tanned leatlier), he does not go further than the“ evident proof’’ that, the latter is a chemical combination, withoutgiving any explanation as to what this evidence is. The authors,therefore, undertook to complete this investigation. They found thatleather made with vegetable tannin was more easily decomposablethan iron-tanned leather. The same was the case with tanned orchamois leather. D. B