tween the anus and genitals, and is also found adhering to the trunks of trees from the animal rubbing on them. This secretion is a thick liquid, and is put into the horns of goats, or, for the retail trade, into small tin boxes. It is extensively used as a perfume, sometimes under the name of moskos, the men employing it on the turban and the women on their veils. Civet is also used as a remedy in hysterical and other nervous complaints, and is used for protecting cloths from moths, the cloths being kept in chests made of cedar or cypress wood. The price of a civet cat is from 2,000 to 3,000 piastres, and from 500 to 1,500 piastres are paid for the skins, which are used for furs.-Amer. Jour. Phar., Jan. 1883, 4. Musk-Masking of Odor.-Prof. Wiesenthal uses hydrochloride or sulphate of quinine, whereby the musk becomes inodorous. For removing the penetrating musk odor from the hands, it is sufficient to put a little quinine in the palm of the hand, moisten it with acidulated water, and rub the hands.-Amer. Jour. Phar., May, 1883, 374, from Phar. Post, 1883, p. 73.

INORGANIC CHEMISTRY.

OXYGEN.

Oxygen-Rapid Preparation.-Voracek recommends adding hydrogen peroxide to potassium permanganate, when the evolution takes place at the common temperature and without requiring special caution. According to "Industrie-Blätter," No. 15, a much cheaper source is barium peroxide, to 15 grams of which are added 100 cc. of a mixture of equal volumes of concentrated potassium bichromate solution and nitric acid, sp. Instead of the bichromate, potassium permanganate may be gr. 1.2. employed, but is more costly.-Amer. Jour. Phar., Aug. 1882, 407, from Arch. d. Phar., May 1882, p. 369.

Oxygen--Presence of Chlorine when Prepared from Chlorate of Potassium.-Schönbein observed that chlorate of potassium, heated with a little ferric oxide, yielded oxygen gas contaminated with chlorine. Pettenkofer & Voit have also noticed the presence of chlorine in oxygen gas prepared from a mixture of chlorate of potassium and binoxide of manganese (or powdered quartz, or oxide of copper). A. Wagner, having also made this observation, determined to ascertain the cause, and we quote here the results he arrived at:

Oxygen gas prepared from commercial chlorate of potassium (at least from that used by Wagner) is always contaminated with chlorine. On the other hand, chemically pure chlorate of potassium yields a gas completely free from chlorine, provided every trace of organic substances or carbonic acid gas is absent. Carbonic acid may decompose even chem

ically pure chlorate of potassium, when heated, so as to liberate some chlorine; the same effect is caused by organic substances, and, in this case, the residue has a strongly alkaline reaction. The presence of chlorate of calcium may also produce the separation of a little free chlorine, as has been already noticed by Wächter.-New Rem., Feb. 1883, 53, from Zeitsch. f. Anal. Chem., 1882, 507.

Active Oxygen-Characters.-Mr. E. Baumann believes that, in addition to ozone and the ordinary inactive form of oxygen, there exists yet another modification--active or nascent oxygen-which, like nascent hydrogen, does not admit of isolation, and can only be examined through its action on other bodies. The active oxygen (O) is the most powerful oxidizing agent known, and is in a state to combine with inactive oxygen (O), in order to form ozone (O). In its action it differs from ozone, in that it is capable of converting water into peroxide of hydrogen, and the nitrogen of the air into nitrous and nitric acid, which ozone does not. If a mixture of ozonized air and carbonic oxide be passed through baryta water, no turbidity is produced; carbonic oxide cannot be converted into carbonic anhydride by this means, as already pointed out by Remsen and Southworth. If, however, palladium foil saturated with hydrogen, be enclosed in a glass tube with clean lime water, oxygen, and carbonic oxide, turbidity is slowly produced. The active oxygen, developed under these circumstances, possesses a power which ozone does not.-Jour. Chem. Soc., July 1882, 691, from Zeitschr. Physiol. Chem. 5, 244-257.

Ozone and Teroxide of Hydrogen-Formation.-Professor S. Kappel, during his researches on the formation of nitric and nitrous acids from ammonia in contact with copper and air (see nitrogen), has made some interesting observations relative to the formation of ozone and peroxide of hydrogen. He had experimented to determine whether nitrites could be formed from the nitrogen of the air in presence of caustic alkalies and copper, and sums up his observations as follows:

1. When pure air is passed through a pure alkaline solution, in contact with copper, there is scarcely any formation of nitrites, but ozone and peroxide of hydrogen are formed.

2. The alkali is primarily concerned in the formation of the peroxide of hydrogen, with which it combines, and which is liberated on the addition of an acid.

3. Inasmuch as these reactions only occur in the heat, the view that peroxide of hydrogen is an endothermic compound is confirmed.

4. Metals which liberate hydrogen in contact with alkalies, such as zinc, etc., are incapable of producing ozone, because the nascent hydrogen causes reduction.-Arch. d. Phar., Aug. 1882, 573-577.

Ozone-Action on Metallic Salts and Oxides.-Mailfert has studied the action of ozone on metallic salts and oxides, with the following results :

Mercurous Salts.-The nitrate is entirely decomposed by ozone, with formation of mercuric nitrate and a yellow precipitate of trimercuric nitrate. The sulphate behaves in a similar manner, mercuric sulphate and basic sulphate being formed. Mercurous chloride is acted on somewhat more slowly, with formation of mercuric chloride, and a brick-red precipitate, apparently an oxychloride. The bromide is acted on in a similar manner. With the iodide the action is extremely slow, mere traces of red precipitate being produced even after the ozonized gas had been passed for 15 hours.

Silver Salts.-With the nitrate, a bluish-black flocculent precipitate of peroxide is produced, which, however, is decomposed and redissolved on agitating the solution. The sulphate likewise gives peroxide, but the chloride and the cyanide are only very slowly acted on.

Palladium Salts.-The nitrate, chloride, and protoxide give the dioxide by the action of ozone. The protoxide, in presence of potassium hydroxide, gives potassium palladate.

Cobalt and Nickel Salts.-The sulphates, nitrates, and chlorides are but slowly attacked. The protoxides, on the other hand, are easily converted into peroxides.

Lead Salts.-All the basic salts give lead peroxide, as do many of the neutral salts; the chloride, nitrate, oxalate, and phosphate, however, are but very slowly acted on. Lead oxide is also changed into peroxide by ozone; in presence of potassium hydroxide, it gives potassium plumbate.

Manganese Salts.-All the manganese salts, in moderately concentrated solution, give a brown or black precipitate, consisting of the hydrated dioxide if the ozone is in excess, and of a lower oxide if it is not. In the former case a violet solution, containing permaganic acid, is frequently produced. If excess of ozone acts on a very dilute solution of a manganous salt (in 30,000 to 60,000 of water), a brown dicroic solution is obtained, which slowly decomposes after a time, depositing a rusty brown precipitate, and leaving permaganic acid in solution.

Chromic Salts.-The sulphate, chloride, and oxide all yield chromic acid. If ether is present, perchromic acid is formed.

Bismuth oxide gives bismuthic acid, and in presence of potassium hydroxide potassium bismuthate.

Iron sesquinoxide is not acted on by ozone, but in presence of potassium hydroxide it yields potassium ferrate.-Amer. Jour. Phar., Dec. 1882, 617-618, from Compt. Rem., 94, 850-863, through Jour. Chem. Soc., Nov. 1882.

HYDROGEN.

Water-Test Solution for Hardness.-Mr. C. R. C. Tichborne ob

serves that the process for determining the hardness of water, originally invented by Dr. Clarke, nearly half a century ago, has never been improved upon, and that there seems at the present time no necessity for a change. He, however, proposes a modification in respect to the soap solution, which consists in preparing it from oleic acid, and standardizing it to the amount of volumetric soda solution required to neutralize the fatty acid. The following is the process:

5 cc. of oleic acid are measured with a pipette, and 50 cc. spirit added to it in a beaker; 2 drops of phenol-phtalein solution are also added, and

immediately a volumetric solution of soda (NHO) is run in until a pink

1000

indication is produced. This must be done accurately, as the success of the process depends upon this measurement. The oleate of soda is then made up to the required measure, i. e., 820 cc. for 15.5 cc. of soda solution used by the addition of a mixture of equal parts of rectified spirit and distilled water. Such a solution makes a lather exactly on the original scale of Clarke; and, although different oleic acids might differ in purity, such a condition of things introduces no error, as the volumetric soap solution is made up in the saturating power of the acid employed, which alone determines the strength. In the author's experience 15.5 cc. of soda solution neutralized 5 cc. of oleic acid, both of known purity and from the candle manufacturers.

The above process gives a solution, 32 cc. of which when operating on 100 cc. of water, represent 16° of hardness per gallon by Clarke's scale.-Yearbook of Pharm., 1882, 424-427.

Water-Formation of a Definite Compound with Carbonic Acid, which see under "Carbon."

Hydrogen Peroxide-Action on Organic Matter.-MM. Paul Bert and P. Regnard have studied the action of hydrogen peroxide upon various forms of organic matter and upon fermentations, and find that it possesses very remarkable antiseptic properties. The results of their investigations may be summed up as follows:

1. Hydrogen peroxide, even when very dilute, arrests fermentations due to the development of living organisms, and the putrefaction of all substances which do not decompose it.

2. It has no effect upon diastase fermentations.

3. Dilute hydrogen peroxide is not destroyed by fats, starches, soluble ferments, egg albumen, casein, the peptones, creatine, creatinine or urea. 4. It is rapidly destroyed by nitrogenous collagens, by musculin, fibrin of the blood, and various nitrogenous vegetable matters.

5. This action is definitely arrested by a temperature above 70°. Putrefaction, however, leaves it entirely intact.

As it appeared from the powerful antiseptic properties of hydrogen peroxide that it might prove of value in surgery, experiments were made

upon the point by MM. Péan and Baldy at the hospital of St. Louis, with very successful results. The hydrogen peroxide, in solutions containing from two to six times its volume of oxygen, according to the circumstances of the case, was used, both externally, as a dressing for wounds, ulcers, etc., and also given internally in certain affections, in doses of from three to five grains, containing six times its volume of oyxgen. M. Bert draws attention to the fact that hydrogen peroxide for surgical use must be entirely neutral.-Amer. Jour. Phar., Jan. 1883, 21-22, from Compt. Rend. 94, 1383, and 95, 49, through Amer. Chem. Jour.

Oxygenated Water-Antiseptic Action.-Dr. Péan has made experiments on the antiseptic action of oxygenated water. Water containing from two to twelve times its volume of oxygen was used as a dressing after major operations, such as amputation of the arm, leg and thigh, etc., a spray of the same liquid being also played on the wound during the operation. Under the influence of these applications, the wound showed a favorable tendency to unite by first intention; and in the case of chronic ulcers, cicatrization was observed to be effected more rapidly than with any other dressing. Salutary results were also obtained when oxygenated water was given internally to patients who had been treated by other means, and who were threatened with septicemia.--New Rem., Oct. 1883, 310, from Med. Press.

Sulphuretted Hydrogen-Improved Apparatus.-Mr. Clemens Winkler describes an apparatus which he considers to be the best and most serviceable in use. A leaden cylinder, securely fastened in a wooden frame, is intended for the reception of the acid, and it is provided, for this purpose, with a tubulure; its lower end has a conical shape, and terminates in a pipe, which is connected by means of a rubber tube and suitable pipes with a cistern, located underground, or in some other convenient place, and intended to receive the saturated solution. Within the cylinder, another narrower leaden cylinder, may be raised or lowered by means of a winch and pulley. This cylinder is filled to near the top with sulphide of iron. It fits snugly to the outer cylinder, and is arrested from complete descent in the latter by means of a collar. At its upper end it is provided with a lateral tubulure and stop-cock, which is connected with two wash-bottles, the first of which is intended for washing the gas, and the second for affording a constant supply of hydrosulphuric acid water, which may be drawn off from a faucet at the bottom. The top of the cylinder is closed by a round disk of thick rubber, and over this by a flat disk of iron securely clamped on, making a perfectly tight gas joint. The stirrup carrying the inner cylinder runs in grooves situated in the uprights, and is, therefore, raised and lowered with perfect ease, and without warping the joints. When it is desired to generate gas, the inner cylinder is lowered into the acid, and the generation ceases by again raising it.-New Rem., Oct. 1882, 295, from Zeitsch. f. Anal. Chem., 1882, 386.