Page:Experimental researches in chemistry and.djvu/98

1893] but I have endeavoured since to do so by means of cooling mixtures. The hydrate in thin plates was put into solutions of muriate of lime of different densities, but of the temperature of 32° Fahr. It seemed to remain in any part of a solution of specific gravity 1.2, but there was constantly a slight liberation of gas; and as minute and imperceptible bubbles may have adhered to the hydrate, the result can only be considered as a loose approximation. The solid crystals would probably be heavier than 1.2.

The hydrate of chlorine acts upon substances, as might be expected, from the action of chlorine upon the same substances, and it may perhaps now and then offer a convenient form for its application in experiment. When put into alcohol, an elevation of temperature amounting to 8° or 10° took place. There was rapid action, much ether, and muriatic acid formed, and a small portion of a triple compound of chlorine, carbon and hydrogen.

When put into solutions of ammonia cal salts it liberated nitrogen gas, formed muriatic acid, and also chloride of nitrogen, which remained undissolved at the bottom of the solution.

In aqueous solution of ammonia similar effects were produced, but less chloride of nitrogen was formed.

In order to arrive at a knowledge of the composition of this substance, I adopted the following process:—The crystals were collected together by a small quantity of solution of chlorine, then filtered and pressed between successive portions of bibulous paper at a temperature of 32° (care being taken to expose them as little as possible to the air), until as dry as they could be rendered by this means. A glass flask with a narrow neck, and containing a portion of water at 32°, having been previously counterpoised, a portion of the crystals were immediately after the last pressing introduced into it; they sank to the bottom of the water, and the flask being again weighed, the quantity of crystals introduced was ascertained. A weak solution of pure ammonia was then poured into the water in the flask, care being taken to add considerable excess over that required by the chlorine beneath. The whole was left for twenty-four hours, in which time the chlorine had had sufficient opportunity to act on the ammonia, and any portion of chloride of nitrogen that might at first have been formed would be resolved into its elements, and its chlorine be