Publisher's Synopsis
This historic book may have numerous typos and missing text. Purchasers can usually download a free scanned copy of the original book (without typos) from the publisher. Not indexed. Not illustrated. 1849 edition. Excerpt: ... color; the neutral succinate of ammonia is then added, upon which succinate of peroxide of iron of a brown color is precipitated; it is filtered when quite cold, and washed first with cold water, and, finally, with a warm solution of ammonia, in order to remove a portion of the succinic acid: it is then dried and ignited in a current of air, in order thoroughly to peroxidize the iron. The sesquioxide of iron is--Two equivalents of Fe... 56... 70 Three do. of 0... 24... 30 One do. of Fe203... 80....100 Separation of Peroxide of Iron from Protoxide of Iron.--This is attended with very great difficulties, and can only be accomplished when the compound is soluble in acids. When no other base but iron is present, as, for example, in native magnetic iron ore, Rose directs that a weighed quantity of the substance should be dissolved in hydrochloric acid, and, having boiled with nitric acid to peroxidize the whole of the iron, it is to be precipitated by ammonia; the increase of weight is owing to the acquisition of oxygen, which has combined with the protoxide of the compound, and is half as much in quantity as the oxygen previously existing in the protoxide, for the protoxide of iron, on being fully converted into peroxide, acquires one-half more oxygen than it already possessed. 2 (FeO) + 0 = Fe30s. Thus, then, finding first the quantity of oxygen gained by the substance operated on, we find next the quantity of oxygen belonging to the protoxide existing in the compound, and from this it is easy to calculate the quantity of the protoxide. When this is found, the quantity of peroxide contained in the substance is learned from the difference in weight between the quantity of the compound submitted to analysis and the quantity of protoxide made...
