Chemical Gazette, 1846
Or Journal of Practical Chemistry, Vol. 4
by Unknown Author
The following computer-generated description may contain errors and does not represent the quality of the book:
Scientific and Medicinal Chemistry. basic compounds, the alkaline bicarbonates produce, immediately if they are added in excess, in the nitrate and sulphate similar red-brown precipitates as the solutions of the neutral carbonates; but in the solution of the perchloride of mercury they merely give rise to a faint whitish opacity; only after some time is a greater or less amount of a reddish-brown precipitate of a basic salt formed in proportion as the carbonic acid escapes. Carbonate of lime and baryta behave like the bicarbonates; both immediately precipitate reddishbrown precipitates from the solution of the pernitrate of mercury; but from the persulphate dissolved in sulphuric acid, mineral turpeth, which becomes brownish-red by long standing, especially when heated with carbonate of baryta. On the contrary, carbonate of lime or baryta produce no precipitate in a solution of the perchloride of mercury, or at the utmost only a slight reddish-brovn tint is formed on boiling at the margin of the vessel. Perchloride of mercury is not altered, either in the cold or on boiling, by a solution of pi-otosulphate of iron; while irom the solution of the nitrate or sulphate the whole of the mercury is eliminated, even in the cold, by the protosulphate of iron. The solution of the perchloride of mercury contains consequently no muriate of the oxide which would be reduced by the protosulphate of iron. The greater affinity of the mercury for chlorine than for oxygen is moreover evident from the circumstance that nitric acid, and even sulphuric acid, do not decompose the perchloride of mercury, and convert it into an oxysalt, either v.ith or without the application of heat. The protosalts of mercury cannot be compared with the protochloride, on account of the insolubility of the latter; but that the mercury is likewise, in this case, combined more intimately with the chlorine than in the salts with oxygen and acids, is evident from the fact that the protosulphate of iron does not decompose the moist protochloride of mercury, Avhile the mercury is instantly precipitated in a metallic state from a solution of the protoniti-ate by a solution of the protosulphate of iron. On this account a solution of protochloride of iroi likewise produces in protonitrate of mercury a precipitate of protochloride, which is not decomposed by any excess of the protochloride of iron. In like manner the protochloride of mercury is not decomposed by carbonate of baryta or lime, or the bicarbonates of the fixed alkalies, while these readily decompose solutions of the protonitrate of mercury. The chloride and the oxysalts of silver exhibit a very similar behaviour. Recently precipitated moist chloride of silver is not decomposed by protosulphate of iron; while, as is well knoAvn, the whole amount of silver can be precipitated from the solution of the nitrate by that salt. When a solution of nitrate of silver is mixed with one of protochloride of iron, only chloride of silver separates, and no metallic silver. Again, solutions of the alkaline carbonates do not decompose the chloride of silver in the cold, and only to a very slight extent on the application of heat. A solution of caustic potash likewise effects a decomposition of the chloride of silver only when heated.
APA: (2013). Chemical Gazette, 1846: Or Journal of Practical Chemistry (Vol. 4). London: Forgotten Books. (Original work published 1846)
MLA: Chemical Gazette, 1846: Or Journal of Practical Chemistry. Vol. 4. 1846. Reprint. London: Forgotten Books, 2013. Print.