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Updated: May 15, 2025
In Rural Economy there are Abstracts from papers of considerable value and extent on Pasturages, Chlorides applied to diseased Animals, Quality of Waste Land from the plants growing in it, Malt Duties, Beet Root Sugar, Aliment from Straw, Planting and Pruning, Indian Corn, Mangold Wurzol, &c. In Gardening are upwards of 40 similar Abstracts.
Let it be assumed that the weight of the mixed chlorides is 0.15 gram, and that it contains 53 per cent of chlorine. The simplest solution of such a problem is reached through algebraic methods. The weight of chlorine is evidently 0.15 x 0.53, or 0.0795 gram. Let x represent the weight of sodium chloride present and y that of potassium chloride.
Wash the filter five times with hot water, add to the filtrate ammonium hydroxide and bromine water as described above, and repeat the precipitation. Collect the precipitate on the filter already used, wash it free from chlorides with hot water, and ignite and weigh as described for ferric hydroxide on page 110. Calculate the percentage of the combined oxides in the limestone.
The electrolytic decomposition of the chlorides has not yet been successfully accomplished, so that prior to the operation it is necessary to convert them into sulphates.
The second is that since the envelope of the supposed spheroid would consist of the gases and non-metallic elements, compounds of these with the metals and with one another would continually accumulate on the molten shell; and the crust, consisting of oxides, chlorides, sulphurets, and the rest, having much less specific gravity than the molten shell, would be readily supported by it.
For some years I have tested the applicability of artificial precipitates to close the holes in boilers, cylinder-covers, and stuffing boxes. I took, generally with the best success, alternate layers of hemp-cotton, thread, and absorbent paper, all well saturated with the chlorides of calcium and magnesium. The next layers of the same fiber are moistened with silicate of soda.
Each part of the chlorides requires three parts by weight of the silver citrate to throw down the chlorine, thus: 3NaCl + Ag C H O = Na3.C H O +3AgCl. The silver chloride formed a dense insoluble precipitate, and the supernatant fluid was decanted and filtered through a rubber tube and handed round as a beverage. with less than half a grain of undecomposed chlorides.
While it is likely that some of the chlorine was due to the presence of chlorides other than common salt, as the position of the point of observation is not removed more than a mile from oil distilleries and smelting and sulphuric acid works in New Jersey, yet this could not even generally have been so, as the rain storms came, for the greater number of instances, from the east, in an opposite direction to the position of the factories alluded to.
It should be noted that, in general, the changes occurring at the cathode are reductions, while those at the anode are oxidations. For analytical purposes, solutions of nitrates or sulphates of the metals are preferable to those of the chlorides, since liberated chlorine attacks the electrodes.
The salts are sulfates, phosphates and chlorides of sodium, potassium, calcium and magnesium. The organic and inorganic matter varies with the ration. The quantity of urine secreted within a given time varies in the different species and at different times in the same individual.
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