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Image from page 46 of “An introduction to practical chemistry : including analysis” (1856)
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Identifier: 101501916.nlm.nih.gov
Title: An introduction to practical chemistry : including analysis
Year: 1856 (1850s)
Authors: Bowman, John E. (John Eddowes), 1819-1854
Subjects: Chemistry Chemical Phenomena
Publisher: Philadelphia : Blanchard and Lea
Contributing Library: U.S. National Library of Medicine
Digitizing Sponsor: Open Knowledge Commons, U.S. National Library of Medicine

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Text Appearing Before Image:
II.Preparation of Ammoniacal Gas (NH^.a 55. This gas may be prepared in a similar manner tothe last; but as it is specifically lighter than commonair, the bottles in which it is collected must be kept,while filling, with the mouth downwards, the deliver-ing tube passing upwards, to the top (Fig. 1G); theneck of the retort should be furnished as before with aroll of filtering paper. 56. Reduce 300 grains of quick lime (CaO) to powderin a mortar, and slake it in a small basin with a drachm • Water at common temperatures is capable of dissolving no less than480 times its own volume of hydrochloric acid. The liquid hydro-chloric or muriatic acid of commerce is a solution of the °-as in water 2 The specific gravity of ammoniacal gas is 0-589, 100 cubic inchesweighing 18-288 grains. Its atomic weight is 17, and its atomicvolume 2. PI! EPA II A XI ON OF AM M OX I AC A L GAS. 19 and a half of water ; then pound 400 grains of muriateof ammonia (KH4C1); mix the powders as quickly as rig. 16.

Text Appearing After Image:
Fig. 17 Preparation of Ammoniacal Gas. possible, and without loss of time transfer the mixtureto the retort. The following decomposition takes place:— XH4Cl+CaO=CaCl+/fO+NH3. If the gas does not come over rapidly, a gentle heatmay be applied. When three or four bottles have beenfilled, proceed with the following ex-periments :— 57. Observe the effect of the gas on alighted taper: it extinguishes the flame,and at the same time shows a slighttendency to burn with a pale greenflame. 58. Remove the stopper from one ofthe bottles, and close the mouth with adry glass plate (read paragraph 52); theninvert it, and having placed it underwater, remove the glass plate and ob-serve the rapid absorption. That whichremains unabsorbed is atmospheric air.1 59. Test the liquid obtained in thelast experiment (which is a weak solu-tion of ammonia) with turmeric and rcd- 1 Water at common temperatures is capable of absorbing nearly 700times its volume of ammoniacal gas.

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