Essentials of medical and clinical chemistryWith laboratory exercises . Hydrogen ChloriteâChlorous +H20=2HCI03âHydrogen ChlorateâChloric ,+H20=2HC104âHydrogen PerchlorateâPerchloric acid. The Hydracids of the chlorine group are as follows :â H + F = IIFâHydrogen FluorideâHydrofluoric acid. H + CI = HClâHydrogen ChlorideâHydrochloric (muriatic) acid. H + Br = HBrâHydrogen BromideâHydrobromic acid. H + I = HIâHydrogen IodideâHydriodic acid. Prepared by treating the appropriate salt with H2SO4, thus :â CaF, +H2SOi = CaSOj + + H2SO4 = NajSO, + 2Ha.«2KBr -I- HjSOi = K2
Essentials of medical and clinical chemistryWith laboratory exercises . Hydrogen ChloriteâChlorous +H20=2HCI03âHydrogen ChlorateâChloric ,+H20=2HC104âHydrogen PerchlorateâPerchloric acid. The Hydracids of the chlorine group are as follows :â H + F = IIFâHydrogen FluorideâHydrofluoric acid. H + CI = HClâHydrogen ChlorideâHydrochloric (muriatic) acid. H + Br = HBrâHydrogen BromideâHydrobromic acid. H + I = HIâHydrogen IodideâHydriodic acid. Prepared by treating the appropriate salt with H2SO4, thus :â CaF, +H2SOi = CaSOj + + H2SO4 = NajSO, + 2Ha.«2KBr -I- HjSOi = K2SO4 -f +H2S04 = KjS04 +2HI. * To prepare hydrochloric acid gas, put several ounces of common salt and4 42 ESSENTIALS OF CHEMISTRY. Physical Properties.â\ox\ts&, irritating gases; sharp, sourtaste; very soluble, water dissolving several hundred times itsown volume, forming aqucB known by the simple name of the aciditself, thus : The officinal hydrochloric acid is a solution of thehydrochloric acid gas in water. Fig. Chemical Properties.âStrong acids; true acids even withoutwater. Uses.âHF attacks silica energetically, hence is used to etchglass ; very poisonous, and burns made by it heal with difficulty. about twice as much sulphuric acid into a flask, and warm. The gas comes offin abundance and may be collected in a dry bottle (like chlorine, Fig. 16), orover mercury. The solution of the gas (the ordinary form) is obtained bypassing the gas through a series of Wolff bottles containing cold water andarranged as shown in Fig. 17. For making HBr or III, phosphoric acid isbetter, since sulphuric is apt to be partially reduced with evolution of SO2. Fill a large dry glass tube with HCl gas and quickly invert it in a dish ofwater colored blue with litmus. Note that the gas is instantly dissolved andthat the water rushes up to take its place and the litmus is reddened bythe acid. Let some of the gas pour into the mouth and note sour taste. PART I.
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