DIY History | Transcribe | Scholarship at Iowa | The Analytical Separation of Iron and Aluminium by Henry Erdmann Radasch, 1897 | The Analytical Separation of Iron and Aluminium by Henry Erdmann Radasch, 1897, Page 33

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The Analytical Separation of Iron and Aluminium by Henry Erdmann Radasch, 1897

The Analytical Separation of Iron and Aluminium by Henry Erdmann Radasch, 1897, Page 33

[page]31[/page]

first transferred to the filter it was dark red, as the zinc salt should be. By the time that the washing with alcohol was completed the precipitate had changed to a dark green throughout. The wash water and alcohol were both tested for alkalies but none found. The zinc chloride solution gave no reaction for iron, sodium or ammonia. The precipitate was tested for manganese but none was found. It was tested for iron, by igniting a little upon a platinum foil to redness, but the residue was yellow while hot -- and white -- [??] in color. An iron would have given this residue, of zinc oxide, a tinge of red. Subsequent analysis of the salt (the determination of the zincs) showed the percentage of zinc to be a great deal higher than that of the normal zinc salt. The percentages were only approximate as the determination was made by direct ignition of the organic salt. Some of the zinc was no doubt lost by [?solatilisation?]. Several lots of this zinc nitross-[?beta?]-naphthol had been prepared before this and all were deep red. Another lot was prepared

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[page]31[/page] first transferred to the filter it was dark red, as the zinc salt should be. By the time that the washing with alcohol was completed the precipitate had changed to a dark green throughout. The wash water and alcohol were both tested for alkalies but none found. The zinc chloride solution gave no reaction for iron, sodium or ammonia. The precipitate was tested for manganese but none was found. It was tested for iron, by igniting a little upon a platinum foil to redness, but the residue was yellow while hot -- and white -- [??] in color. An iron would have given this residue, of zinc oxide, a tinge of red. Subsequent analysis of the salt (the determination of the zincs) showed the percentage of zinc to be a great deal higher than that of the normal zinc salt. The percentages were only approximate as the determination was made by direct ignition of the organic salt. Some of the zinc was no doubt lost by [?solatilisation?]. Several lots of this zinc nitross-[?beta?]-naphthol had been prepared before this and all were deep red. Another lot was prepared