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            "2073": {
                "pageid": 2073,
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                "title": "Reaction vessel",
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                        "*": "{{Stub}}\nA '''reaction vessel''' is a type of glass lab item used to perform chemical reactions under controlled conditions.\n\nLarge scale reaction vessels are called '''reactors''', and are ubiquitous in chemical industry.\n\n==General==\nReaction vessels consist of cylindrical walled flask with round or pear-shaped bottom, with a glass cover containing 3, 4, 5 or more female [[ground glass joint]]s of equal size, while other types have a large diameter central joint and 2, 3 or more smaller joints. They are typically made of borosilicate glass Unlike typical lab round bottom flasks, reaction vessels are thick walled, allowing them to be used in high vacuum or high pressure processes. The cover is held to the main body using a special metal clamp and a large [[polytetrafluoroethylene|PTFE]] ring is used as seal. Complex types of reaction vessels come with an outer jacket, where a working fluid maintains a desired temperature in the reaction flask. Other types have a stopcock on the bottom of the flask, to drain the reaction flask.\n\nSpecial reaction vessels come with a digital controller, which allows you to adjust temperature, stirring, pressure, time, etc.\n\n[[Schlenk flask]]s are sometimes called reaction vessels, though their use is different from that of chemical reactors.\n\n==Availability==\nReaction vessels can be bought online from lab suppliers. They are not cheap.\n\n==Projects==\n*Synthesis of chemical compounds under pressure\n*Synthesis of bulk amounts of compounds\n*Photochemical reactions\n\n==See also==\n*[[Round-bottom flask]]\n*[[Schlenk flask]]\n\n==References==\n<references/>\n===Relevant Sciencemadness threads===\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=72789 50l Chemglass reaction vessel with motorized overhead stirrer - Any interest?]\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=8747 Reaction vessel from a computer cathode tube.....]\n\n[[Category:Glassware]]\n[[Category:Lab equipment]]"
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                "title": "Reactivation of calcinated oxides",
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                        "*": "{{Stub}}\nMost oxides sold in hardware stores as pigments tend to be calcinated at high temperatures, which changes their crystalline structure and makes them resistant to the attack of most corrosive reagents, like acids, aqueous alkali, metal halides or halogens. Indurated oxides can be '''reactivated''' by fusing them with molten alkali or [[sodium bisulfate]], though this too may not always work.\n\nNote that some oxides, like [[titanium dioxide]] and [[zirconium dioxide]] are normally (almost) inert without calcination.\n\n==Successful methods==\n===Fusion with molten alkali===\nMixing the inert oxide with an alkali hydroxide, like [[sodium hydroxide]], [[potassium hydroxide]] and melting the resulting mixture for a few hours will break down the oxide's inert structure and make it more reactive. May not work with all oxides, such as [[calcium oxide]] or [[magnesium oxide|magnesia]]. Reaction with [[chromium(III) oxide]] can give chromate or dichromate, while with [[iron(III) oxide]] will give ferrate.\n\n===Fusion with molten sodium bisulfate===\nMolten [[sodium bisulfate]] (NaHSO<sub>4</sub>) has been claimed to react with calcinated oxides.\n\n===Dissolution in hydrofluoric acid===\n[[Hydrofluoric acid]] is the only acid that can attack any metal oxide, however since many fluorides are almost insoluble in water, dissolving large amounts of inert oxide will take forever. And since working with hydrofluoric acid is very dangerous, this route is both expensive and extremely hazardous.\n\n===Dissolution in hot concentrated sulfuric acid===\nSome metal oxides like titanium dioxide will react with hot conc. sulfuric acid, forming TiOSO<sub>4</sub>, which hydrolyzes in the presence of water, giving raw titanium dioxide. If the TiOSO<sub>4</sub> is kept in sulfuric acid, and [[hydrogen peroxide]] is added, an orange colored peroxo titanium oxide compound is obtained.\n\n===Reduction to metal===\nUsing a reducing metal, like [[aluminium]] or [[magnesium]] or a non-metal, like [[carbon]] into a thermite reaction to obtain the metal from the oxide is another accessible route. To obtain the oxide again, dissolve the metal in an acid, precipitate it with aq. ammonia then heat the product until it decomposes. While attractive, this method will consume plenty of useful aluminium or magnesium powders that would be of better use elsewhere. The thermite reaction also produces plenty of slag, which may be inert.\n\n==Failed methods==\n===Calcination with ammonium chloride===\nHeating the oxide with [[ammonium chloride]] gave no results.\n\n===Fusion with alkali nitrates===\nMelting together a calcinated metal oxide, like chromium(III) oxide with molten [[potassium nitrate]] will give a brownish product, insoluble in water, without any visible reactivity.\n\n==Safety==\nWorking with molten alkali and salts is very dangerous and proper protection equipment should be worn all the times.\n\n==References==\n<references/>\n===Relevant Sciencemadness threads===\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=25744 Chromium (III) from Cr2O3]\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=27545 Failed attempt at dissolving zinc oxide in alkaline solutions]\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=21663 Very low solubility of erbium oxide in mineral acids]\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=12220 NiO > NiCH3COO]\n*[http://www.sciencemadness.org/talk/viewthread.php?tid=13856 Cerium (III) Oxide]\n\n[[Category:How-to]]"
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