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Aluminium oxide is an amphoteric substance, meaning it can react with both acids and bases, such as hydrofluoric acid and sodium hydroxide, acting as an acid with a base and a base with an acid, neutralising the other and producing a salt. Al 2 O 3 + 6 HF → 2 AlF 3 + 3 H 2 O Al 2 O 3 + 2 NaOH + 3 H 2 O → 2 NaAl(OH) 4 (sodium aluminate)
The Bayer process is the principal industrial means of refining bauxite to produce alumina (aluminium oxide) and was developed by Carl Josef Bayer.Bauxite, the most important ore of aluminium, contains only 30–60% aluminium oxide (Al 2 O 3), the rest being a mixture of silica, various iron oxides, and titanium dioxide. [1]
Virtually all the aluminium hydroxide used commercially is manufactured by the Bayer process [10] which involves dissolving bauxite in sodium hydroxide at temperatures up to 270 °C (518 °F). The waste solid, bauxite tailings , is removed and aluminium hydroxide is precipitated from the remaining solution of sodium aluminate .
The aluminium oxides, oxide hydroxides, and hydroxides can be summarized as follows: aluminium oxides. corundum (Al 2 O 3); aluminium oxide hydroxides diaspore (α-AlO(OH)) ...
Sodium aluminate is an inorganic chemical that is used as an effective source of aluminium hydroxide for many industrial and technical applications. Pure sodium aluminate is a white crystalline solid having a formula variously given as NaAlO 2, NaAl(OH) 4 (), [3] Na 2 O·Al 2 O 3, or Na 2 Al 2 O 4.
As per researches conducted by V.K.Chhabra, Chief Chemist (retd.) P.H.E.D. Rajasthan, activated alumina, when used as a fluoride filter, under field conditions can best be regenerated by a solution of lye (sodium hydroxide; NaOH), sulfuric acid (H 2 SO 4). The fluoride uptake capacity (FUC) of commercial activated alumina can be up to 700 mg/kg.
In hot concentrated hydrochloric acid, aluminium reacts with water with evolution of hydrogen, and in aqueous sodium hydroxide or potassium hydroxide at room temperature to form aluminates—protective passivation under these conditions is negligible. [9] The reaction with aqueous alkali is often written: [2] Al + NaOH + H 2 O → NaAlO 2 ...
In chemistry, ammonolysis (/am·mo·nol·y·sis/) is the process of splitting ammonia into + +. [1] Ammonolysis reactions can be conducted with organic compounds to produce amines (molecules containing a nitrogen atom with a lone pair, :N), [2] or with inorganic compounds to produce nitrides.