Balance The Equation Al2O3 + 2 Naoh ↠ H2O + 2 Naalo2 +H2O

If aluminum is coated with a passive layer (AlO3) and it reacts with NaOH solution the oxide layer is dissolved, but what is the reaction and what happens to aluminum superficie? Oxide layer remains or any aluminum hydrate is formed. I need to prepare the surface for zincating process.

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however, as the alkaline etching medium is generally aqueous, the first reaction will again form an hydroxyde or eventually oxide layer after drying again. In order to prevent this you will need to work water-free due to the high oxophilicity of aluminum.

Đang xem: Al2o3 + 2 naoh → h2o + 2 naalo2

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It depends on the solution that have been used after the immersion in NaOH solution. Normally, a smut layer will be formed resulting from the reaction of NaOH and Al. Some researchers used HNO3 to remove this layer. At this stage, aluminum hydroxide will be deposited on the Al surface but it converts to aluminum oxide (Al2O3) during the drying process.

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I had read something like that, but literarura always refers to the passive layer (aluminum oxide) but not aluminum hydroxide due to it is formed only in aqueous solutions.
however, as the alkaline etching medium is generally aqueous, the first reaction will again form an hydroxyde or eventually oxide layer after drying again. In order to prevent this you will need to work water-free due to the high oxophilicity of aluminum.
I recommend publication: Su-Il Pyun, Sung-Mo Moon, Corrosion mechanism of pure aluminium in aqueous alkaline solution, J. Solid State Electrochem (2004) 4: 267-272.
Aluminum reacts with sodium hydroxide to form a salt called sodium aluminate(NaAlO2) and hydrogen gas. Aluminum is an interesting alternative to generate high purity hydrogen. Generally, a metal reacts with an acid, it forms salt and hydrogen gas. This case aluminium acts as an amphoteric metal which basically means that it has both acidic and basic properties.
This reaction only occurs in the presence of NaOH and KOH, which behave as catalysts. The reaction rate with sodium hydroxide (NaOH) is strongly affected by temperature and the concentration of alkali, which acts as catalyst. The speed of aluminum consumption might be easily controlled by connecting such a system to a fuel cell or another device able to burn hydrogen to generate energy, especially for portable and medium scale electric devices.
The main advantages of using aluminum for indirect energy storage are: recyclability, non-toxicity and easiness to shape. Alkali concentrations varying from 1 to 3 mol.L-1 can be applied to different metallic samples, either foil (0.02 mm thick) or plates (0.5 and 1 mm thick) form, and reaction temperatures between 295 and 345 K are suggested.
Different temperatures can take for different thicknesses of metallic plates due to the very long reaction time for thicker samples at room temperature (295 and 305 K). This drawback caused some difficulties in the evaluation of the reaction rates, so a higher temperature can be chosen for the 1-mm thick aluminum plates to avoid this problem.
The aluminum samples should completely consumed in the reaction experiments. Nonetheless, it is possible to view the change in the color of the samples as the reaction proceeds. This color becomes a dark gray as the metal is consumed, and the thickness slowly decreases.
**Time reaction rate may depend upon the thickness, temperature, type of alkali and concentrations. If thickness is less, concentration is less, it can consume high time for consumption of aluminum during reaction, while thickness is long and concentration is high it can take less time. This may indicate that the mechanism of catalysis is slightly different for each alkali. For 0.5 mm thick plates with concentration 2.5 mol/litre can predict time of 950 minutes, while for 1 mm thickness with concentration of 3.0 mol/litre can take only 335 minutes(This is a one of the study data from another researchers). Generally, chemical reaction has a tendency to proceed more quickly in the presence of NaOH.
Aluminum reacts with sodium hydroxide to form a salt called sodium aluminate(NaAlO2) and hydrogen gas. Aluminum is an interesting alternative to generate high purity hydrogen. Generally, a metal reacts with an acid, it forms salt and hydrogen gas. This case aluminium acts as an amphoteric metal which basically means that it has both acidic and basic properties.
This reaction only occurs in the presence of NaOH and KOH, which behave as catalysts. The reaction rate with sodium hydroxide (NaOH) is strongly affected by temperature and the concentration of alkali, which acts as catalyst. The speed of aluminum consumption might be easily controlled by connecting such a system to a fuel cell or another device able to burn hydrogen to generate energy, especially for portable and medium scale electric devices.
The main advantages of using aluminum for indirect energy storage are: recyclability, non-toxicity and easiness to shape. Alkali concentrations varying from 1 to 3 mol.L-1 can be applied to different metallic samples, either foil (0.02 mm thick) or plates (0.5 and 1 mm thick) form, and reaction temperatures between 295 and 345 K are suggested.

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Different temperatures can take for different thicknesses of metallic plates due to the very long reaction time for thicker samples at room temperature (295 and 305 K). This drawback caused some difficulties in the evaluation of the reaction rates, so a higher temperature can be chosen for the 1-mm thick aluminum plates to avoid this problem.
The aluminum samples were completely consumed in all the experiments. Nonetheless, it is possible to view the change in the color of the samples as the reaction proceeds. This color becomes a dark gray as the metal is consumed, and the thickness decreases.
**Time reaction rate may depend upon the thickness, temperature, type of alkali and concentrations. If thickness is less, concentration is less, it can consume high time for consumption of aluminum during reaction, while thickness is long and concentration is high it can take less time. This may indicate that the mechanism of catalysis is slightly different for each alkali. For 0.5 mm thick plates with concentration 2.5 mol/litre can predict time of 950 minutes, while for 1 mm thickness with concentration of 3.0 mol/litre can take only 335 minutes. Generally, chemical reaction has a tendency to proceed more quickly in the presence of NaOH.
Aluminum oxide reacts with sodium hydroxide to produce sodium aluminate and water. This reaction takes place at a temperature of 900-1100°C. A salt and water is obtained in this reaction in which aluminium oxide acts as an acid. Since, Aluminum oxide is amphoteric in nature; it can react with a strong acid9just example HCl may be best) instead of a strong base too.
Crystalline Al2O3 at room temperature is hardly soluble in any solvent, even concentrated acid or alkali, for kinetic reasons. Al2O3 only reacts with as strong solvent as melted NaOH.
Now see the list of another action of aluminum oxide with sodium hydroxide and water, one for metallurgy and another for just chemical reaction(in both case product is tetrahydroxoaluminate)
(Aluminum oxide, sodium hydroxide and water) without a particular temperature or concentration consideration.
*Hot concentrated sodium hydroxide solution, aluminium oxide reacts to give a solution of sodium tetrahydroxoaluminate, for a general chemical reaction,
This is detailed information regarding the dissolution of Al. Please send the link of the article which reported: ” For 0.5 mm thick plates with concentration 2.5 mol/litre can predict time of 950 minutes, while for 1 mm thickness with concentration of 3.0 mol/litre can take only 335 minutes “.
I am preparing a mesoporous mix of Al2O3(8%wt.) and Fe2O3. To remove Si ( used as template in the synthesis) I use NaOH (2M) but I am concerned about removing Al2O3 in this step.
I know it is practically insoluble in water, so which solvents can be used to dissolve aluminium oxide?
I have a solid residue which is supposed to be mainly composed by alumina. My goal is to dissolve it or at least weaken it. I have tried concentrated inorganic acids such as HF and HCl, organic acids such as glycolic and citric, bases such as NaOH, Na2CO3… All at 60-90ºC. Nothing seems to attack it. I appreciate any advice or recommendation
How can i prepare 60% of NaoH solution? In a article (I J Scientific and Engineering Research, Volume 6(5) May 2015) they prepared only 60% NaoH but they didn't mention the volume of the solution. So i need some suggestions.
I will be etching Al6063 and Cu101 to remove the oxide layer. I will use nitric acid HNO3 or NaOH solution. Is either solution better for a bath containing Al and Cu plates?
Is Al oxide and Cu oxide soluble in these solutions? Does the oxide layer dissolve, or does the solution only break the bond, still leaving oxide particles suspended in the solution?
If the Al and Cu plates are allowed to dry with the solution on the surface, and then exposed to a vacuum, would the dried solution continue to etch the surface in the vacuum or is the etching action halted while in a vacuum?
I have collect a cyclic voltammetric data by taking Ag/AgCl as the reference electrode. But I want to convert this one to Potential with respect to Reversible Hydrogen Electrode. Please suggest me the required conversion equation. 0.5M H2SO4 was taken as the supporting electrolyte.

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