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Reaction of aluminum hydroxide and nitric acid
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Kieren Reeves
Reaction of aluminum hydroxide and nitric acid
Aluminum oxide could be the product of fusing Al(NO3)3 at high enough temperature. Aluminum metal would not be a product, in water or in fused salt.
2.Aluminum metal does not readily dissolve in nitric acid because of formation of passive oxide/hydroxide film. The nuclear power industry had need of large amounts of aluminum nitrate, and it was made by dissolving aluminum metal in hydrochloric acid (very fast) and treating the solution with nitric acid, boiling off the HCl.
Aluminum metal is often prepared for welding by removing the oxide film with dilute hydrofluoric acid. The aluminum surface is bare metal for, oh, maybe a microsecond, before oxidizing back to the oxide. But the aluminum oxide film will be very thin for a few hours and easy to weld. The oxide film grows thicker in air as it ages.
Aluminum oxide could be the product of fusing Al(NO3)3 at high enough temperature. Aluminum metal would not be a product, in water or in fused salt.
2.Aluminum metal does not readily dissolve in nitric acid because of formation of passive oxide/hydroxide film. The nuclear power industry had need of large amounts of aluminum nitrate, and it was made by dissolving aluminum metal in hydrochloric acid (very fast) and treating the solution with nitric acid, boiling off the HCl.
Aluminum metal is often prepared for welding by removing the oxide film with dilute hydrofluoric acid. The aluminum surface is bare metal for, oh, maybe a microsecond, before oxidizing back to the oxide. But the aluminum oxide film will be very thin for a few hours and easy to weld. The oxide film grows thicker in air as it ages.
Industrial preparation of Al using electrolysis of molten $\ce{AlF3/AlO2}$ mixture at $\pu{1500 ^\circ C}$ is done not because they like using high temperatures, but because there are no other good ways to make Al. Hydrolysis of aqueous solutions of aluminum salts will not yield metallic aluminum.
Can $\ce{Al(OH)3}$ react with $\ce{HNO3}$? It really depends. Fresh $\ce{Al(OH)3}$ will dissolve in dilute $\ce{HNO3}$. Old $\ce{Al(OH)3}$ ages to $\ce{Al(OH)3}$ and is much less reactive.
Electrolysis of water solution of aluminum salt will not yield metallic aluminum. Hydrolysis of $\ce{AlCl3}$ yields $\ce{H2 + O2/Cl2}$. $\ce{Al(NO3)3}$ will be reduced by forming hydrogen, so you well get a a mix of products: $\ce{NO2}$, $\ce{NO}$, $\ce{H2}$, but not aluminum metal. If this were easy, industry wouldn't bother with hydrolysis of molten $\ce{AlF3/Al2O3}$.
Industrial preparation of Al using electrolysis of molten $\ce{AlF3/AlO2}$ mixture at $\pu{1500 ^\circ C}$ is done not because they like using high temperatures, but because there are no other good ways to make Al. Hydrolysis of aqueous solutions of aluminum salts will not yield metallic aluminum.
Can $\ce{Al(OH)3}$ react with $\ce{HNO3}$? It really depends. Fresh $\ce{Al(OH)3}$ will dissolve in dilute $\ce{HNO3}$. Old $\ce{Al(OH)3}$ ages to $\ce{Al(OH)3}$ and is much less reactive.
Electrolysis of water solution of aluminum salt will not yield metallic aluminum. Hydrolysis of $\ce{AlCl3}$ yields $\ce{H2 + O2/Cl2}$. $\ce{Al(NO3)3}$ will be reduced by forming hydrogen, so you well get a a mix of products: $\ce{NO2}$, $\ce{NO}$, $\ce{H2}$, but not aluminum metal. If this were easy, industry wouldn't bother with hydrolysis of molten $\ce{AlF3/Al2O3}$.
Aluminum oxide could be the product of fusing Al(NO3)3 at high enough temperature. Aluminum metal would not be a product, in water or in fused salt.
2.Aluminum metal does not readily dissolve in nitric acid because of formation of passive oxide/hydroxide film. The nuclear power industry had need of large amounts of aluminum nitrate, and it was made by dissolving aluminum metal in hydrochloric acid (very fast) and treating the solution with nitric acid, boiling off the HCl.
Aluminum oxide could be the product of fusing Al(NO3)3 at high enough temperature. Aluminum metal would not be a product, in water or in fused salt.
2.Aluminum metal does not readily dissolve in nitric acid because of formation of passive oxide/hydroxide film. The nuclear power industry had need of large amounts of aluminum nitrate, and it was made by dissolving aluminum metal in hydrochloric acid (very fast) and treating the solution with nitric acid, boiling off the HCl.
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Industrial preparation of Al using electrolysis of molten $\ce{AlF3/AlO2}$ mixture at $\pu{1500 ^\circ C}$ is done not because they like using high temperatures, but because there are no other good ways to make Al. Hydrolysis of aqueous solutions of aluminum salts will not yield metallic aluminum.
Can $\ce{Al(OH)3}$ react with $\ce{HNO3}$? It really depends. Fresh $\ce{Al(OH)3}$ will dissolve in dilute $\ce{HNO3}$. Old $\ce{Al(OH)3}$ ages to $\ce{Al(OH)3}$ and is much less reactive.
Electrolysis of water solution of aluminum salt will not yield metallic aluminum. Hydrolysis of $\ce{AlCl3}$ yields $\ce{H2 + O2/Cl2}$. $\ce{Al(NO3)3}$ will be reduced by forming hydrogen, so you well get a a mix of products: $\ce{NO2}$, $\ce{NO}$, $\ce{H2}$, but not aluminum metal. If this were easy, industry wouldn't bother with hydrolysis of molten $\ce{AlF3/Al2O3}$.
Industrial preparation of Al using electrolysis of molten $\ce{AlF3/AlO2}$ mixture at $\pu{1500 ^\circ C}$ is done not because they like using high temperatures, but because there are no other good ways to make Al. Hydrolysis of aqueous solutions of aluminum salts will not yield metallic aluminum.
Can $\ce{Al(OH)3}$ react with $\ce{HNO3}$? It really depends. Fresh $\ce{Al(OH)3}$ will dissolve in dilute $\ce{HNO3}$. Old $\ce{Al(OH)3}$ ages to $\ce{Al(OH)3}$ and is much less reactive.
Electrolysis of water solution of aluminum salt will not yield metallic aluminum. Hydrolysis of $\ce{AlCl3}$ yields $\ce{H2 + O2/Cl2}$. $\ce{Al(NO3)3}$ will be reduced by forming hydrogen, so you well get a a mix of products: $\ce{NO2}$, $\ce{NO}$, $\ce{H2}$, but not aluminum metal. If this were easy, industry wouldn't bother with hydrolysis of molten $\ce{AlF3/Al2O3}$.
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