Aluminium normally has a thin, colorless coating of its oxide, which is essentially inert chemically. (Such a coating is called a protective oxide.) The nitric acid can’t attack the metal under its “armor coating”. If the metal were scratched while it was in the acid, so that there was a break in the oxide, then corrosion would begin.
Aluminium normally has a thin, colorless coating of its oxide, which is essentially inert chemically. (Such a coating is called a protective oxide.) The nitric acid can’t attack the metal under its “armor coating”. If the metal were scratched while it was in the acid, so that there was a break in the oxide, then corrosion would begin.
Nitric acid is an acid, but it also is a powerful oxidizing agent. Nitrogen in HNO3 is in +5 oxidation state, and is looking to add electrons (get reduced). Lead metal is a somewhat active reductant (it is a metal after all), since it can donate electrons (get oxidized) and get up to +2 [Pb (II)] or +4 [Pb (IV)] oxidation state.
When Pb metal reacts with dilute HNO3, a redox reaction takes place, and Pb(NO3)2 + NO + H2O is formed. Nitric oxide (NO) can react further with oxygen in the air to form nitrogen dioxide (NO2).
When concentrated HNO3 is used with lead metal, formation of PbO (lead oxide) is favored. Lead oxide is insoluble in acid, and forms a coating over the residual metal, rendering it inactive (inaccessible to acid). Therefore, no apparent reaction is observed.
PbO formed above can react further with HNO3 to produce Pb(NO3)2, NO2 + H2O. However, this might require the use of finely divided Pb metal to start the reaction.
Nitric acid is an acid, but it also is a powerful oxidizing agent. Nitrogen in HNO3 is in +5 oxidation state, and is looking to add electrons (get reduced). Lead metal is a somewhat active reductant (it is a metal after all), since it can donate electrons (get oxidized) and get up to +2 [Pb (II)] or +4 [Pb (IV)] oxidation state.
When Pb metal reacts with dilute HNO3, a redox reaction takes place, and Pb(NO3)2 + NO + H2O is formed. Nitric oxide (NO) can react further with oxygen in the air to form nitrogen dioxide (NO2).
When concentrated HNO3 is used with lead metal, formation of PbO (lead oxide) is favored. Lead oxide is insoluble in acid, and forms a coating over the residual metal, rendering it inactive (inaccessible to acid). Therefore, no apparent reaction is observed.
PbO formed above can react further with HNO3 to produce Pb(NO3)2, NO2 + H2O. However, this might require the use of finely divided Pb metal to start the reaction.
Thermodynamically, aluminum will react with any acid, but some acids (such as HCl) are better at getting through the protective oxide layer on the surface of aluminum, and thus there can be big differences kinetically.
Thermodynamically, aluminum will react with any acid, but some acids (such as HCl) are better at getting through the protective oxide layer on the surface of aluminum, and thus there can be big differences kinetically.
When Al reacts with HCl it forms AlCl3 which is soluble but when it reacts with HNO3 its upper layer gets oxidised in to Al2O3 which is passive for further reaction with HNO3 as Al2O3 is highly stable metal oxide.
When Al reacts with HCl it forms AlCl3 which is soluble but when it reacts with HNO3 its upper layer gets oxidised in to Al2O3 which is passive for further reaction with HNO3 as Al2O3 is highly stable metal oxide.
It will depend on the concentration of the nitric acid used….
Although aluminium reacts with dilute nitric acid to produce aluminium nitrate and hydrogen gas, concentrated (>60%) nitric acid is such a powerful oxidising agent that it instantly causes a thin layer of aluminium oxide to coat the surface of the aluminium.
The oxide coating is resistant to nitric acid attack and therefore prevents any further reaction. This process is called passivation and also occurs with chromium, cobalt, iron and nickel.
It will depend on the concentration of the nitric acid used….
Although aluminium reacts with dilute nitric acid to produce aluminium nitrate and hydrogen gas, concentrated (>60%) nitric acid is such a powerful oxidising agent that it instantly causes a thin layer of aluminium oxide to coat the surface of the aluminium.
The oxide coating is resistant to nitric acid attack and therefore prevents any further reaction. This process is called passivation and also occurs with chromium, cobalt, iron and nickel.
Aluminium is so reactive that as soon as you cut the surface, the fresh aluminium reacts with oxygen from the air to form an insoluble, mostly impervious, layer that prevents any further reaction.
This means that the aluminium, although it is high on the reactivity series, it appears less reactive than iron.
Aluminium is so reactive that as soon as you cut the surface, the fresh aluminium reacts with oxygen from the air to form an insoluble, mostly impervious, layer that prevents any further reaction.
This means that the aluminium, although it is high on the reactivity series, it appears less reactive than iron.
Nitric acid reacts with aluminium and forms a protective layer i.e. Al2O3. This protective layer makes aluminium unreactive towards HNO3 and therefore, it can be stored in aluminium containers.
Nitric acid reacts with aluminium and forms a protective layer i.e. Al2O3. This protective layer makes aluminium unreactive towards HNO3 and therefore, it can be stored in aluminium containers.
When aluminium reacts with dilute sulphuric acid it forms aluminium salt and hydrogen gas evolve…….
METAL+ DILUTE ACID———- SALT+ HYDROGEN GAS
2Al+ 3H2SO4————-2Al(SO4)3 + 3H2
When aluminium reacts with dilute sulphuric acid it forms aluminium salt and hydrogen gas evolve…….
METAL+ DILUTE ACID———- SALT+ HYDROGEN GAS
2Al+ 3H2SO4————-2Al(SO4)3 + 3H2
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Why can nitric acid not react with aluminium?
Aluminium normally has a thin, colorless coating of its oxide, which is essentially inert chemically. (Such a coating is called a protective oxide.)
The nitric acid can’t attack the metal under its “armor coating”.
If the metal were scratched while it was in the acid, so that there was a break in the oxide, then corrosion would begin.
Why can nitric acid not react with aluminium?
Aluminium normally has a thin, colorless coating of its oxide, which is essentially inert chemically. (Such a coating is called a protective oxide.)
The nitric acid can’t attack the metal under its “armor coating”.
If the metal were scratched while it was in the acid, so that there was a break in the oxide, then corrosion would begin.
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Nitric acid is an acid, but it also is a powerful oxidizing agent. Nitrogen in HNO3 is in +5 oxidation state, and is looking to add electrons (get reduced). Lead metal is a somewhat active reductant (it is a metal after all), since it can donate electrons (get oxidized) and get up to +2 [Pb (II)] or +4 [Pb (IV)] oxidation state.
When Pb metal reacts with dilute HNO3, a redox reaction takes place, and Pb(NO3)2 + NO + H2O is formed. Nitric oxide (NO) can react further with oxygen in the air to form nitrogen dioxide (NO2).
When concentrated HNO3 is used with lead metal, formation of PbO (lead oxide) is favored. Lead oxide is insoluble in acid, and forms a coating over the residual metal, rendering it inactive (inaccessible to acid). Therefore, no apparent reaction is observed.
PbO formed above can react further with HNO3 to produce Pb(NO3)2, NO2 + H2O. However, this might require the use of finely divided Pb metal to start the reaction.
Nitric acid is an acid, but it also is a powerful oxidizing agent. Nitrogen in HNO3 is in +5 oxidation state, and is looking to add electrons (get reduced). Lead metal is a somewhat active reductant (it is a metal after all), since it can donate electrons (get oxidized) and get up to +2 [Pb (II)] or +4 [Pb (IV)] oxidation state.
When Pb metal reacts with dilute HNO3, a redox reaction takes place, and Pb(NO3)2 + NO + H2O is formed. Nitric oxide (NO) can react further with oxygen in the air to form nitrogen dioxide (NO2).
When concentrated HNO3 is used with lead metal, formation of PbO (lead oxide) is favored. Lead oxide is insoluble in acid, and forms a coating over the residual metal, rendering it inactive (inaccessible to acid). Therefore, no apparent reaction is observed.
PbO formed above can react further with HNO3 to produce Pb(NO3)2, NO2 + H2O. However, this might require the use of finely divided Pb metal to start the reaction.
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Thermodynamically, aluminum will react with any acid, but some acids (such as HCl) are better at getting through the protective oxide layer on the surface of aluminum, and thus there can be big differences kinetically.
Thermodynamically, aluminum will react with any acid, but some acids (such as HCl) are better at getting through the protective oxide layer on the surface of aluminum, and thus there can be big differences kinetically.
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But it does dissolve in nitric acid. (I have done it a few times as part of a phos anodize demo tank prep.)
Check your sources b4 u post. Save from making your cheeks so pink.
But it does dissolve in nitric acid. (I have done it a few times as part of a phos anodize demo tank prep.)
Check your sources b4 u post. Save from making your cheeks so pink.
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When Al reacts with HCl it forms AlCl3 which is soluble but when it reacts with HNO3 its upper layer gets oxidised in to Al2O3 which is passive for further reaction with HNO3 as Al2O3 is highly stable metal oxide.
When Al reacts with HCl it forms AlCl3 which is soluble but when it reacts with HNO3 its upper layer gets oxidised in to Al2O3 which is passive for further reaction with HNO3 as Al2O3 is highly stable metal oxide.
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HNO3 or nitric acid is made by dissolving NO2 in water
H2O + 2NO2 = 2HNO3
HNO3 or nitric acid is made by dissolving NO2 in water
H2O + 2NO2 = 2HNO3
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It will depend on the concentration of the nitric acid used….
Although aluminium reacts with dilute nitric acid to produce aluminium nitrate and hydrogen gas, concentrated (>60%) nitric acid is such a powerful oxidising agent that it instantly causes a thin layer of aluminium oxide to coat the surface of the aluminium.
The oxide coating is resistant to nitric acid attack and therefore prevents any further reaction. This process is called passivation and also occurs with chromium, cobalt, iron and nickel.
It will depend on the concentration of the nitric acid used….
Although aluminium reacts with dilute nitric acid to produce aluminium nitrate and hydrogen gas, concentrated (>60%) nitric acid is such a powerful oxidising agent that it instantly causes a thin layer of aluminium oxide to coat the surface of the aluminium.
The oxide coating is resistant to nitric acid attack and therefore prevents any further reaction. This process is called passivation and also occurs with chromium, cobalt, iron and nickel.
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Aluminium is so reactive that as soon as you cut the surface, the fresh aluminium reacts with oxygen from the air to form an insoluble, mostly impervious, layer that prevents any further reaction.
This means that the aluminium, although it is high on the reactivity series, it appears less reactive than iron.
Aluminium is so reactive that as soon as you cut the surface, the fresh aluminium reacts with oxygen from the air to form an insoluble, mostly impervious, layer that prevents any further reaction.
This means that the aluminium, although it is high on the reactivity series, it appears less reactive than iron.
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Nitric acid reacts with aluminium and forms a protective layer i.e. Al2O3. This protective layer makes aluminium unreactive towards HNO3 and therefore, it can be stored in aluminium containers.
Nitric acid reacts with aluminium and forms a protective layer i.e. Al2O3. This protective layer makes aluminium unreactive towards HNO3 and therefore, it can be stored in aluminium containers.
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What…?
Let’s take conc. HCl, 12M for example. The result is obvious.
BHP
What…?
Let’s take conc. HCl, 12M for example. The result is obvious.
BHP
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