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What does lithium and nitric acid form?
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Kaju Deka
What does lithium and nitric acid form?
You cannot convert concentrated nitric acid into anhydrous nitric acid by distillation, because the standard concentration is an azeotrope.
The anhydrous acid is known commercially as white fuming nitric acid WFNA and is used as an oxidant with rocket fuel. It is also available for laboratories.
In order to manufacture it, you have to make it without water, by swapping the sulfate bit of H2SO4 with the nitrate from KNO3. That is, heat these two compounds together and condense the vapors which come off, since HNO3 has a lower boiling point (83°C) than H2SO4 (337°C). Further purification using a great deal of skill to get to the assay you require.
It is recommended that you do not do this at home!
While at school, I came across an exam question which was why anhydrous copper nitrate could not be prepared (because the hydrated form decomposes when you try to remove the water). So as a project I prepared it by dissolving copper metal in N2O4. This taught me a lot about working with dry materials. It was furiously hygroscopic.
You cannot convert concentrated nitric acid into anhydrous nitric acid by distillation, because the standard concentration is an azeotrope.
The anhydrous acid is known commercially as white fuming nitric acid WFNA and is used as an oxidant with rocket fuel. It is also available for laboratories.
In order to manufacture it, you have to make it without water, by swapping the sulfate bit of H2SO4 with the nitrate from KNO3. That is, heat these two compounds together and condense the vapors which come off, since HNO3 has a lower boiling point (83°C) than H2SO4 (337°C). Further purification using a great deal of skill to get to the assay you require.
It is recommended that you do not do this at home!
While at school, I came across an exam question which was why anhydrous copper nitrate could not be prepared (because the hydrated form decomposes when you try to remove the water). So as a project I prepared it by dissolving copper metal in N2O4. This taught me a lot about working with dry materials. It was furiously hygroscopic.
Since nitric acid is a strong oxidising agent, even in dilute solution, hydrogen gas is not produced when lithium (and many other metals) react with nitric acid.
In the case of lithium and dilute nitric acid, lithium nitrate, ammonium nitrate and water are produced;-
8 Li + 10 HNO₃ → 8 LiNO₃ + NH₄NO₃ + 3 H₂O
Concentrated nitric acid reacts with lithium to produce lithium nitrate, nitric oxide gas and water;-
Since nitric acid is a strong oxidising agent, even in dilute solution, hydrogen gas is not produced when lithium (and many other metals) react with nitric acid.
In the case of lithium and dilute nitric acid, lithium nitrate, ammonium nitrate and water are produced;-
8 Li + 10 HNO₃ → 8 LiNO₃ + NH₄NO₃ + 3 H₂O
Concentrated nitric acid reacts with lithium to produce lithium nitrate, nitric oxide gas and water;-
You cannot convert concentrated nitric acid into anhydrous nitric acid by distillation, because the standard concentration is an azeotrope.
The anhydrous acid is known commercially as white fuming nitric acid WFNA and is used as an oxidant with rocket fuel. It is also available for laboratories.
In order to manufacture it, you have to make it without water, by swapping the sulfate bit of H2SO4 with the nitrate from KNO3. That is, heat these two compounds together and condense the vapors which come off, since HNO3 has a lower boiling point (83°C) than H2SO4 (337°C). Further purification using a great deal of skill to get to the assay you require.
It is recommended that you do not do this at home!
While at school, I came across an exam question which was why anhydrous copper nitrate could not be prepared (because the hydrated form decomposes when you try to remove the water). So as a project I prepared it by dissolving copper metal in N2O4. This taught me a lot about working with dry materials. It was furiously hygroscopic.
You cannot convert concentrated nitric acid into anhydrous nitric acid by distillation, because the standard concentration is an azeotrope.
The anhydrous acid is known commercially as white fuming nitric acid WFNA and is used as an oxidant with rocket fuel. It is also available for laboratories.
In order to manufacture it, you have to make it without water, by swapping the sulfate bit of H2SO4 with the nitrate from KNO3. That is, heat these two compounds together and condense the vapors which come off, since HNO3 has a lower boiling point (83°C) than H2SO4 (337°C). Further purification using a great deal of skill to get to the assay you require.
It is recommended that you do not do this at home!
While at school, I came across an exam question which was why anhydrous copper nitrate could not be prepared (because the hydrated form decomposes when you try to remove the water). So as a project I prepared it by dissolving copper metal in N2O4. This taught me a lot about working with dry materials. It was furiously hygroscopic.
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Since nitric acid is a strong oxidising agent, even in dilute solution, hydrogen gas is not produced when lithium (and many other metals) react with nitric acid.
In the case of lithium and dilute nitric acid, lithium nitrate, ammonium nitrate and water are produced;-
8 Li + 10 HNO₃ → 8 LiNO₃ + NH₄NO₃ + 3 H₂O
Concentrated nitric acid reacts with lithium to produce lithium nitrate, nitric oxide gas and water;-
Li + 2HNO₃ → LiNO₃ + NO₂ + H₂O
See Properties of lithium, and the reactions of water and certain acids with lithium
Since nitric acid is a strong oxidising agent, even in dilute solution, hydrogen gas is not produced when lithium (and many other metals) react with nitric acid.
In the case of lithium and dilute nitric acid, lithium nitrate, ammonium nitrate and water are produced;-
8 Li + 10 HNO₃ → 8 LiNO₃ + NH₄NO₃ + 3 H₂O
Concentrated nitric acid reacts with lithium to produce lithium nitrate, nitric oxide gas and water;-
Li + 2HNO₃ → LiNO₃ + NO₂ + H₂O
See Properties of lithium, and the reactions of water and certain acids with lithium
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