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How to prepare manganese nitrate Mn(NO3)2?
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+ Inorganic chemistry
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Mike Webster
How to prepare manganese nitrate Mn(NO3)2?
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Hi, I tried to prepare Mn(NO3)2 in the lab using Mn powder and dil HNO3, filter and dry. I got brown powder and I tested the nitrate ion in the product solution using NaOH and Al-foil but I got Red brownish fumes and it should be ammonia fumes. Does any know correct method to prepare Mn(NO3)2? Thanks
Uhlmann's suggests MnCO3 + HNO3 - see https://en.wikipedia.org/w/index.php?title=Manganese(II)_nitrate&oldid=703933419 which may also explain your fumes.
Hi, I tried to prepare Mn(NO3)2 in the lab using Mn powder and dil HNO3, filter and dry. I got brown powder and I tested the nitrate ion in the product solution using NaOH and Al-foil but I got Red brownish fumes and it should be ammonia fumes. Does any know correct method to prepare Mn(NO3)2? Thanks
Uhlmann's suggests MnCO3 + HNO3 - see https://en.wikipedia.org/w/index.php?title=Manganese(II)_nitrate&oldid=703933419 which may also explain your fumes.
Other cheaper option would be to start wie MnSO4 and Ba(NO3)2 you get BaSO4 as precipitate and Mn(NO3)2 will be in the solution. Cheaper as to use AgNO3.
Other cheaper option would be to start wie MnSO4 and Ba(NO3)2 you get BaSO4 as precipitate and Mn(NO3)2 will be in the solution. Cheaper as to use AgNO3.
I mix MnCO3 with Dil HNO3 (10%)(reaction for 20min) then filter
If I have not mistaken in my calculations, 10% HNO3 is about 2.4M, which maybe still too concentrated to prevent unwanted oxidation. I learnt from school that if only acid-base reactions are desired, 'very dilute'(<0.1M) HNO3 is used.
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I found dark brown residue in filter paper can't be removed
I mix MnCO3 with Dil HNO3 (10%)(reaction for 20min) then filter
If I have not mistaken in my calculations, 10% HNO3 is about 2.4M, which maybe still too concentrated to prevent unwanted oxidation. I learnt from school that if only acid-base reactions are desired, 'very dilute'(<0.1M) HNO3 is used.
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I found dark brown residue in filter paper can't be removed
well, I prepared MnCO3 from MnCl2 and Na2CO3(reaction for 24h) after that I mix MnCO3 with Dil HNO3 (10%)(reaction for 20min) then filter, and evaporate the filtrate but after evaporation I didn't get any product(flask was empty).
well, I prepared MnCO3 from MnCl2 and Na2CO3(reaction for 24h) after that I mix MnCO3 with Dil HNO3 (10%)(reaction for 20min) then filter, and evaporate the filtrate but after evaporation I didn't get any product(flask was empty).
well, I prepared MnCO3 from MnCl2 and Na2CO3(reaction for 24h) after that I mix MnCO3 with Dil HNO3 (10%)(reaction for 20min) then filter, and evaporate the filtrate but after evaporation I didn't get any product(flask was empty).
My question is why you have to filter after add nitric to the manganese carbonate. I think your manganese was oxidized to MnO2 . After filtering you have only water and nitric in the flask.
well, I prepared MnCO3 from MnCl2 and Na2CO3(reaction for 24h) after that I mix MnCO3 with Dil HNO3 (10%)(reaction for 20min) then filter, and evaporate the filtrate but after evaporation I didn't get any product(flask was empty).
My question is why you have to filter after add nitric to the manganese carbonate. I think your manganese was oxidized to MnO2 . After filtering you have only water and nitric in the flask.
Nitric acid is a strong oxidizer, it will do more than you need when given metal to react with. MnCO3 and (reasonably) diluted acid sounds like a better option (even if Mn2+ can probably reduce NO3-).
Nitric acid is a strong oxidizer, it will do more than you need when given metal to react with. MnCO3 and (reasonably) diluted acid sounds like a better option (even if Mn2+ can probably reduce NO3-).
Uhlmann's suggests MnCO3 + HNO3 - see https://en.wikipedia.org/w/index.php?title=Manganese(II)_nitrate&oldid=703933419 which may also explain your fumes.
Uhlmann's suggests MnCO3 + HNO3 - see https://en.wikipedia.org/w/index.php?title=Manganese(II)_nitrate&oldid=703933419 which may also explain your fumes.
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Me + 4 HNO3 => Me(NO3)2 + 2 NO2 + 2 H2O
So the recomandation to use Carbonate or maybe also the Hydroxide will be more safe.
Other option would be to use AgNO3 and MnCl2
It will give a precipitation of AgCl and Mn(NO3)2 will be left.
Me + 4 HNO3 => Me(NO3)2 + 2 NO2 + 2 H2O
So the recomandation to use Carbonate or maybe also the Hydroxide will be more safe.
Other option would be to use AgNO3 and MnCl2
It will give a precipitation of AgCl and Mn(NO3)2 will be left.
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If I have not mistaken in my calculations, 10% HNO3 is about 2.4M, which maybe still too concentrated to prevent unwanted oxidation. I learnt from school that if only acid-base reactions are desired, 'very dilute'(<0.1M) HNO3 is used.
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Likely to be MnO2
If I have not mistaken in my calculations, 10% HNO3 is about 2.4M, which maybe still too concentrated to prevent unwanted oxidation. I learnt from school that if only acid-base reactions are desired, 'very dilute'(<0.1M) HNO3 is used.
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Likely to be MnO2
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My question is why you have to filter after add nitric to the manganese carbonate. I think your manganese was oxidized to MnO2 . After filtering you have only water and nitric in the flask.
My question is why you have to filter after add nitric to the manganese carbonate. I think your manganese was oxidized to MnO2 . After filtering you have only water and nitric in the flask.
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MnCO3+HNO3=Mn(NO3)2+H2O+CO2(colorless gas)
MnCO3+HNO3=Mn(NO3)2+H2O+CO2(colorless gas)
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