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pneumatician
National Hazard
Posts: 393
Registered: 27-5-2013
Location: Catalonia
Member Is Offline
Mood: ■■■■■■■■■■ INRI ■■■■■■■■■■ ** Igne Natura Renovatur Integra **
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if you reduce it to dust?? no more sprinkled around???
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DraconicAcid
International Hazard
Posts: 4088
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
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Reacting some of my samarium with sulphuric acid. Yellow.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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B(a)P
International Hazard
Posts: 946
Registered: 29-9-2019
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Mood: Confined
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Distillation of fuming nitric acid from potassium nitrate and concentrated sulfuric acid.
Measured density 1.54 g/mL +- 0.03 g/mL at 15C, so likely north of 98% concentration.
Pretty happy with that!
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Sir_Gawain
Harmless
Posts: 30
Registered: 12-10-2022
Location: Camelot
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Mood: Li2CO3
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Tried to make NHN with hydrazine dihydrogenchloride. The freebasing really sucked because I ran out of filter paper. When I began addition of nickel
nitrate a bluish precipitate formed, then changed to light purple. The dried product was only slightly energetic.
The difference between chemistry and alchemy is that, with alchemy, if things go yellow, that's good!
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solitanze
Harmless
Posts: 26
Registered: 4-2-2016
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Mood: No Mood
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I made a good sized quantity of Mohr's salt, ferrous ammonium sulfate from fertilizers. The pale green crystals are really pretty.
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DraconicAcid
International Hazard
Posts: 4088
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
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Going to work up my samarium(III) sulphate.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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Rainwater
National Hazard
Posts: 426
Registered: 22-12-2021
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Just watched my fireworks sparkle. 3 of 5 were successful.
All burned completely, failures simply did not have effect, only color.
All ammonia perchlorate based, 8g
powdered sugar, 5g
2g sulfur
10g nitrate salts charcoal powder blend
5g of effect
6in long, 1in diameter cardboard tube.
Aluminum nitrate with Iron powder wrapped in magnesium foil
Copper nitrate with wax coated Calcium metal beads.
Tin nitrate wax coated Sodium beads (Fail)
Silver nitrate with wax coated Potassium/sodium beads. (Will do again, machine gun like pops)
Lithium nitrate with wax coated aluminum powder(fail)
Stay safe friends
"You can't do that" - challenge accepted
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DraconicAcid
International Hazard
Posts: 4088
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
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Okay, so I worked up my samarium(III) sulphate. Nice yellow powder (gonna have to find a way to get crystals of it).
A bunch of the metal didn't react, so I put it in hydrochloric acid. Immediate, vigorous reaction, and it turned red. Once it settled down, there
was a yellow solution, a bit of still-fizzing metal bits, and some red precipitate. Red?? I thought all samarium(III) compounds were yellow.
Samarium(II) chloride is brown, but isn't water-stable. Insoluble samarium(II) sulphate, maybe?
ETA: Actually, it seems that it should be samarium(II) sulphate:
https://scholarworks.uni.edu/cgi/viewcontent.cgi?article=315...
If so, it should be samarium(III) tomorrow.
ETA: Yep. It's all yellow now.
[Edited on 5-1-2023 by DraconicAcid]
[Edited on 5-1-2023 by DraconicAcid]
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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j_sum1
Administrator
Posts: 5973
Registered: 4-10-2014
Location: Unmoved
Member Is Offline
Mood: It's chromium time.
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Potassium dichromate
Potassium dichromate
One of my first ever experiments was the aluminothermic reduction of pottery grade chromium oxide to obtain elemental chromium for my element
collection. Product was obviously impure with lots of aluminium products in the mix. Recently I have been attempting to make something useful from
the mixture. Procedure as follows:
Digest with concentrated HCl to make a solution containing Cr(III)
Neutralise and precipitate with sodium carbonate.
Repeated filter and wash steps to obtain Cr2(CO3)3 of acceptable purity. (Stuff is a dog to filter: not as bad as calcium sulfate but close.)
Dry and roast to obtain Cr2O3
React with KNO3 to get potassium dichromate. Cr2O3 + 2KNO3 --> K2Cr2O7 + 2NO.
Dissolve in water, filter and crystallise.
I have had a bit of fun playing with other routes and other oxidisers to target other useful Cr(VI) compounds: sodium or ammonium dichromate of
chromates. The problem with sodium dichromate is separating it from soluble byproducts at sensible yields. Similarly, ammonium dichromate is going
to have high yield loss and impurity issues due to other species that will crystallise out at the same time. Isolation of calcium chromate might be
a good idea, and easy to separate since it has an inverse solubility curve and is quite insoluble anyway. But I have very little calcium nitrate and
so it is not very practical as a recovery method.
I do have a lovely array of bright coloured test tubes for my efforts.
[Edited on 1-4-2023 by j_sum1]
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Admagistr
Hazard to Others
Posts: 184
Registered: 4-11-2021
Location: Central Europe
Member Is Offline
Mood: The dreaming alchemist
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@ j_sum1
Neutralise and precipitate with sodium carbonate.
Repeated filter and wash steps to obtain Cr2(CO3)3 of acceptable purity.
Are you sure that chromium (III) carbonate exists??When I precipitated it out of solution, after a short time CO2 was released and undoubtedly Cr(OH)3
was formed. Similarly, aluminium carbonate cannot be prepared...Even in the literature-Remy,Inorganic Chemistry-It is said that carbonates of Al and
Cr cannot be precipitated from aqueous solution because they are unstable and turn into hydroxides when CO2 is released...
[Edited on 1-4-2023 by Admagistr]
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