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bur
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Radium extration
Has anyone ever tried to extract Radium?
I know the amounts are tiny, so I'm thinking of a Ra+-solution as the product. The extration to the point of a RaCl solution is not too hard:
Dissolution of U ore in H2SO4 leaves Ba,Ra and some other insoluble sulfates.
Most impurities are removed via NaOH and subsequent HCl.
Ba impurities remain in the sludge and the (Ba,Ra)SO4 is converted to (Ba,Ra)CO3 and dissolved in HCl.
The only practical way to know if you were successful is from radiation though. As I don't have a gamma spectrometer available I'd have to rely on a
Geiger counter. My problem is, there are lots of other radioactive isotopes in the ore and I'm not sure if any of them might not be extracted along
the Radium. Of course their amounts are minute, but their activity isn't. So if the product is active it might be anything.
Especially the two Pb isotopes 210 and 214-Pb could end up with the Ba. I'd say separation of ng amounts of Pb from Ba might not be possible?
I thought I could add Ba at the last extraction step so I have something to precipitate. Then I'd end up with BaSO4 with a small amount of Ra
incorporated.
Long story short: Will I be able to separate the Ra from the other decay products?
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DoctorOfPhilosophy
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Alexander Wimmer (a student in Austria) did exactly that, starting with uranothorianite. Supposedly his yield was 0.5 ug.
http://theodoregray.com/periodictable/Elements/088/index.s7....
Edit: to be exact, it's a small amount of RaCO3 in BaCO3. I doubt anyone has gotten past that point in recent times but it's no secret how to
concentrate the radium further.
[Edited on 21-6-2016 by DoctorOfPhilosophy]
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metalresearcher
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How did you get the U metal ?
Most ebay shops don't sell radioactive elements or compounds, except K (which contains 1:8600 K-40).
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careysub
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You should consult Mme Curie's original papers on radium extraction (her PhD dissertation for example), and other radium extraction literature.
The techniques are all detailed there (but use better safety methods).
[Edited on 21-6-2016 by careysub]
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phlogiston
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metalresearcher, he mentions U ore, which is a much better choice, because it will have all of U's daughters in equilibrium concentrations, whereas
these will not be present except in minute quantities in U metal because they take a long time to grow back in (they have been removed when U was
extracted from the ore).
bur, a colleague a long time ago used a method to extract small lead impurities from a barium sulphate precipitate with certain solutions but
unfortunately I can't recall what he used exactly. Sorry, but at least it is possible. A quick google search suggest ammonium acetate or EDTA, but I
haven't looked into it.
Pb-214 has a short half-life (around 22 minutes), so you won't have to worry about it. That is not the case for Pb-210 though.
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bur
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Thanks for your answers.
phlogiston, you're right I completely forgot about the high decay rate of Pb-214... But after having a look at the decay chain again I think it won't
help. Pb-214 ends up as Pb-210 via Bi-214 and Po-214 after a few minutes. Then it takes a couple of decades to end up as stable Pb-206.
So I guess I'll just go with the simple procedure and hopefully end up with (Ba,Ra,Pb)CO3.
As was stated to extract Ra you need ore as it takes about 100 000 years until Ra equilibrium is reached. You can easily detect how much more active
ore is compared to synthetic U compounds (including non-depleted). This is why mine tailings are usually more active than the extracted product.
metalresearcher, you're right metal cannot be bought easily anymore at least in the EU unless you have a license. If you're in the US however, there
is at least one shop selling depleted U metal and other compounds.
This whole extraction is illegal in many countries though unless you have permission to produce radioactive substances.
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Heavy Walter
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OTC radium
Hi bur
In case you do for the fun of the extraction chemistry, go to the U ore (many mineral clubs and fairs sell small samples of different U minerals).
In case of looking the Ra for other experiments, I suggest to look at antique shops, flea markets and old clock repair shops for two items:
products from the radium quack (water "activators") and spare needles from luminous watches. (Later Ra was replaced by Tritium, so you need to measure
activity).
I have been successful in both areas, even getting a kit to apply the radioactive painting!
Of course, a handy Geiger is mandatory.
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careysub
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Here are some notes I took while reading Mme Curie's writings on uranium ore extraction. She of course was interested in separating all of the
radioactive elements, not just radium
"Digestion of ore in concentrated sulfuric acid dissolves uranium and protactinium. For many uranium ores oxidizing conditions are needed for complete
uranium dissolution. Lead, radium, polonium and actinium sulfates are insoluble.
The insoluble residue is dissolved with HCl which removes some of the polonium and actinium. Polonium can be precipitated with H2S. Actinium can be
obtained after separating the solution from the sulfide residues, peroxidizing, then precipitating with ammonia.
The sulfate residue is boiled with sodium carbonate to remove all sulfates, it is then washed with water, and then dissolved in dilute HCl (sulfuric
acid free). This solution contains radium, actinium and polonium. It is filtered and precipitated with sulfuric acid, which carries down barium and
radium plus a little lead and actinium. The solution still contains a little actinium and polonium which can be recovered by using HCl.
The sulfate precipitate is boiled with sodium carbonate, then dissolved in HCl. Polonium is precipitated with H2S. The solution is oxidized with
chlorine and precipitated with pure ammonia to remove actinium. The filtered solution is precipitated with sodium carbonate. The precipitate is washed
and converted to chlorides, which are evaporate to dryness and washed with conc. HCl. Calcium chloride dissolves almost entirely, leaving barium and
radium chloride, ready for fractionation."
[Edited on 24-6-2016 by careysub]
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careysub
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Quote: Originally posted by Heavy Walter  | Hi bur
In case you do for the fun of the extraction chemistry, go to the U ore (many mineral clubs and fairs sell small samples of different U minerals).
In case of looking the Ra for other experiments, I suggest to look at antique shops, flea markets and old clock repair shops for two items:
products from the radium quack (water "activators") and spare needles from luminous watches. (Later Ra was replaced by Tritium, so you need to measure
activity).
I have been successful in both areas, even getting a kit to apply the radioactive painting!
Of course, a handy Geiger is mandatory. |
If you want to get a good quantity of ore for extraction, at a reasonable price, contact Shannon and Sons Minerals, particularly Michael Shannon
himself (I can U2U his email address, I don't post anyone's personal email on a public forum). I got 2 kg of Radium King Mine uraninite (pitchblende)
from him for $100 with shipping.
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neptunium
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Where did you find this Careysub? I've look everywhere for this! Obviously not good enough ....
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careysub
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What, my extraction notes above?
From reading Curie's original publications. Look up "Radioactive Substances" and "The Discovery of Radium", both are available on-line.
See also:
https://www.aip.org/history/exhibits/curie/discover.htm
for a translation of the original radium discovery publication “Sur une nouvelle substance fortement radio-active, contenue dans la pechblende,”
Comptes rendus de l'Académie des Sciences, Paris, 1898 (26 December), vol. 127, pp. 1215-1217.
I have some journal articles on radium extraction that are too large to post here.
There are also old patents on radium extraction of interest.
[Edited on 24-6-2016 by careysub]
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neptunium
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Thats great ! And I read French....thanks Careysub!!
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bur
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careysub, thanks, that's really interesting reading.
I can also give a small update. I decided to at first extract the uranium and later recover the Ra from the sludge.
About 50 g Ore (forgot to weigh...) was crushed, 30% H2SO4 + 30% H2O2 were added, result was a greenish/yellow liquid. Addition of ammonia gave a
yellow/orange precipitate. Probably mainly U + Fe. Precipitate was dissolved in HNO3. To extract the U, I added a solution of 5% TBP
(tributylphosphate) in hexane. TBP is a very selective U ligand that makes a complex soluble in non-polar solvents.
Now for the first interesting result: The (UO2)(NO3)2(TBP)2/hexane solution has mild activity of about 0.2 µSv/h gamma ray measured 5 cm above
surface. Beta+gamma is about 0.8 µSv/h. Background is 0.1 µSv/h. I guess this is typical natural U.
But the aquaeous phase, holding the impurities showed this: 0.3 µSv/h gamma and 3 µSv/h beta. So there's a strong beta source in there and only weak
gamma. This could be Bi, Pb or Th. Pb-sulfate is not soluble. Also Bi and Pb 210/214 are both relatively strong gamma emitters. So I guess the
solution holds mostly Th-234/230.
I'm trying to figure out how the beta activity should behave over the next few days. Th-234 has 24 days half-life, decaying to U-234 with a large
half-life. So I should be able to detect how Th-234 decays.
What is a bit puzzling is Bismuth. It should be soluble in H2SO4 though I'm not sure how the H2O2 interferred. But if there was Bi-210/214 in there
the gamma activity should be higher. But maybe I can deduce this from measuring the beta-activity over time.
Bi-214 decays with 20 mins half-life. As none of the Po-218 mother nuclide should be present it will be gone by now having decayed (via µs Po-214
alpha emitter) to Pb-210. This is a beta-emitter with 20 years half-life making it fairly low active compared to Th-234 and Bi-210.
Bi-210 has 5 days half-life decaying to Po-210, which is a relatively stable (130 days) alpha emitter.
Bottom line: Now the solution should hold the beta-emitter Th-234 and (depending on whether or not Bi was extracted) Pb-210 and Bi-210. If it's just
Th-234 the decy curve should be more or less mono-exponential, otherwise I should see the 5 day half-life of Bi-210.
Does that make sense? I'll keep posting the beta/gamma activities, though unfortunately starting Monday as I'm not working on the weekend... 
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careysub
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Great to see some one starting on this! (I will in the by and by, someday hoping to do a pre-pub on this using thorium and uranium ores).
What mineral/ore type are you starting with?
Yes, you are doing exactly the right thing to track your separations, measuring the decay (and build up) of the short-lived child nuclides and
distinguishing between gamma and beta emissions.
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phlogiston
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Very interesting, thanks for sharing.
I was considering a similar project, it is really interesting to read how you are progressing.
Do you know the approximate mineralogical composition of your ore? Are you working on 50 g as a test sample?
In my attempt to find literature on the best conditions for the sulphate to carbonate conversion step I found this thesis helpful, it may be of interest to you.
Incidentally, it has a clear picture of 60 mg of pure radium sulphate on page 18. Ofcourse, it looks rather unremarkable, but imagine the crazy amount
of radiation that guy must have been dealing with to handle it.
[Edited on 12-8-2016 by phlogiston]
[Edited on 12-8-2016 by phlogiston]
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"If a rocket goes up, who cares where it comes down, that's not my concern said Wernher von Braun" - Tom Lehrer |
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The jersey rebel
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| Quote: Originally posted by bur | Has anyone ever tried to extract Radium?
I know the amounts are tiny, so I'm thinking of a Ra+-solution as the product. The extration to the point of a RaCl solution is not too hard:
Dissolution of U ore in H2SO4 leaves Ba,Ra and some other insoluble sulfates.
Most impurities are removed via NaOH and subsequent HCl.
Ba impurities remain in the sludge and the (Ba,Ra)SO4 is converted to (Ba,Ra)CO3 and dissolved in HCl.
unfortunately it's extremely difficult as radium compounds coprecipitate with barium salts. the only way i can think of is electrolysis under an inert
atmosphere at a negative pressure or in in the presence of sodium or something else that can readily react with chlorine without actually being in the
mixture. then the radium metal can react with HCl to make pure radium chloride
The only practical way to know if you were successful is from radiation though. As I don't have a gamma spectrometer available I'd have to rely on a
Geiger counter. My problem is, there are lots of other radioactive isotopes in the ore and I'm not sure if any of them might not be extracted along
the Radium. Of course their amounts are minute, but their activity isn't. So if the product is active it might be anything.
Especially the two Pb isotopes 210 and 214-Pb could end up with the Ba. I'd say separation of ng amounts of Pb from Ba might not be possible?
I thought I could add Ba at the last extraction step so I have something to precipitate. Then I'd end up with BaSO4 with a small amount of Ra
incorporated.
Long story short: Will I be able to separate the Ra from the other decay products? |
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The jersey rebel
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unfortunately it's extremely difficult as radium compounds coprecipitate with barium salts. the only way i can think of is electrolysis under an inert
atmosphere at a negative pressure or in in the presence of sodium or something else that can readily react with chlorine without actually being in the
mixture. then the radium metal can react with HCl to make pure radium chloride
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neptunium
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Even a gamma spectrometer won't help much. Trust me I've done it. Most of the heavier isotopes have few (if any) characteristic gamma or x rays lines
to be easily identify.
However, an alpha spectrometer (wich I have been searching for since 2014) would greatly help identifying most if not all the isotopes of the U and Th
decay chain... The 2 ortec alpha spectrometer on eBay are outrageously expensive for being sold as "for parts or not working" and missing the tray
holder AND more importantly the very precious detector!...which I have a few of 
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aga
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Hi bur.
Can you post some photos of your process, especially the residues and final results ?
If you have no hi-res video camera, just use your phone.
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unionised
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As a theoretical study it's an interesting bit of chemistry. I'm not sure it's legal and it's not very safe.
If you get the chemistry right it's relatively easy to separate Ra from most of the rest of the periodic table apart from barium.
You might as well make use of that by adding a little barium at the outset and extracting it back again. It will carry any Ra with it.
The insolubility of the sulphate is useful since most sulphates are soluble.
Essentially, if you precipitate sulphates from acid solution you have the alkaline earth metals and lead.
You can redissolve them by repeated treatment with NaCO3 solution to turn them into carbonates then redissolve them in HCl - that will leave a lot of
the PbCl2 behind.
Classical chemistry would remove the remaining lead as PbS
You might find it helpful to use the difference in solubility of barium and calcium chromates to remove calcium- which also has a fairly insoluble
sulphate.
IIRC lead chromate is soluble in dilute acetic acid but Ba chromate isn't- less smelly than ppt ing it as PbS.
Once you have a sulphate that is insoluble in water and was produced by adding dilute sulphuric acid to a chromate that wasn't soluble in dilute
acetic acid; then pretty much any the radioactivity is from radium
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Heavy Walter
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Hi Neptunium
About amateur alpha spectrometry, see this wonderful site:
http://physicsopenlab.org/2016/10/28/diy-alpha-spectrometry/
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neptunium
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Very interesting, I have the Amptek software because it runs the MCA . I've used this software before . I didn't know about the 7.2 version that
includes the alpha spectroscopy data.... Thanks a lot Heavy Walter! Precious info indeed!
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Heavy Walter
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Neptunium
A friend of mine is building one.
I will keep you updated.
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unionised
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Can you use the range in air as a measure of the energy?
The resolution would be awful- but the kit is cheap.
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Heavy Walter
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Hi unionised
You are right.
Range and energy are related to each other.
See setup from Melissinos'book:
Attachment: Alphas by Ion Chamber.docx (133kB)
This file has been downloaded 723 times
[Edited on 8-2-2017 by Heavy Walter]
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