Sciencemadness Discussion Board

Sodium Garbage Time And Unusual Results

m1tanker78 - 25-4-2011 at 09:31

First, let me explain what 'garbage time' or 'trash time' is. I normally reuse the electrolysis blocks 2 to 4 times before I chuck 'em and start over with fresh, clean ingredients. I normally limit the run times to 30 - 60 minutes. When I decide that the block will be discarded, I usually take around 30 minutes extra at the tail end to introduce different stuff to the melt or generally try something new which usually contaminates the block. This aptly earns the term 'garbage time'.

I did a 1 hour run this weekend + 1 hour GT. When garbage time came around, I replaced the anode with a 18/0 'stainless' fork but didn't leave it for very long. I began to see a yellow-green substance condense around the melt. I don't use a fume hood, only forced ventilation and was concerned about chrome toxicity.

After I replaced the anode, I introduced some small chunks of cinder block to the melt and let it brew for a little while. Of course, there isn't any set composition for cinder block; it's just a mixture of aggregate and (supposedly) ash.

I had some unusual difficulty coalescing the sodium that resulted (I included a video below). When the nugget cooled, it appeared to have a bluish-purple-gray color and moreover, it seemed to form a skin on the nugget. I've seen this skin effect with calcium contamination before but not that color! I haven't conducted any flame test or anything yet. I'm open to suggestions for determining impurities. With such a high MP, I don't see how chromium could be the culprit but can't rule it out just yet. Potassium and calcium seem like good candidates...

A shot of the nugget and the contrast it creates. The mass is 3.6g




This video demonstrates the slight difficulty I had coalescing the beads. They normally 'pop' together in a matter of 5 - 10 seconds with little or no need to guide them together. If you look closely toward the end, you can see impurities 'swimming' on the surface of the molten nugget. The black masses are normal; easy to remove. PLEASE RESERVE STUPID COMMENTS ABOUT CLEANLINESS AND "METH LAB" BULLSHIT. THANKS!

<iframe sandbox title="YouTube video player" width="640" height="510" src="http://www.youtube.com/embed/RAwca9B1BN4" frameborder="0" allowfullscreen></iframe>

Please share your thoughts (cinder block content, nugget color, chrome, etc.).

Tom

blogfast25 - 25-4-2011 at 09:43

What do you mean by 'electrolysis blocks'?

Any dirt on the surface of the nuggets will somewhat hinder their coalescence (I see that a lot with K too...) but this sodium seems to coalesce really just fine to me.

What's your electrolysis apparatus?

m1tanker78 - 25-4-2011 at 10:57

Blog, 'block' is a generic term I use for the solidified melt. I use an iron vessel for the crucible, steel cathode and carbon anode.

Tom

cyanureeves - 25-4-2011 at 11:12

m1tanker78 arent you the one who said your method of making sodium was ridiculously simple?how simple?how do you do it with cathode and anode?with a welding machine? do you zap a heap of sodium hydroxide?do you have a video of such process?have you seen the prices for sodium on that site nurd rage posted?you can make money even.

m1tanker78 - 25-4-2011 at 12:17

Quote: Originally posted by cyanureeves  
m1tanker78 arent you the one who said your method of making sodium was ridiculously simple?how simple?how do you do it with cathode and anode?with a welding machine? do you zap a heap of sodium hydroxide?do you have a video of such process?have you seen the prices for sodium on that site nurd rage posted?you can make money even.


I don't know what site you're talking about but I don't aim to sell it.

Tom

cyanureeves - 25-4-2011 at 15:47

wow! symboom posted a youtube video of sodium being made with what looks like a battery charger,two electrodes and molten sodium hydroxide. also posted a video of a humphrey davey using the servants quarters to do experimental lab work with potassium.very interesting and smart dude.

m1tanker78 - 25-4-2011 at 16:21

@cyanureeves: I'm fascinated with Davy's work. I know other scientists of that time did work with alkali metals but as far as I'm concerned, Davy is the patron saint of alkali metals. :D What I'd give to live in those times (temporarily) LOL.

I might publish some of my work here in the near future. It takes quite some time to condense notes, edit videos, etc just to have the discussion derail into personal attacks and such. For now, could someone kindly give me a simple procedure that I can use to test the nugget for chromium?

For example, can I cut a little piece off, put it in cold distilled water (to react Na/K/Ca). After reaction, acidify with HCl and possibly add a little H2O2 and look for a _______ tint?

Does this sound like a reasonable test? If so, what color would Cr(III)(?) produce in acidic solution? Some sources say amber, others say green. I know several members here have experience with Cr compounds so let's hear it! :D

Tom

plante1999 - 25-4-2011 at 16:35

ad it to melted naoh and than ad it to water you will get orange sol if Cr is present. if no.... i think you know...

cyanureeves - 25-4-2011 at 16:49

if its chromium it will turn bright canary yellow. i just did the method plante1999 did to extract chromate from nichrome wire using lead acetate and got a bright orange precipitate just as bright as sodiumdichromate. since your chromium is already mixed with sodium it probably will turn yellow as soon as you use hcl.but you forgot about iron because when i carbonated the acidic chromium/iron solution and back to acidic with vinegar i got a purple solution. youtubers bad mouth alot about drug manufacture and appearaces,but probably not here.

bob800 - 25-4-2011 at 16:51

Quote: Originally posted by cyanureeves  
wow! symboom posted a youtube video of sodium being made with what looks like a battery charger,two electrodes and molten sodium hydroxide. also posted a video of a humphrey davey using the servants quarters to do experimental lab work with potassium.very interesting and smart dude.


Where are these videos??

cyanureeves - 25-4-2011 at 17:01

@ bob800 right here, right now. second page under sodium by electrolysis.

m1tanker78 - 25-4-2011 at 17:09

bob800, http://www.youtube.com/results?search_query=molten+sodium+el...

Tom

blogfast25 - 26-4-2011 at 04:43

I don’t see any videos signed ‘synboom’.

Tanker78, your search for chromium may just be a wild goose chase.

Here’s a tentative explanation for the brown film: thin layer diffraction. It’s very common on the surfaces on many transition metals where an oxide layer of only a few molecules thickness can cause all sorts of colourful effects to appear, much like a thin film of petrol on a puddle of water does. Nb, W, Mn, V and Ti have all shown this property to me.

Now, Na isn’t a hard transition metal of course but an unusually obtained film of Na oxide/superoxide might still generate unusual colours.

Just an idea…

Alternatively, just peel that ‘potato’, dissolve the 'peel' in water (add HCl for water insolubles) and test for chromium: it’s easy to do


[Edited on 26-4-2011 by blogfast25]

m1tanker78 - 26-4-2011 at 05:27

I cut a small piece of sodium in question and dropped it in dilute HCl. Most of it shot out (as expected). I reset and dropped another small piece in cold distilled water. After it got done skimming around, I acidified with HCl. There may have been a hint of yellow (but it could have been the HCl, itself. After an hour or so, I added a little bit of H2O2 to the solution. No strange color changes.

**************

The inside of the nugget is most definitely contaminated with something. A cross section where I sliced it revealed a dark(er) substance in the center. This I've never seen with pure Na or even low potassium NaK alloy...






Any suggestions??


**************

Blog and others, the videos that are being talked about don't belong to symboom. He posted links to them in another thread. The videos depict the author(s) electrolyzing molten NaOH.

Tom

blogfast25 - 26-4-2011 at 06:14

Tanker78:

Trying to dissolve Na in even dilute HCl isn’t clever: the metal needs to be tamed, not irritated, don’t play with the dragon’s tail!! Alcohol or methanol is actually a better solvent for analytical work on Na metal. Then add water or HCl to dissolve the insoluble bits. Or evaporate the alcohol and dissolve the obtained Na ethoxide (or methoxide) in water, which will almost completely hydrolyse it to NaOH + alcohol. The colour of the alkoxide residue alone should be telling (Na alkoxides are white)…

Seems to me your colour was simply surface oxide: people have reported all kinds of colours for oxidising sodium.

Suggestions? Not to worry so much! That spec could be a vacuole or a minor solid contaminant caught in the sodium close to melting point. Your metal seems of very good quality on the whole, so when are you going to show the set up?

m1tanker78 - 26-4-2011 at 07:43

Blog, the spec could be a gnat that fell in the oil for all I know. :D

I was talking about the dark patch around the speck. This was visible just as soon as I sliced the nugget. That isn't normally seen in pure samples of alkali metals or alloys. I'm not too hung up on it, just a little curious about it. The crystallization pattern is also way off the mark.

These photos show a comparison of what pure sodium (different nugget than above) looks like after being cut and after the crystallization patterns become visible...







==================

Any ideas concerning the cinder block content?

m1tanker78 - 26-4-2011 at 14:30

Quote:
Alcohol or methanol is actually a better solvent for analytical work on Na metal.


Would 91% IPA be good enough for this?

m1tanker78 - 26-4-2011 at 22:30

I put a small piece from the sodium nugget in question into 91% IPA. After the reaction was complete, there were 3 layers. The bottom layer turned yellow and has some small black specks in it...





I included the video of the reaction here in case anyone would like to watch it...

<iframe sandbox title="YouTube video player" width="640" height="510" src="http://www.youtube.com/embed/As2TKGtRQRc?rel=0" frameborder="0" allowfullscreen></iframe>


I'm not too concerned with the black specks - probably carbon. What is the middle layer and what should I make of the yellow stuff?

cyanureeves - 27-4-2011 at 04:22

ha!one of the neatest thing ever. it looks like naplam falling from the sky. the solid would be sodium something?is that a so called ethoxide solution?it looks like something separated from water.was the mist cold?how about the solution?your yellow stuff looks pretty concentrated too and not so much like a tincture.

unionised - 27-4-2011 at 04:36

I'm not sure about the 3 layers but sodium hydroxide solution does not mix with IPA and wet IPA may not mix with some hydrocarbon oils.
Had the Na been kept in oil?

blogfast25 - 27-4-2011 at 06:42

In all likelihood the formed sodium isopropoxide (sodium 2-methylpropoxide) is ‘salting out’ the 91 % IPA, that is: it’s driving out the water, explaining the layers. At the same time the isopropoxide is hydrolysing to NaOH due to the water. It’s also possible that the sodium is reacting preferentially with the water, thus forming NaOH (which then salts out the IPA). Pure IPA isn't soluble in water with high salts contents...

To answer your previous question about the suitability of 91% IPA, in short; ‘NO!’

But you can repeat the experiment in a meaningful way as follows: look up ‘salting out IPA’ (or similar terms): there are plenty web pages that detail how to convert 91% IPA to almost 100% IPA by adding lots and lots of NaCl to it. The salt ‘pulls’ out the water leaving you, after filtering usually, with quite pure isopropyl alcohol.

Next, instead of dunking a whole nugget into the alcohol, cut a neat piece, totally free of skin and protective oil and see how it reacts and whether you’re getting a clean, clear solution of sodium isopropoxide in IPA. Any oil would probably emulsify into the alcohol, creating deceptive results…

Alternatively, use any dry alcohol: methyl, ethyl, propyl…

Salting out IPA:

http://www.instructables.com/id/How-to-Salt-Out/

[Edited on 27-4-2011 by blogfast25]

m1tanker78 - 27-4-2011 at 12:45

Thanks Blog, I'll repeat the experiment with some [almost] dry IPA.

FYI, this particular nugget was mostly free of the superficial crust. The reason it's rounded is because I remelted it in some heavy oil. I made every effort to manually remove the oil from it but a little undoubtedly transferred to the IPA.

cyanureeves, I'm blind and lost when it comes to organics so maybe another member can answer your question. My belief is that the white flakes were (mostly) NaOH which settled at the bottom then pulled water from the IPA. It didn't take them long to dissolve and form an aqueous layer.

+++++++++++++++++++++

EDIT: I'm a little confused. The questionable nugget is now silvery-white (was purplish). It still shows a darker band in the cross section. The bottom most layer of the IPA sol'n is fading from yellow to crystal clear and a white satin-like substance is dropping out in what was the middle layer. *SIGH*.....

Here's what the nugget looks like now. It's the one that's been cut:



Tank

[Edited on 4-28-2011 by m1tanker78]

blogfast25 - 28-4-2011 at 03:30

It points to my hypothesis that this is a purely superficial phenomenon, involving a surface oxide layer that's changing in thickness and composition. I really wouldn't worry about it too much: I've seen far, far worse looking sodium.

The alcohol-to-alkoxide (alt. alcoholate) test is more significant IMHO because it tells you something about the bulk of the metal, if properly executed.

cyanureeves - 29-4-2011 at 14:41

yipee! i made sodium today. i charged my piece of crap 12v black and decker weed wacker battery pack and hooked it to two pieces of welging rods held by clothes pins,pour some sodium hydroxide,warmed it and the current kept it molten.little bb's kept forming but i couldn't scoop them out because i was too excited so they just blended back into the unmelted portion. i did scoop up some bb's and dropped them in oil but a good many just went back into the puddle also.what becomes of the poor lost little bb's?do they turn back into sodium hydroxide?i hope so because i'm using the same melt over again.some bb's were cover in the hydroxide and when i dropped them in water they would only fizz but when i squished them,then they would do the sodium dance on the surface. time to invest in a battery charger! hey, would that green draino work? it has salt,sodium nitrate,sodium hydroxide and aluminum.

m1tanker78 - 29-4-2011 at 15:53

Quote: Originally posted by cyanureeves  
yipee! i made sodium today.[...]


First of all, if you intend to go down the sodium hydroxide road then len1's work is required reading. Those threads should answer all your questions.

Let me add that if you're going to spend the bucks on a 12V battery charger, you might want to consider buying a cheap DC inverter welder with adjustable current setting instead. The main thing to look for in any case is the DUTY CYCLE. A cheap welder will probably provide more juice at 100% duty cycle; something to consider.

NaOH has it's advantages but I quit NaOH because it's expensive (relatively), it's very hygroscopic (think about it - hard to reuse!), it's very harsh for certain electrodes, it produces caustic fumes, it spits and splatters a lot, IIRC it requires a cell separator for decent efficiency. There's also a very finite temperature window - 10*C IIRC. Under that, little or no sodium. Over, Na diffuses back into the melt.

If you get it going then post up some alkali metal porn. :D

blogfast25 - 30-4-2011 at 05:00

Quote: Originally posted by cyanureeves  
hey, would that green draino work? it has salt,sodium nitrate,sodium hydroxide and aluminum.


No and it's an accident waiting to happen: molten NaOH reacts almost violently with aluminium. To spice things up, you've got a strong oxidiser in there: NaNO3!

NaOH + 2/3 Al --- > Na + 1/3 Al2O3 + 1/2 H2
NaNO3 + 2 Al --- > Na + 1/2 N2 + Al2O3.

Check out the standard heat of formation of Al2O3 to predict end result! :mad:

[Edited on 30-4-2011 by blogfast25]

cyanureeves - 30-4-2011 at 05:32

blogfast25 i wont do it then. besides i saw flames when some of the sodium popped at the anode and i dont like the toxic fumes tanker talked about either.

blogfast25 - 30-4-2011 at 12:33

Yes, stay well clear: molten caustic soda is dangerous enough, w/o Al or nitrate in the mix...

Try providing an argon blanket: use welding gas (but not Ar/CO2 mix!) and get a gentle flux to cover the surface of the melt and electrodes. Depriving sodium of air oxygen prevents it from oxidising...

m1tanker78 - 30-4-2011 at 17:03

91% IPA Experiment Update:

All of the remaining IPA has evaporated, leaving only the bottom aqueous(?) layer. It has the strong, skunky odor of the heavy oil I used to melt the sodium nugget prior to the experiment. I suppose that accounts for the yellow color I observed at the bottom. In spite of practically scrubbing the nugget with a paper towel, a little bit of the oil still stuck to it! This is the final nail in the coffin of the heavy oil I experimented with. Good riddance!

Tom

blogfast25 - 1-5-2011 at 05:49

For storage, a clean, clear kerosene or unadulterated paraffin oil is really the best with both Na and K.

m1tanker78 - 6-5-2011 at 11:29

I was digging around in the can where I kept the original junk from the cinder block/chrome GT and came across another unusual find. I removed a few 'sodium' beads and placed them in clean(er) mineral oil. Some of the beads retained a red tint in various shades. Purple sodium (original post) was weird enough but red?

Ascending intensity of red beginning at the 12 o'clock position with 4 o'clock being the most intense...


Has anyone here seen sodium superoxide (NaO2) up close? I'm not saying that these beads are covered with NaO2. I'm curious about the claims of it being "yellow-orange". I've never seen any practical references for it and I can't find a single 'real life' image for it.

Tank

m1tanker78 - 7-5-2011 at 11:09

I made another sodium nugget only this time, I didn't contaminate the bath with anything so the new nugget is as close to 100% Na as it gets. For coalescing, I used approximately the same volume of oil and heated approximately to the same temperature and length of time as I did for the prior nugget in question. Upon cooling, I was surprised to see the surface slowly change from a mirror finish to a semi-matte violet then bluish violet. I suspect that after a day or two, it'll settle at silvery-white like the original.

New sodium nugget at forefront, prior questionable nugget just behind on the left...


ASSUMPTIONS: The higher heat and longer length of heating caused the sodium metal to 'anneal' which sort of explains the weird colors and above all, the unusual crystallization patterns in the cross section. BlogFast nailed it but I wanted to find out specifically what oxides and why. I'm still puzzled with the red colored sodium in my previous post. Seems like a large disparity in light diffraction to only be one compound.

So far, I've seen plenty of bluish coloring and not so much red. The spectral extremes seem to be blue and red. A fine dispersion of the two will obviously appear to be violet/purple in differing shades which I've also seen. For now, I can only assume that the blue hue is seen because of sodium oxide and the red hue is possibly sodium superoxide. Sodium peroxide is light yellow; a pretty well known fact and one I've seen myself.

Tank

blogfast25 - 7-5-2011 at 12:17

Quote: Originally posted by m1tanker78  
BlogFast nailed it but I wanted to find out specifically what oxides and why. I'm still puzzled with the red colored sodium in my previous post. Seems like a large disparity in light diffraction to only be one compound.

So far, I've seen plenty of bluish coloring and not so much red. The spectral extremes seem to be blue and red. A fine dispersion of the two will obviously appear to be violet/purple in differing shades which I've also seen. For now, I can only assume that the blue hue is seen because of sodium oxide and the red hue is possibly sodium superoxide. Sodium peroxide is light yellow; a pretty well known fact and one I've seen myself.

Tank

m1tanker78 - 7-5-2011 at 12:21

Addendum to my red sodium post above:

From Wiki -
Quote:
"Ozonide is an unstable, reactive polyatomic anion O3−, derived from ozone, or an organic compound similar to organic peroxide"
[...]
"Inorganic ozonides[1] are dark red ionic compounds"


Link to the brief wiki entry: http://en.wikipedia.org/wiki/Ozonide

Seems highly unlikely given the conditions required to form as well as the low temperature decomposition and general reported instability. I don't know what else to think. Here's a list of oxidation states and observed or reported colors pertaining to sodium:

Na2O - Sodium Oxide - silvery white (possibly bluish tint)
Na2O2 - Sodium Peroxide - light yellow (appears [off]white in certain lighting)
NaO2 - Sodium Superoxide - "yellow-orange"
NaO3 - Sodium Ozonide - "dark red"

?????

Tank

blogfast25 - 7-5-2011 at 12:26

Hmm, the different coulours, assuming I'm more or less right right that thin layer diffraction (TLD) is causing the various colours is much more to do with the oxide thickness than with the type of oxide. The red may also be caused by TLD, e.g. a bit of mineral oil forming a very thin layer.

For the kind of strange colouring effect that oxide layers can cause metals to TLD, see examples here (scroll down):

http://periodictable.com/Elements/041/index.html

Niobium metal can be given almost any colour by means of this layer anodisation.

I doubt if you're seeing superoxides, they take time to build...

m1tanker78 - 1-6-2011 at 16:17

Returning to my sodium in IPA experiment...

After roughly a month, I noticed that all of the liquid was gone so I broke up and scooped out the crystals. I've been researching their composition but came up with more questions than answers (as usual). I hit a dead end in my search and I know how much you all love puzzles. [/sarcasm] Seriously though, I'd appreciate any leads on this.

The crystals don't melt or decompose when heated to cherry red. They turn white after strong heating. They don't seem to have any water trapped in their structure and don't exhibit signs of being hygroscopic. I don't see how the crystals could be Na-alkoxide (low MP, 'violent' reaction with moisture). One thing I'm sure of after a flame test is that it's a sodium compound. It definitely isn't NaOH.

Virgin crystals as removed from the vessel:


Small sample after strong heating:


Tank

ScienceSquirrel - 1-6-2011 at 16:41

That looks like sodium carbonate to me.
Sodium hydroxide and alkoxides absorb carbon dioxide from the air to form sodium carbonate, bicarbonate, sesquicarbonate, etc as various hydrates depending on conditions.
Try adding a few drops of acid to some of the solid, I bet it fizzes.

Neil - 1-6-2011 at 16:52

Did you weigh the glass reaction vessel before and after? Perhaps silicates? Was that red heat taken inside in the shade or outside under full sun?

[Edited on 2-6-2011 by Neil]

m1tanker78 - 1-6-2011 at 17:10

Quote: Originally posted by ScienceSquirrel  
That looks like sodium carbonate to me.
Sodium hydroxide and alkoxides absorb carbon dioxide from the air to form sodium carbonate, bicarbonate, sesquicarbonate, etc as various hydrates depending on conditions.
Try adding a few drops of acid to some of the solid, I bet it fizzes.


I put a couple of drops of conc HCl on some of the crystals and it fizzes like crazy. I initially dismissed the carbonate because it's very hygroscopic but for whatever reason, these crystals remained [mostly] anhydrous. Thanks!

Neil, the glass wasn't attacked if that's what you meant.

Tank

ScienceSquirrel - 2-6-2011 at 02:38

Sodium carbonate is not hygroscopic at normal humidities.
The decahydrate and heptahydrate are quite stable in air and crystalline but will effloresce to form the monohydrate which will form the anhydrous salt on heating. The monohydrate and anhydrous salt are both white powders.

m1tanker78 - 7-6-2011 at 07:03

Quote: Originally posted by blogfast25  
In all likelihood the formed sodium isopropoxide (sodium 2-methylpropoxide) is ‘salting out’ the 91 % IPA, that is: it’s driving out the water, explaining the layers. At the same time the isopropoxide is hydrolysing to NaOH due to the water. It’s also possible that the sodium is reacting preferentially with the water, thus forming NaOH (which then salts out the IPA). Pure IPA isn't soluble in water with high salts contents...

To answer your previous question about the suitability of 91% IPA, in short; ‘NO!’

But you can repeat the experiment in a meaningful way as follows: look up ‘salting out IPA’ (or similar terms): there are plenty web pages that detail how to convert 91% IPA to almost 100% IPA by adding lots and lots of NaCl to it. The salt ‘pulls’ out the water leaving you, after filtering usually, with quite pure isopropyl alcohol.

Next, instead of dunking a whole nugget into the alcohol, cut a neat piece, totally free of skin and protective oil and see how it reacts and whether you’re getting a clean, clear solution of sodium isopropoxide in IPA. Any oil would probably emulsify into the alcohol, creating deceptive results…

Alternatively, use any dry alcohol: methyl, ethyl, propyl…

Salting out IPA:

http://www.instructables.com/id/How-to-Salt-Out/

[Edited on 27-4-2011 by blogfast25]


I got my hands on some pure methyl alcohol so I went ahead with blogfast's suggestion. The result was very different from the original sodium in 91% IPA experiment. I cut 2 slivers from the same sodium nugget as before and used the 2nd sliver to eliminate as much 'face' contamination as possible. I removed virtually all of the oil manually (no solvent rinse) then cut away the outer perimeter. In the process of doing all of this, the sodium sliver oxidized some but without argon, there's nothing I could have done to prevent it. I'd like to think it was [at least] clean oxidation. Anyway,

2 CH3OH + 2 Na > 2 CH3ONa + H2

I believe that's the correct notation for the reaction. I observed the following differences compared to the previous:

1. A little less vigor of reaction.
2. Less white flakes sinking to the bottom.
3. No layering in the liquid during nor after rxn.
4. A few tiny white specks remained undissolved (sodium oxide?)
5. The liquid was, and remains, perfectly clear.
Quote: Originally posted by unionised  
I'm not sure about the 3 layers but sodium hydroxide solution does not mix with IPA and wet IPA may not mix with some hydrocarbon oils.

The lack of layering in this experiment seems to reinforce what unionised and blogfast stated about solubilities. This time around, there simply wasn't any water in the methanol to screw up solubilities.

I'm thinking of separating the remaining methoxide solution into 3 or 4 smaller samples for further analysis to check for impurities. I don't care much about the impurities, themselves. I believe that isolating them would be 85% of the fun. :D

Here's the video clip of the reaction...

<iframe sandbox width="480" height="390" src="http://www.youtube.com/embed/idepSOh0A3c?rel=0" frameborder="0" allowfullscreen></iframe>

Tank

blogfast25 - 7-6-2011 at 08:27

Nice, clean, crisp reaction Tank. Your sodium is fairly pure by the looks of it: no inclusions and such like. Of course actual purity can not be established only this way but its very encouraging, I'd say.