I have heard that magnesium and sodium hydroxide react to form an explosive mixture producing MgO, H2, and Na - I figured "yeah, whatever" thinking that it would be nearly impossible to recover any sodium.
However it is fairly do-able and especially at smaller amounts. I believe that we can find a way to very effectively improve the yield and the extraction process.
[youtube]http://www.youtube.com/watch?v=908rjHQ5mmc&feature=fvw[/youtube]
[youtube]http://www.youtube.com/watch?v=faorfmRkCv0&feature=channel[/youtube]
Any ideas on how to improve the yield?
Clearly mixing the reactants in a proper ratio, the better off you will be - excess NaOH will react with sodium at those temperatures. I would think excess magnesium would be highly desirable.
One other thing is if there could be a chemical one could mix with the NaOH and Mg to absorb a decent amount of the heat, it would prevent the reaction from being so violent. It is hard to think of anything that with sufficent heat would not react with Mg, NaOH, or Na. Perhaps the addition of finely ground carbon? A extremely high boiling point wax or oil? etc...
For extraction...
I think an effective method of extraction would be to grind the "ash" to a fine powder under mineral oil in a mortar & pestle than transferring that to a long tube in which heating and stirring can be performed. The heating will allow the sodium metal to form blobs and sink into the bottom while the other materials would stay as a powder and hopefully get suspended into the mineral oil.
Is there a solvent that is nonreactive towards sodium, has a density greater than sodium and a boiling point above the melting point of sodium? If so - that would be very useful.
The best thing that could ever happen would be to find a mixture of sodium and potassium hydroxide that has a lower melting point, and actually be able to melt the hydroxide mixture under a mineral oil solution than slowly add an excess of magnesium or even aluminum - which the guy from the video eludes to the idea that aluminum would be higher yielding in sodium.
To find an inert substance with a boiling point above 360*C sounds like a really really difficult task.
However -- hxxp://pubs.acs.org/doi/abs/10.1021/je60023a009#
If I am reading this correctly, a mixture of NaOH and KOH can produce a mixture that melts at 170*C - which means great things, since that is very much in the reach of some fancy solvent, I bet. What is the boiling point of wax?
Seems pretty easy!
The boiling point of paraffin oil is around 224*C.
Slowly adding the Mg while stirring ought to allow for some heat to form and be lost. It would be dangerous, you'd probably want to reflux the oil, and keep an eye on everything.
Off-topic but related: Does NaOH dissolve in things such as Ethylenediamine, liquid ammonia, etc? If so - perhaps slowly adding Mg or Al to that could be very useful.
However it is fairly do-able and especially at smaller amounts. I believe that we can find a way to very effectively improve the yield and the extraction process.
[youtube]http://www.youtube.com/watch?v=908rjHQ5mmc&feature=fvw[/youtube]
[youtube]http://www.youtube.com/watch?v=faorfmRkCv0&feature=channel[/youtube]
Any ideas on how to improve the yield?
Clearly mixing the reactants in a proper ratio, the better off you will be - excess NaOH will react with sodium at those temperatures. I would think excess magnesium would be highly desirable.
One other thing is if there could be a chemical one could mix with the NaOH and Mg to absorb a decent amount of the heat, it would prevent the reaction from being so violent. It is hard to think of anything that with sufficent heat would not react with Mg, NaOH, or Na. Perhaps the addition of finely ground carbon? A extremely high boiling point wax or oil? etc...
For extraction...
I think an effective method of extraction would be to grind the "ash" to a fine powder under mineral oil in a mortar & pestle than transferring that to a long tube in which heating and stirring can be performed. The heating will allow the sodium metal to form blobs and sink into the bottom while the other materials would stay as a powder and hopefully get suspended into the mineral oil.
Is there a solvent that is nonreactive towards sodium, has a density greater than sodium and a boiling point above the melting point of sodium? If so - that would be very useful.
The best thing that could ever happen would be to find a mixture of sodium and potassium hydroxide that has a lower melting point, and actually be able to melt the hydroxide mixture under a mineral oil solution than slowly add an excess of magnesium or even aluminum - which the guy from the video eludes to the idea that aluminum would be higher yielding in sodium.
To find an inert substance with a boiling point above 360*C sounds like a really really difficult task.
However -- hxxp://pubs.acs.org/doi/abs/10.1021/je60023a009#
If I am reading this correctly, a mixture of NaOH and KOH can produce a mixture that melts at 170*C - which means great things, since that is very much in the reach of some fancy solvent, I bet. What is the boiling point of wax?
Quote
The molten electrolyte for each experiment was a eutectic mixture of sodium and potassium hydroxides (51 mol % NaOH, 49 mol % KOH, Alfa Aesar). This eutectic has the benefit of a much lower melting temperature (170° C.) compared to the melting temperatures of pure sodium and potassium hydroxides (323° C. and 360° C., respectively).hxxp://www.faqs.org/patents/app/20090017345
Seems pretty easy!
The boiling point of paraffin oil is around 224*C.
Slowly adding the Mg while stirring ought to allow for some heat to form and be lost. It would be dangerous, you'd probably want to reflux the oil, and keep an eye on everything.
Off-topic but related: Does NaOH dissolve in things such as Ethylenediamine, liquid ammonia, etc? If so - perhaps slowly adding Mg or Al to that could be very useful.