Posted by Larry Hoover on September 19, 2003, at 9:42:46
In reply to Re: NaCl, Epsom salts .. Lar?, posted by tealady on September 19, 2003, at 7:23:29
> Hi Lar,
> Your back! Gee your posting early...or not asleep yet?Just got up. Last night, when I arrived home, I was stunned from the brutal truck driving regime.
> >> Leave as a solution and just use a couple of drops at a time instead of salt, say in oatmeal, or on steak..that's been heaps for me!
>
> >> I also use the epsom salts in baths.
>
> >I'm glad I didn't reply when I first read your post. I was too tired to catch that you were recrystallizing the salt.> I wasn't. I shouldn't have added that comment I guess. I was just giving another use for the packet of epsom salts I buy to start with
The process of purification by forming crystals is called recrystallization.
> >Frankly, I have no idea if it will work. You may be leaving the magnesium behind just as much as you are sulphate ions. Or, you may not be doing either, as all the ions are readily soluble.
>
> Oh, this was the idea, I got from a chemist. But I was uncertain whether I was getting the sulphate or not. You wouldn't want to take too much if you couldn't be sure you were getting rid of the sodium sulphate.Two things. Sodium ions, chloride ions, magnesium ions, and sulphate ions, are all very soluble in water. To precipitate out a particular salt, you have to use a different process than you're using.
Second, what is it about sulphate that troubles you?
> 8 teaspoons of magnesium sulphate (Epsom Salt) to four teaspoons of sodium chloride . ie in the ratio (by weight) 2:1, although the requirement is for twice as many sodium atoms as magnesium - the chemistry works out a bit odd, but is OK.
> Magnesium Sulphate + 2xSodium Chloride=Magnesium Chloride+ Sodium Sulphate
> 246 grams 2 x 58 grams 95 grams+(126 grams H2O)+142 grams
> this doesn't balance without the water that comes with Epsom Salt (this amounts to another 126 grams and would show up on the right hand side of the equation.In solution, however, there is no association of ions. You've merely created a binary solution. A salty (sodium chloride salty) solution of magnesium sulphate.
> Cool the concentrated solution of the two salts then place the cold liquid in a freezer at below - 4 degrees Celsius. This should cause the sodium sulphate to crystallize out (a bit jelly like but it is OK).
But sodium sulphate is equally soluble to the other salts. I can't see how this would work.
> Filter the cold solution through anything clean and fine meshed (coffee filter paper?). (I used a clean piece of an old laddered stocking)
> The solution of mostly magnesium chloride can be re-frozen and strained (twice)to separate out some more sodium sulphate .
> My first go (last year), I tried it the other way around ( 4 spons NaCl to 2 spoomns Epsom salts), and it came out OK, very saltytaste. Still good as a replacement salt.
> My last go I used the above (8 spoons Epsoms salts to 2 spoons NaCl)and I think I had a some sulphate left in.
> So I was thinking of just trying for a Na, Mg salt mix again..maybe reversing again or equal spoons of each and using that as a salt replacement.Find the bluedog thread again, and go to the list of other postings that are at the bottom of the page. One of the bluedog post just above the one you quoted has the name of the chemical supplier for IV grade mag chloride. All the stoichiometry (the proportions) for the solution(s) is given in the thread, as well.
> >What makes the idea of using a solution so useful is that the dose is infinitely variable, once you have the concentration of the solution worked out.
>
> Well it was good to use as a condiment. Just not completely certain it works,
> I thought some others might be interested if it did work. Perhaps not if it may leave some sulphate in.Again, what's up with the sulphate concern?
> I definitely felt like I was getting some magnesium this way.....even if I was getting some sulphate as well.
>
> Thanks Lar, JanYou're welcome, though I'm trying hard to understand the chemistry you've presented (I'm a chemist, ya know).
Lar
poster:Larry Hoover
thread:261436
URL: http://www.dr-bob.org/babble/alter/20030903/msgs/261591.html