Posted by tealady on September 19, 2003, at 14:26:04
In reply to Re: NaCl, Epsom salts .. Lar? » tealady, posted by Larry Hoover on September 19, 2003, at 9:42:46
> The process of purification by forming crystals is called recrystallization.
OOPs. Well No chemistry here, except in Junior high school, which is why I wanted to run it by you.
I have not yet figured out how one tells which way a formulae goes..I know something to do with strength of bonds. I'm guessing their is no easy answer. OK, failed that one.> > >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.Thanks. I did think it tasted more like a sulphate than a chloride when I used more of the epsom salts..which is what one would expect given the above happens...
I read somewhere that Magnesium made a "salt" moist and they purposedly extracted the magnesium from our table salt due to this, perhaps not true..but I thought this may mean Mg may stay in the solution more easily, less likely to recrystallize ..some strange logic along those lines, so I thought their might be some sense in it....OK failed again <g>> Second, what is it about sulphate that troubles you?
Nothing, I think. Still confused aboout sulphate, sulphites, sulphurs, metabisulphate (ites), sulphur drugs and T3S etc..but thats' another story.
It's just not knowing WHAT I am doing, or taking, that troubles me <g>>
> 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.
>
> 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.
>
> You're welcome, though I'm trying hard to understand the chemistry you've presented (I'm a chemist, ya know).<g> I thought you might know a little about it
Thanks again, Jan
poster:tealady
thread:261436
URL: http://www.dr-bob.org/babble/alter/20030903/msgs/261666.html