Pissant
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 Posted: Fri Oct 10, 2008 7:46 am Post subject: Preperation of Magnesium Chloride from Magnesium Sulphate |
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Magnesium chloride has a large number of medicinal uses which have been
known for many years, but knowledge of the uses is not widespread.
Pierre Delbet, a surgeon, in 1915 on September 6, with Dr. Karalanopoulo, he
submitted to the French Academy of Science the paper Cytophylaxis,
advocating that magnesium increases the efficiency of the white blood cells.
His early findings have been greatly expanded on regarding the importance of
dietry magnesium in the two publications linked at the end of this posting.
See here.
http://www.arthritistrust.org/Articles/Magnesium%20Chloride%20Hexahydrate%20Therapy.pdf
You can buy magnesium chloride, or you can also very cheaply prepare it
yourself from magnesium sulphate (Epsom salts) and Sodium bicarbonate to
produce pure magnesium carbonate, which is then reacted with hydrochloric
acid to produce magnesium chloride. You can buy both of these salts in a
grocery store, or in a bulk goods shop for only a dollar two a kilo.
Hydrochloric acid you can buy cheaply from a swimming pool shop as it is
used for regulating the PH of swimming pools.
Process to prepare magnesium chloride.
Dissolve a quantity of Epsom salts, magnesium sulphate MgSO4 in distilled
water in a glass container or plastic bucket, NOT METAL. The process can be
scaled up or down, and the relative quantities can be readily deduced from
observing the reaction.
Add sodium bicarbonate (baking soda) NaHCO3 slowly. The mixture will
effervesce vigorously and two new substances will be formed. Magnesium
carbonate MgCO3 which is completely insoluble in water, will be precipitated
as a white powder that will eventually settle to the bottom of the reaction
vessel. The vigorous reaction will also splatter small particles of MGCO3
onto the walls of the containing vessel, so use a large container, and don>t
more than half fill it at the very most with the magnesium sulphate
solution. Sodium Sulphate (Glauber>s Salt) will also be formed. This is very
soluble in water, is non toxic and will be removed later by pouring off the
liquid after the magnesium carbonate has settled. A small amount left behind
as an impurity will have no adverse effect.
Keep slowly adding sodium bicarbonate as long as the reaction continues as
indicated by the effervescence. Stir the mixture with a glass or plastic
stirrer as you add the sodium bicarbonate. Add slowly until there is no more
effervescence, indicating all of the Magnesium sulphate has been used up in
the reaction.
Allow the mixture to settle and then pour off the liquid containing the
unwanted sodium sulphate and any excess sodium bicarbonate or magnesium
sulphate which will be dissolved.
This will leave a slurry of mainly magnesium carbonate. Add more clean water
(distilled water is best if your local water supply is chlorinated,
fluoridated of contains minerals) to wash the magnesium carbonate, allow to
settle and pour off the water with any dissolved residual salts. You will
now have almost pure magnesium carbonate.
You can now either filter the slurry through a filter paper (a coffee filter
and a funnel will do) and then dry the magnesium carbonate powder, or you
can proceed directly to reacting the slurry with hydrochloric acid. Drying
the powder will enable you to later more easily work out the strength of
your final magnesium chloride solution for dosage calculation.
In a class or plastic container, (NOT METAL) add enough distilled water to
the magnesium carbonate to well cover it, then slowly add hydrochloric acid,
stirring with a non metallic stirrer. Slowly add acid until effervescence
stops. Then add a very small amount of Magnesium carbonate, and see that it
DOES NOT EFFERVESCE, and remains undissolved, to prove that all of the
hydrochloric acid has reacted.
You now have a colourless solution of magnesium chloride.
To calculate the concentration of magnesium in the solution you will need to
know the weight of the magnesium carbonate you used and the amount of
distilled water and hydrochloric acid used. The method of doing this
involves calculating the molecular weights of the substances in the final
reaction and the quantities of water and acid used. I will post more details
on this when I work out an example, unless some chemist wants to do it
first.
The concentration of the solution can then be adjusted to give a standard
solution which has I suggest ten milligrams of magnesium per millilitre of
solution. This will be a suitable concentration for measuring dosage as
mentioned in the above linked reference.
See also, for information on the importance of dietry magnesium.
http://www.mgwater.com/Seelig/Magnesium-Deficiency-in-the-Pathogenesis-of-Disease/jacket.shtml
http://www.mgwater.com/rodtitle.shtml
Pissant from OZ
(Gullible idiot and candidate for the "Darwin Award", according to several
of the learned colleagues here. Perhaps they are of the type that insisted
that the earth was flat, and that Copernicus was a heretic in the middle
ages. So sure in their little bit of knowledge, their minds are made up, and
they refuse to be confused with facts!) |
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