Terri,
Thanks for forwarding this, and thanks to Kemlo for giving permission
to forward. Interesing.
Phil
>With permission from the email author - for your consideration.
>
>Thanks Kemlo!
>
>(makes sense of his email correction to the list of "hydroxide, not
>carbonate")
>
>
>-----Original Message-----
>From: Kemlo Rogerson [mailto:Kemlo.Rogerson@waht.swest.nhs.uk]
>Sent: Thu 9/20/2007 9:50 AM
>To: Johnson, Teri
>Subject: RE: [Histonet] NTMT woes
>
>Magnesium chloride is the name for the chemical compounds with the
>formulas MgCl2 and its various hydrates MgCl2(H2O)x. These salts are
>typical ionic halides, being highly soluble in water. The hydrated
>magnesium chloride can be extracted from brine or sea water. Anhydrous
>magnesium chloride is the principal precursor to magnesium metal, which
>is produced on a large scale.
>
>The most common magnesium carbonate forms are the anhydrous salt called
>magnesite (MgCO3) and the di, tri, and pentahydrates known as
>barringtonite (MgCO3*2H2O), nesquehonite (MgCO3*3H2O), and lansfordite
>(MgCO3*5H2O), respectively. Some basic forms such as artinite
>(MgCO3*Mg(OH)2*3H2O), hydromagnestite (4MgCO3*Mg(OH)2*4H2O), and
>dypingite (4MgCO3* Mg(OH)2*5H2O) also occur as minerals. Magnesite
>consists of white trigonal crystals. The anhydrous salt is practically
>insoluble in water, acetone, and ammonia. All forms of magnesium
>carbonate dissolve in acids. Magnesium carbonate crystallizes in the
>calcite structure wherein Mg2+ is surrounded by six oxygen atoms. The
>dihydrate has a triclinic structure, while the trihydrate has a
>monoclinic structure.
>
>Could it be there's a chemical reaction from chloride to carbonate with
>the subsequent falling out of solution? Isn't it called a double
>decomposition of a salt?
>
>Kemlo Rogerson
>Pathology Manager
>DD 01934 647057 or extension 3311
>Mob 07749 754194; Pager 07659 597107;
--
Philip Oshel
Microscopy Facility Supervisor
Biology Department
024C Brooks Hall
Central Michigan University
Mt. Pleasant, MI 48859
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