LAST ONE...( lol )Was closing out research windows and i noticed one of the pdf's didn't open.
It's actually a good research paper.
Brines + Hardrock Carbonate using - oxalic acid.
The result shows that
oxalate precipitation .... following process by
carbonate precipitation process extracted
98.86% Mg, 73% Ca,
22.53% Li,
82.04% Al, 14.38% B, 12.50% K, 2.27% Na.
.... magnesite (MgCO3), calcium lithium aluminum (Al1.19 Ca1Li0.81), dolomite (CaCO3.MgCO3) appear in salt precipitated by oxalic acid.
LINK - https://www.google.com/url?sa=t&rct=j&q=&esrc=s&source=web&cd=&cad=rja&uact=8&ved=2ahUKEwikje31sc75AhWCJX0KHVL2CoAQFnoECAcQAQ&url=https%3A%2F%2Faip.scitation.org%2Fdoi%2Fpdf%2F10.1063%2F1.5038289&usg=AOvVaw0kd370Bb8JrF3G3hilJiAc
LOOK WHAT I FOUND..... Glad i kept researching - converting magnesium oxide with oxalate
I see -
2H20 ( deuterium )
Magnesium oxalate is an organic compound comprising a magnesium cation with a 2+ charge bonded to an oxalate anion. It has the chemical formula MgC2O4. Magnesium oxalate is a white solid that comes in two forms: an anhydrous form and a dihydrate form where two water molecules are complexed with the structure.
Related compounds: Magnesium Oxide
Chemical formula: MgC2O4; MgC2O4•2H2O ...
ONLY - 150 degrees C heat -
Synthesis and reactions
- Mg2+ + C2O42− → MgC2O4
A specific example of a synthesis would be mixing Mg(NO3)2 and KOH and then adding that solution to dimethyl oxalate, (COOCH3)2.[10]
When heated, magnesium oxalate will decompose. First, the dihydrate will decompose at 150 °C into the anhydrous form.
- MgC2O4•2H2O → MgC2O4 + 2 H2O
With additional heating the anhydrous form will decompose further into magnesium oxide and carbon oxides between 420 °C and 620 °C. First, carbon monoxide and magnesium carbonate form. The carbon monoxide then oxidizes to carbon dioxide, and the magnesium carbonate decomposes further to magnesium oxide and carbon dioxide.[8]