MgCO3 + Oxalate Acid
= Magnesium Oxalate
What happens when
magnesium oxalate is placed in water ?
ANSWER ?
Magnesium Oxalate + Water = Carbon Dioxide + Brucite + Tritium Let's focus on the Bruucite
= magnesium hydroxide
= Mg ( OH) 2
The trick here is....
how to pull the magnesium hydroxide out of this aqueous solution
there's co2 + H3 ( tritium )
what i could not find out was...
if co2 gas is emitted and if H3 is emitted.
if they are... then, the remaining solution would be - magnesium hydroxide.
simple dryers could be employed to evaporate the water from the - mgo.
resulting in - mgo.
if one studies the process of - calcination vs dehydration to form = mgo.
calcination via furnace melt causes decomposition of other impurities.
resulting in... mgo.
VERSUS
aqueous magnesium hydroxide and the use of, dehydration - dryers.
Is there a difference in mgo ?
Is fired and decomposition via calcination a better mgo ?
or.. is dehydrating an aqueous magnesium hydroxide still the same ?
HERE'S A PAPER ON IT...
The mgo crystalization ( cubic ) still forms when magnesium hydroxide is dehydrated.
Go figure.
I would tend to think...
that high furnace heat could actually lose some of the mgo via decomposition.
while - dehydrating the mangesium hydroxide would lessen the loss.
might result in - more mgo content.
LINK - https://pubs.acs.org/doi/10.1021/j100027a033 Why even mention this ? Or shall we discuss a $100/mil furnace ?
wink.
This is perhaps a far cheaper method than...
furnace route. Catalyst reaction using acids.
To arrive at an mgo.
( with perhaps more mgo than using furnace method and perhaps bonus H3 )
-------------------------------------------------------------------------------------------------------------------------------------------
This eve...
i was also researching -
magnesium bicarbonate. sodium bicarbonate and magnesium bicarbonate are similar formulas.
each in this phase are
soluble. what is found online is-
once in a bicarbonate state and introduced to boiling water...
co2 off gasses.
Many... will exclude the tartaric acid from the - bicarbonate formula.
hence - they are only experimenting with - plain bicarbonates.
no acid in the mix.
Sodium Bicarbonate = has TartaricAcid in it's mixture.
Tartaric acid makes a whole lotta difference ( acid catalyst )
So... what now happens to a sodium bicarbonate with tartaric acid -
boiled ? Why did i choose boiled ?
It is not - electrolysis
But rather a new method of imparting hydrogen from an aqueous solution.
Solar panels that supply HEAT to boil water.
Steam reformation - sort of.
Sodium bicarbonate is NaHCO3
Tartaric acid is C4H6O6
So, the reaction is:
NaHCO3 + C4H6O6 + 2H2O(l) = 5CO2(g) + NaOH + 5H2(g)
Hydrogen is given off in a gas.
5 H2 gas ( hello )
But.. at the same time, there are
5 CO2 also given off.
What if one captured the co2 and reused it and combined it with the NaOH ( sodium hydroxide ) ?
NaOH + co2 = NaCO3
Right back to the original =
NaCO3 QUESTION - Could this be applied to - magnesium bicarbonate ?
i haven't come across any other using this - steam boiling - method to produce hydrogen
using a magnesium bicarbonate.
One would have to resort to - oxalate acid with mgco3
turn to magnesium hydroxide
then.. .dehydrate to form magnesium hydroxie
then introduce a co2to arrive at a magnesium bicarbonate
But... if we analyze the formula of, mgco3
there are 3 oxygens and 1 carbon ?
Is there another way of dropping the 3 oxygen and adding one carbon to arrive at,
bicarbonate ?