Dear Madams/Sirs,
I would greatly appreciate receiving some info about the solubility in water at room temperature of MgCO3*2H2O (barringtonite) and 4MgCO3*Mg(OH)2*4H2O (hydromagnesite).
Many thanks!
Here is a table which contains the thermodynamics solubility equilibrium constants for both magnesium carbonate and hydroxides:
https://www.aqion.de/site/16
When you calculate the combined solubility, please take the autoprotolysis equilibrium of water into account.
Dear Jurgen, many thanks for your kind answer! Unfortunately, the list refers only to magnesite (anhydrous MgCO3), whose data are well known and are different from the ones of MgCO3.xH2O (x=2,3,5), which are more soluble than anhydrous MgCO3. The rarest data (those I am looking for) are for x=2.
In any case, many thanks again!
For hydromagnesite:
Article Hydromagnesite solubility product and growth kinetics in aqu...
A.P. Reverberi Whether a compound was previously hydrated or not makes a difference for the dissolution kinetics, but once it is in solution the thermodynamics parameter of solubility applies and that doesn't care where the ions came from. So, the solubility is the same, only the kinetics changes (although a tempered crystal may be so inert that you will not get to an equilibrium solution within a feasible experimental time).
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