In my research I try to prepare trimagnesium dicitrate aqueous solution. Initially it stays clear, but after some time white insoluble precipitate is formed. Initial pH was about 4,5-5,0. If pH is lowered, there is less precipitate. But why? From solubility equation pH should be >8 to form Mg(OH)2 precipitate at the concentration I am using. Is there some other Mg compound formed?

  • $\begingroup$ It depends on concentration -- even at that pH, enough Mg(OH)2 might be forming that it cannot stay in solution. If it's open to air, also consider the carbonate; test by acidifying and look for CO2. $\endgroup$ Dec 19, 2022 at 20:20


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