0
$\begingroup$

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?

Improve this question
$\endgroup$
1
  • $\begingroup$ 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. $\endgroup$
    – DrMoishe Pippik
    Dec 19, 2022 at 20:20

0

Reset to default

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service and acknowledge that you have read and understand our privacy policy and code of conduct.