I was hoping for some advice regarding potentiometry. I am working with ternary complexes of Cu(II) involving bidentate N-donor and O-donor ligands. I want to do potentiometric (pH-metric) titartions in order to determine stability constants as well as do speciation. The problem I have is that I have a decomposition of my O-donor ligand, as a result of a Cu(II) assisted hydration and oxidation, which takes place above a certain pH. I know what the decomposition product is as I have managed to crystallize it.
So my question is, is there a way of including this oxidation step in the interpretation of the potentiometric titration curves or is it simply going to be a nightmare to do speciation when both acid-base reactions and redox reactions are taking place. Also, a side product of the decomposition of the ligand is CO2, will this significantly affect the results in terms of H2CO3.
Any advise will be appreciated.
Thank you.
I do not have direct experience with this type of system, however I would recommend delving into the primary literature. If your ligands are known, then others may have experienced something similar so that you will not "reinvent the wheel" with your work. Try SciFinder Scholar and ISI Web of Knowledge as good entry points. Science librarians are experts at assisting one to dig into the literature, so if you have such librarians, they might be able to help.
Using the potentiometric (pH-metric, or acid base) titRAtion is designed to determine pKa values. Only protonation/deprotonation should take place in your system. Otherwise, the interpretation is very complex. "but determine stability constants as well as do speciation." "Speciation" is a very vague term. Basically, it means a composition of a solution depending on a certain parameter (pH, electrochemical solution potential, concentrations, etc).
https://www.researchgate.net/post/How_can_I_get_free_access_to_SciFinder_Scholar3
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