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$\begingroup$ It seems not to address ferric ions hydrolysis, but hydration isomerism. Sure, you could formally replace NO3- by OH-. $\endgroup$
– Poutnik
Commented May 16, 2023 at 9:14
$\begingroup$ @Poutnik I couldn't find many sources regarding hydrolysis of ferric nitrate. I assumed it meant hydration of ferric nitrate. Sometimes the water of hydration does deprotonate and ligate as hydroxide. Could you help a little here? $\endgroup$
– ananta
Commented May 16, 2023 at 9:25
$\begingroup$ $\ce{[Fe(H2O)_{6-n}(OH)_n]^{3-n}(aq) + H2O(l) <=> [Fe(H2O)_{5-n}(OH)_{n+1}]^{2-n}(aq) + H3O+(aq)}$ for $n=0..2$ $\ce{2 [Fe(H2O)3(OH)3](aq) <=> [Fe(H2O)3(OH)2-O-Fe(H2O)3(OH)2](aq) + H2O(l)}$ and further condensation... // the actual mechanism is complex and particular structures may be guesses. there would be also multiple parallel ways of simultaneous hydrolysis and condensation. $\endgroup$
– Poutnik
Commented May 16, 2023 at 9:34
$\begingroup$ @Poutnik sorry for the bother, but could you provide a citation... I want to know the $\mathrm{pH}$ at which these reactions occur, and if at all, mixing $\ce{Fe(NO3)3}\cdot 9H2O$ would form hydroxide complexes at a neutral $\mathrm{pH}$. $\ce{HO-}$ is a weaker field ligand than $\ce{H2O}$. $\endgroup$
– ananta
Commented May 16, 2023 at 9:40
1

$\begingroup$ No cit. available. Ferric ion start to hydrolyze even near pH 3-4. Hydroxide reportedly coagulates at pH 4.5 // Try searching for ferric ion hydrolysis. I do not have access to paywalled articles. // sciencedirect.com/topics/earth-and-planetary-sciences/… // pubs.acs.org/doi/10.1021/jp980229p // pubs.acs.org/doi/10.1021/ja01324a018 $\endgroup$
– Poutnik
Commented May 16, 2023 at 10:00

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