1
$\begingroup$

Iron(II) sulfate (ferrous sulfate) is a salt that, in an aqueous solution, dissolves and yields $\ce{Fe^{2+}(aq)}$ and $\ce{SO4^{2-}(aq)}$. It then decomposes to ferric sulfate shortly thereafter.

But what happens to the iron(III) sulfate (ferric sulfate) in solution? Is the $\ce{Fe_2(SO_4)_3}$ compound preserved?

Improve this question
$\endgroup$
4
  • $\begingroup$ Fe2+ is oxidated by oxygen, Fe3+ can't be ox. this way. $\endgroup$
    – Mithoron
    Commented Aug 8, 2015 at 0:49
  • $\begingroup$ Are you asking whether the ferric sulphate dissociates in solution into separate ions? $\endgroup$
    – bon
    Commented Aug 8, 2015 at 17:33
  • $\begingroup$ @bon yes. Or maybe some kind of reaction takes place? $\endgroup$
    – Sparkler
    Commented Aug 8, 2015 at 18:06
  • $\begingroup$ Well hydrolysis may take place $\endgroup$
    – Mithoron
    Commented Aug 8, 2015 at 18:13

1 Answer 1

Reset to default
5
$\begingroup$

In aqueous solution $\ce{Fe2(SO4)3}$ dissociates into $\ce{Fe^{3+} (aq)}$ and $\ce{SO4^{2-} (aq)}$ ions. The sulphate ions will be solvated by hydrogen bonding with the water and the iron ions will form the hexaaquairon(III) complex, $\ce{[Fe(H2O)6]^{3+}}$.

As @Mithoron mentioned, the $\ce{Fe^{3+}}$ ions cannot easily be further oxidised so no additional reaction takes place.

Improve this answer
$\endgroup$

Your Answer

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

Not the answer you're looking for? Browse other questions tagged or ask your own question.