Can iron react with other inorganic substances and form a red precipitate?

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Iron can react with inorganic substances like KNO3 and Fe(SCN)3 to form a red precipitate, specifically Fe2(SO4)3, when combined with Na2SO4. The discussion also explores the potential reaction with NaOH, suggesting that while NaOH may not effectively precipitate KSCN, it could be used in other reactions. The user is seeking advice on how to precipitate thiocyanate ions from an aqueous solution of NaNO3 and KSCN. The conversation highlights the complexities of these chemical interactions and the challenges in isolating specific compounds. Overall, the discussion emphasizes the feasibility of these reactions while addressing the limitations of certain precipitating agents.
alotropia_entropia
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I'm with a small doubt let me show for you:

I have a solution:
KNO3 + Fe(SCN)3

Plus:
Na2SO4 (aq)

I would like to know if could happen it?

---> NaNO3 + FeSO4↓ppt red + KSCN

Or plus:

NaOH (aq)

Could Happen ?
----> NaNO3+ Fe(OH)3 ↓ppt red +KSCN

Thank you

Paulo
 
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Yes, it happened : But
6KNO3+ 2Fe(SCN)3+ 3Na2SO4---->Fe2(SO4)3 ↓ppt red + 6KSCN (aq) + 6 NaNO3 (aq)

Now I want to know how precipitate the [SCN] from aqueous solution NaNO3 + KSCN

Could anyone help me?
Thanks
 
Maybe it could being done add NaOH (aq)?
 
NaOH isn't good to precipitate KSCN ... the KSCN is unsoluble into etanol but is a bit expansive...until now
 
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TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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