Description of experiment
Below follows a plain text transcript of the selected experiment.
Needed compounds:
-----------------
sodium hydroxide : NaOH
hydrochloric acid : HCl
ferric chloride : FeCl3 . 6H2O
hydroxyl amine sulfate : (NH3OH)2 SO4
Class:
------
elem=Fe
coordination
redox
Summary:
--------
When an acidified solution of ferric chloride is mixed with a solution
of hydroxyl amine sulfate, then an almost colorless compound is formed,
but this compound does not seem to be an iron (II) compound.
Description:
------------
Add some solid hydroxyl amine sulfate to a solution of ferric chloride, which
is acidified with HCl in order to keep it clear (appr. 50 grams of FeCl3.6H2O
and 5 grams of HCl per liter): The yellow/brown liquid becomes almost
colorless (very light green) and remains clear. No gas is evolved.
Add an excess amount of a solution of NaOH: Formation of a brown precipitate
(iron (III) hydroxide?).
Remark: After the liquid has become almost colorless a green/grey precipitate
was expected on addition of NaOH-solution, due to formation of iron (II)
hydroxide. Was the almost colorless compound a coordination complex of iron
(III) or was this aqueous iron (II)?