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how can remove chloride from ferric chloride? Answered

First i dissolved iron ore with Hcl and then i filtered it and then i  titrated that filtrate  with NaoH then i got precipitated iron ore solids by filter that solution, but more than 10% chlorides are present in that solids, so can any body tell how to remove that chlorides from that solids ?


I dunno, there's lots of stuff to try.

Maybe wash the solids you've got with water a few times. I would expect almost any chloride to be soluble in water. In contrast I would expect iron oxides and hydroxides to be insoluble in water.

A slight excess of base during the titration step might help. I mean increasing the concentration of OH-, should drive

M+n + n OH- = M(OH)n

to the left, towards more M(OH)n.

Bubbling air through it might help, during the step when it is ore dissolved in aqueous HCl. Guessing the O2 to in the air might help form some oxides directly. Also the air bubbles ?might? be able to carry away some HCl(g) in gas phase. I mean if that trick actually worked, it would be neat, since air is so much cheaper than NaOH.

Thank you Mr. Jack for your valuable feed back, i washed many times but even though i am getting 10% cl in that solids, and sorry i couldnt understand that air bubble metod so can u pls establish that method....

So you have insoluble chlorides. Wow! I wonder what they are.
I mean there are just a few of them, I think, Ag+, Pb2+, Cu+ and (Hg2)2+

Whatever they are, it seems like those should have come out in an earlier step. Like right after mixing the ore with HCl, the insoluble chlorides should have come out, or not dissolved in the first place.

Maybe the HCl acid used for that step was too strong? In the Wikipedia article for "Qualitative inorganic analysis"


I found this,

1st analytical group of cations consists of ions that form insoluble chlorides. As such, the group reagent to separate them is hydrochloric acid, usually used at a concentration of 1–2 M. Concentrated HCl must not be used, because it forms a soluble complex ion ([PbCl4]2−) with Pb2+. Consequently the Pb2+ ion would go undetected.

I added the bold in that quote.

Regarding this idea of bubbling air through the mixture, that was just a very wild guess. I was just trying to think if there was a cheaper way to remove Cl- ions from a solution. I mean cheaper than neutralizing it with NaOH, and washing out the NaCl.

By the way, how do you know your final product has more than 10% chlorides? I mean there is some sort of testing that determines this. Is it a test you did, or do you send a sample to some other lab, and then they tell you what was in the sample you gave them.

Also BTW, what is the goal here? I am guessing the goal here is to take "dirty" iron ore, and make it into pure iron ore, just iron oxides or hydroxides, by separating out the other metals. Erm, right?

There might be books on this subject, like,



Moles == ?

Gota love, or loathe, High school chemistry :D

Provided you use a chemical resistant tank, the O2 will totally help it along !

I Remember back in highschool electronics we did the same when we etched PCB's Ironically like Icing said, using the same compound your trying to separate :P

Oops. I think I got right and left confused. Increasing the concentration of OH-, should drive

M+n + n OH- = M(OH)n

to the right, ------>, towards more M(OH)n.

I would think that once you have it to this point, the Chlorine will burn off during smelting..

The only feasible way to separate Solids like that would be a Filter/Siv OR put them in a bowl and attach a vibrating motor to the base. Provided you particles are Different sizes, the larger ones will "Float" to the top.


3 years ago

Isn't an aquas solution of Fe Cl used to etch Copper Printed Circuit Boards, by exchanging the iron for the copper ??


that was my first though too

If you are trying to make pure iron, start with the ore.

Add carbon (powdered charcoal is perfect), and heat strongly for 20 minutes if you're working in tea-spoon quantities, hours if you are making more.