Re: Fe questions
From: Mohammed Farooq (farooq_w_at_hotmail.com)
Date: 06/12/04
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Date: 12 Jun 2004 10:58:50 -0700
"Hugh Janus" <HughJanus@bigfoot.com> wrote in message news:<hyzyc.1303$s52.50238@news.xtra.co.nz>...
> The amount of Fe in a 1.0230g sample of the iron ore hematite Fe2 O3, was
> determined as follows:
> the sample was transferred to a 250ml conical flask and completely dissolved
> in diluted hydrochloric acid. All the iron was then present as Fe2+ (aq).
> The contents of the flask were then titrated with a solution of potassium
> permanganate of concentration 0.0195 mol L-1 until the first permanent pink
> colour was obtained. At this point, 24.35ml of permanganate had been added.
> Calculate:
> The percentage of iron. Fe, in the ore;
>
> The percentage of hematite, Fe2 O3 in the ore..
>
> HOW?
> HELP!
This is an answer to "HOW" part of the question.
Assuming that by some "reduction process" all iron was present as
Fe(2+): Don't you think iron from hematite would be present as Fe(3+)
after dissolving in HCl?
1. Write a balanced equation containing MnO4(-), Fe(2+) and H+ ions.
2. Deduce mole ratio between iron and MnO4(1-)
3. You know the concentration and volume of permanganate, find out
moles of KMnO4 consumed.
4. From the mole ratio find out the moles of Fe(2+), which would
ultimately give you mass and hence percentage of iron in the ore.
Provided you find out the percentage of Fe in the ore and show your
calculations here, one can help you in finding out the percentage of
hematite in the ore.
Hint: [2(At.wt Fe) + 3(At.wt O)] gram Fe2O3 contains twice the atomic
weight of iron.
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