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Deferrization from 10 ppm to 0.1 ppm

Deferrization from 10 ppm to 0.1 ppm

Deferrization from 10 ppm to 0.1 ppm

(OP)
I'd posted this question in another forum with no success. I hope this is the right place to collect some valid answer.

I need to treat water (24 m3/day on the average and 1.5 m3/h as peak) in order to remove iron ions. Actual iron concentration is 10 ppm, and I need to bring concentration down below 0.1 ppm. A vendor proposed me a pyrolusite (essentially MnO2) filled filter. The above material needs to be activated with a chlorination process. As an alternative he proposed a zeolite filled filter, which needs KMnO4 as oxidant agent to be activated.
I would like to know whether anyone has any experience with these kinds of filter and whether of filter and used hydrogen peroxide (35% mass concentration or 130 volumes) instead of potassium permanganate when dealing with zeolite.
Please do not suggest to ask the vendor...... Thanks
 

RE: Deferrization from 10 ppm to 0.1 ppm

Iron removal is done all of the time with simple sand filters.

If you have a neutral pH reading, the iron will be in the insoluble Fe+3 form. All you have to do is to run it through a filter.

If the solution is exposed to air, the iron will air oxidize by itself, so you do not need to add an ozidizing agent (chlorine or KMO4).

A zeolite is probably not a good choice to do this. If you add the oxidant to the zeolite, you will also destroy the zeolite.

You are in the water foroum, not the waste forum so I am not going into wastewater.

You can accomplish this iron removal with a small lab unit or a swimmming pool filter.

RE: Deferrization from 10 ppm to 0.1 ppm

(OP)
bimr,

Thanks a lot for your reply (a star for you).
Test conducted on site is not that precise and it gives the whole amount of iron without any distinction between Fe++ and Fe+++.
I do not have a big chemistry background, anyway oxygen should be the element that transforms bivalent iron to trivalent iron. In a water with a poor oxygen content iron should be present as Fe++.

The pH is 7.5. With such a value of pH, is it possible to be sure iron is present as Fe+++ and so in an insoluble form?

RE: Deferrization from 10 ppm to 0.1 ppm

The iron oxidation reaction  occurs slower at lower pH values. At a pH of 7.5, the oxidation of iron when exposed to air should occur within 15 mniutes.

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