As I understand the chemistry, you have some iron sulfate as a pH buffer, but its oxidized to rust. You want to make iron sulfate from rust -- chemically or electrochemically. That's not possible, for a novice.
Enthalpy: said its not necessary. Iron sulfate is water soluble, and rust isn't. You can dissolve in water, strain out, and you will simply have less iron sulfate by the weight of the remaining rust. Or simply use it -- eventually bacteria will reduce the rust to plant usable form.
As I understand the chemistry, you have some iron sulfate as a pH buffer, but its oxidized to rust. You want to make iron sulfate from rust -- chemically or electrochemically. That's not possible, for a novice.
Enthalpy: said its not necessary. Iron sulfate is water soluble, and rust isn't. You can dissolve in water, strain out, and you will simply have less iron sulfate by the weight of the remaining rust. Or simply use it -- eventually bacteria will reduce the rust to plant usable form.
By the way can i use electrolysis to reduce fe3+ to fe2+?
Won't be easy. Fe3+ is practically insoluble in water, as it precipitates as Fe(OH)3. To keep it in the solution you need very low pH, which means you need to add a lot of acid - so it is no longer just a solution of Fe3+ salt. Unfortunately, in highly acidic solutions H+ is reduced much earlier than Fe3+,so you will be electrolyzing water, not converting Fe3+ to Fe2+. Perhaps playing with electrode material and complexing agents it can be possible to design a system in which Fe3+ gets reduced first, but then you will need some way of purifying the salt afterwards. Doesn't make sense.
By the way can i use electrolysis to reduce fe3+ to fe2+?
Won't be easy. Fe3+ is practically insoluble in water, as it precipitates as Fe(OH)3. To keep it in the solution you need very low pH, which means you need to add a lot of acid - so it is no longer just a solution of Fe3+ salt. Unfortunately, in highly acidic solutions H+ is reduced much earlier than Fe3+,so you will be electrolyzing water, not converting Fe3+ to Fe2+. Perhaps playing with electrode material and complexing agents it can be possible to design a system in which Fe3+ gets reduced first, but then you will need some way of purifying the salt afterwards. Doesn't make sense.
Enthalpy: said its not necessary. Iron sulfate is water soluble, and rust isn't. You can dissolve in water, strain out, and you will simply have less iron sulfate by the weight of the remaining rust. Or simply use it -- eventually bacteria will reduce the rust to plant usable form.
Enthalpy: said its not necessary. Iron sulfate is water soluble, and rust isn't. You can dissolve in water, strain out, and you will simply have less iron sulfate by the weight of the remaining rust. Or simply use it -- eventually bacteria will reduce the rust to plant usable form.
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Or Fe2(SO4)3 alone, which is soluble in water while Fe2O3 is not? Is that any feasible?
Or Fe2(SO4)3 alone, which is soluble in water while Fe2O3 is not? Is that any feasible?
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Won't be easy. Fe3+ is practically insoluble in water, as it precipitates as Fe(OH)3. To keep it in the solution you need very low pH, which means you need to add a lot of acid - so it is no longer just a solution of Fe3+ salt. Unfortunately, in highly acidic solutions H+ is reduced much earlier than Fe3+,so you will be electrolyzing water, not converting Fe3+ to Fe2+. Perhaps playing with electrode material and complexing agents it can be possible to design a system in which Fe3+ gets reduced first, but then you will need some way of purifying the salt afterwards. Doesn't make sense.
Won't be easy. Fe3+ is practically insoluble in water, as it precipitates as Fe(OH)3. To keep it in the solution you need very low pH, which means you need to add a lot of acid - so it is no longer just a solution of Fe3+ salt. Unfortunately, in highly acidic solutions H+ is reduced much earlier than Fe3+,so you will be electrolyzing water, not converting Fe3+ to Fe2+. Perhaps playing with electrode material and complexing agents it can be possible to design a system in which Fe3+ gets reduced first, but then you will need some way of purifying the salt afterwards. Doesn't make sense.
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