How could i dissolve iron powder

In summary: Is there a way to make a concentrated solution?Yes, you can make a concentrated solution by boiling the water off.
  • #1
seragrefaat
3
0
I want to make a standard iron solution 1 g/L by using iron powder and i can't dissolve it by any way. Is anyone have an idea? thanks in advance.
 
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  • #2
What form of iron are you after? Iron(0), iron(II) or iron(III).
 
  • #3
6 N HCl solution. Use it all the time to clean up flasks with iron residue.
 
  • #4
seragrefaat said:
I want to make a standard iron solution 1 g/L by using iron powder and i can't dissolve it by any way. Is anyone have an idea? thanks in advance.
HNO3 dissolves iron quickly, but it doesn't have to be concentrated, you have to dilute it with some water (6N should be ok) or the reaction will be blocked by passivation. Be careful to red smokes of NOx, do it in a hood.
 
  • #5
Be careful with the nitric acid. I'm wondering if ammonium nitrate is a possible side product if you try to dissolve Fe with nitric acid. One chemist we had was trying to clean out his glassware of iron residue with nitric acid and caused a massive explosion. Luckily he wasn't hurt, but glass shards went flying everywhere. There were huge 7+ inch shards of glass embedded 8 inches in the wall.
 
  • #6
gravenewworld said:
Be careful with the nitric acid. I'm wondering if ammonium nitrate is a possible side product if you try to dissolve Fe with nitric acid.
With an excess of iron it should be possible; it is, with excess zinc and HNO3. However, if NH4NO3 do really reacts in that way with HNO3, it should be, at least, dry.
One chemist we had was trying to clean out his glassware of iron residue with nitric acid and caused a massive explosion.
It's quite difficult for me to believe it was only Fe, NH4NO3 and HNO3, are you sure there wasn't something else, even in small amounts, in it?
 
  • #7
lightarrow said:
With an excess of iron it should be possible; it is, with excess zinc and HNO3. However, if NH4NO3 do really reacts in that way with HNO3, it should be, at least, dry. It's quite difficult for me to believe it was only Fe, NH4NO3 and HNO3, are you sure there wasn't something else, even in small amounts, in it?

We don't know. There could have been some organic material in there as well. ANyway, we aren't allowed to use nitric acid to clean glassware anymore.
 
  • #8
Not trying to hijack your thread I just had a real quick question that isn't worthy or starting a new thread.

Whats the difference between "solvating" and "dissolving"? I read that solvation is also called dissolution. Is dissolution just the process of dissolving? If I add salt to water I would be dissolving the salt in the water. Would I also be solvating the salt in the water or would I be solvating the water with salt?
 
  • #9
Mr_Bojingles said:
Not trying to hijack your thread I just had a real quick question that isn't worthy or starting a new thread.

Whats the difference between "solvating" and "dissolving"? I read that solvation is also called dissolution. Is dissolution just the process of dissolving? If I add salt to water I would be dissolving the salt in the water. Would I also be solvating the salt in the water or would I be solvating the water with salt?

They are completely different cocepts.
"Dissolve" means to bring something in solution, "solvate" means to make the molecules of that compound surrounded by water molecules, bound with some kind of weak bond, as ion-dipole, dipole-dipole bonds.
If you dissolve NaCl in water you will also have solvation of Na+ and Cl- ions, that is every ion in water will react with H2O molecules forming a weak bond with them (with a variable number of water molecules, depending on the kind of ion, concentration, temperature, ecc.).

In general you will always have more or less solvation, even if in some cases it could be so weak that you can neglete it; in that case you could have dissolution but with very little solvation; dissolution is a more complex phenomenon, that includes also solvation, in general (but not necessarily) but also other processes, that is the brokening of the salt's crystal, for example, and the increasing of the entropy due to the mixing solute/solvent.

So, even if "solvation" do certainly affect solubility, it's different from "dissolution".
 
  • #10
chemisttree said:
What form of iron are you after? Iron(0), iron(II) or iron(III).

it is a standard solution i think Iron(0) is correct

gravenewworld said:
6 N HCl solution. Use it all the time to clean up flasks with iron residue.

ok i'll try and see

lightarrow said:
HNO3 dissolves iron quickly, but it doesn't have to be concentrated, you have to dilute it with some water (6N should be ok) or the reaction will be blocked by passivation. Be careful to red smokes of NOx, do it in a hood.

6N HNO3? i didn't try to use it, thanks for the advice.

gravenewworld said:
Be careful with the nitric acid. I'm wondering if ammonium nitrate is a possible side product if you try to dissolve Fe with nitric acid. One chemist we had was trying to clean out his glassware of iron residue with nitric acid and caused a massive explosion. Luckily he wasn't hurt, but glass shards went flying everywhere. There were huge 7+ inch shards of glass embedded 8 inches in the wall.

thanks for the advice, and how is your friend now?

lightarrow said:
With an excess of iron it should be possible; it is, with excess zinc and HNO3. However, if NH4NO3 do really reacts in that way with HNO3, it should be, at least, dry. It's quite difficult for me to believe it was only Fe, NH4NO3 and HNO3, are you sure there wasn't something else, even in small amounts, in it?

!

gravenewworld said:
We don't know. There could have been some organic material in there as well. ANyway, we aren't allowed to use nitric acid to clean glassware anymore.

!

Mr_Bojingles said:
Not trying to hijack your thread I just had a real quick question that isn't worthy or starting a new thread.

Whats the difference between "solvating" and "dissolving"? I read that solvation is also called dissolution. Is dissolution just the process of dissolving? If I add salt to water I would be dissolving the salt in the water. Would I also be solvating the salt in the water or would I be solvating the water with salt?

it is ok my friend we all learn

lightarrow said:
They are completely different cocepts.
"Dissolve" means to bring something in solution, "solvate" means to make the molecules of that compound surrounded by water molecules, bound with some kind of weak bond, as ion-dipole, dipole-dipole bonds.
If you dissolve NaCl in water you will also have solvation of Na+ and Cl- ions, that is every ion in water will react with H2O molecules forming a weak bond with them (with a variable number of water molecules, depending on the kind of ion, concentration, temperature, ecc.).

In general you will always have more or less solvation, even if in some cases it could be so weak that you can neglete it; in that case you could have dissolution but with very little solvation; dissolution is a more complex phenomenon, that includes also solvation, in general (but not necessarily) but also other processes, that is the brokening of the salt's crystal, for example, and the increasing of the entropy due to the mixing solute/solvent.

So, even if "solvation" do certainly affect solubility, it's different from "dissolution".

thanks for the information

At the end and to be more clear i'll use this standard solution - after dissolving - to make a calibration curve for iron spectroscopic determination, now i'll try to use 6N HCL and 6N HNO3 separately of course and see.
 
  • #11
seragrefaat said:
I want to make a standard iron solution 1 g/L by using iron powder and i can't dissolve it by any way. Is anyone have an idea? thanks in advance.

I'm curious to know exactly what is the iron powder that you're employing; how was it obtained? It could be one of the many forms of the hydroxide precipitate. One other way to dissolve iron into the solution is through electrochemistry methods.
 
  • #12
GCT said:
I'm curious to know exactly what is the iron powder that you're employing; how was it obtained? It could be one of the many forms of the hydroxide precipitate. One other way to dissolve iron into the solution is through electrochemistry methods.

The iron powder i talk about is the one found in this link
http://www.sigmaaldrich.com/catalog/search/SearchResultsPage/PricingAvailability/RIEDEL;12312 1 Kg pack
 
Last edited by a moderator:
  • #13
The link is not functional.
 
  • #14
If you are interested in dissolving zero valent iron, you should use iron pentacarbonyl. Sigma Aldrich product number 481718-25ML(100ML). Be careful, it's very toxic.
 
  • #15
i would go for simply, 5 ml. of dilute sulfuric acid then heating.. or mix of HNO3 & HCL then heating.. the last one should certainly dissolve it.
 
  • #16
Silex7 said:
.. or mix of HNO3 & HCL then heating.. the last one should certainly dissolve it.
Why the need to add HCl? HNO3 alone (not concentrated or Fe would be passivated) dissolves it well.
 
  • #17
hm. Not to change topic (I don't feel like starting a thread for small inquires) but isn't iron powder used in some military hand grenade. I do not remember, but I think it is used in either stun grenades or maybe in some napalm type grenade used in Vietnam. Yeah, cause when it reacts with "something" rust, it let's off heat strong enough to penetrate metal and can burn for hours.
 
  • #18
No, I've heard of that too.
 

1. How does iron powder dissolve in water?

Iron powder can dissolve in water through a process called oxidation, where the iron reacts with oxygen present in the water. This forms iron oxide, which dissolves in the water. The reaction can be sped up by adding an acid, such as lemon juice or vinegar.

2. What is the best solvent for dissolving iron powder?

Water is the most common and effective solvent for dissolving iron powder. However, other solvents such as acids, alcohols, and glycols can also be used depending on the specific properties of the iron powder and the desired concentration of the solution.

3. How long does it take for iron powder to dissolve?

The time it takes for iron powder to dissolve depends on various factors such as the size of the iron particles, the temperature and pH of the solution, and the concentration of the solvent. Generally, it can take anywhere from a few minutes to a few hours for the powder to completely dissolve.

4. Can I speed up the dissolution process of iron powder?

Yes, you can speed up the dissolution process of iron powder by increasing the temperature and acidity of the solution. Stirring the solution can also help to distribute the iron particles evenly, allowing them to dissolve more quickly.

5. Is it safe to dissolve iron powder?

Dissolving iron powder can be hazardous if done without proper safety precautions. Iron powder can be flammable and corrosive, and the resulting solution may be harmful if ingested or inhaled. It is important to wear gloves, safety glasses, and work in a well-ventilated area when handling iron powder and its solvents.

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