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Is zinc powder just crushed zinc?
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Zinc
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#2
15 September 2010 - 12:54 AM
Mr Skeptic 
iDon't-Believe-You
Sort of, but remember that metals are hard to "crush" since they are malleable.
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#3
16 September 2010 - 05:52 PM
The Apprentice
Lepton
Is there an easy way to do it? mabey by breaking it down with hydrochloric acid? but then that wouldnt give the end result i want...
This post has been edited by The Apprentice: 16 September 2010 - 05:53 PM
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#4
5 December 2010 - 09:45 PM
ammonium nitrate
Quark
angle grinder
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#7
18 October 2011 - 11:41 PM
elementcollector1
Baryon
There is a way to do it with muriatic acid, but it requires a more reactive metal, such as magnesium. This is a single displacement reaction:
ZnCl2 + Mg -> Zn + MgCl
So dissolve the zinc in excess hydrochloric acid (until there is no further reaction with the zinc), and add a block of magnesium. The zinc will be precipitated out as a powder, which can then be washed with water and dried.
ZnCl2 + Mg -> Zn + MgCl
So dissolve the zinc in excess hydrochloric acid (until there is no further reaction with the zinc), and add a block of magnesium. The zinc will be precipitated out as a powder, which can then be washed with water and dried.
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#8
19 October 2011 - 06:04 PM
John Cuthber
Chemistry Expert
elementcollector1, on 18 October 2011 - 11:41 PM, said:
There is a way to do it with muriatic acid, but it requires a more reactive metal, such as magnesium. This is a single displacement reaction:
ZnCl2 + Mg -> Zn + MgCl
So dissolve the zinc in excess hydrochloric acid (until there is no further reaction with the zinc), and add a block of magnesium. The zinc will be precipitated out as a powder, which can then be washed with water and dried.
ZnCl2 + Mg -> Zn + MgCl
So dissolve the zinc in excess hydrochloric acid (until there is no further reaction with the zinc), and add a block of magnesium. The zinc will be precipitated out as a powder, which can then be washed with water and dried.
Displacement reactions like that are only marginally effective. What often happens is that the zinc will react with the water to produce hydrogen and zinc hydroxide.
Of course, if there is excess acid present (as you have suggested) then the zinc will react with that, so you will just get a solution of the mixed chlorides and hydrogen.
In any event, you won't get MgCl because Mg doesn't have a stable +II oxidation state.
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#9
19 October 2011 - 11:38 PM
elementcollector1
Baryon
John Cuthber, on 19 October 2011 - 06:04 PM, said:
Displacement reactions like that are only marginally effective. What often happens is that the zinc will react with the water to produce hydrogen and zinc hydroxide.
Of course, if there is excess acid present (as you have suggested) then the zinc will react with that, so you will just get a solution of the mixed chlorides and hydrogen.
In any event, you won't get MgCl because Mg doesn't have a stable +II oxidation state.
Of course, if there is excess acid present (as you have suggested) then the zinc will react with that, so you will just get a solution of the mixed chlorides and hydrogen.
In any event, you won't get MgCl because Mg doesn't have a stable +II oxidation state.
It... doesn't? It's an alkaline earth metal.
And in that case, I'd like to add something to the procedure. Between dissolving acid and adding magnesium, you should first:
-Boil down the solution (carefully and outside, you don't want HCl inside your home)
-Re-dissolve the zinc in distilled water.
Would that work better?
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#10 24 October 2011 - 09:18 AM Guest_meercy_*
Fine zinc powders (formerly named zinc dust) serve as protective pigment in industrial coatings or as reducing agent and catalyst in various chemical reactions.
- 5 plants: Angler (B), Laraine (No), Changsha (Ch), Johan Baruch (Mal) and Melbourne (Au)
- 100 000 T of very Fine Zinc Powder of which 30% produced from recycled secondary zinc
- more than 20 different grades serving various industries
This post has been edited by meercy: 24 October 2011 - 09:19 AM
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