hydrated chemicals - The Planted Tank Forum
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post #1 of 5 (permalink) Old 03-21-2005, 08:57 AM Thread Starter
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hydrated chemicals

I would like to know the reason why certain chemicals for example mgSO4 come in hydrated form(mgSO4+7H2O)and if it makes any difference when disolved in water........
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post #2 of 5 (permalink) Old 03-21-2005, 09:30 AM
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I hope im right.,.. im pretty sure i am anyway, all it means is its readily absorped by the water and the plants.. i think the term is also chelated, there are types or Iron (Fe) that cannot be dissolved as easily as chelated iron therefor leaving deposits etc which are useless.

i also think the process of hydration involves taking the solid to a liquid.. then back to a solid again. but containing only the watersoluble solids that will assure 100% disolution.. and leaving the unsoluble chemicals for other purposes. i might be wrong but someone on here will sure answer you.
but you have the right idea.
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post #3 of 5 (permalink) Old 03-21-2005, 04:53 PM
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HYDRATE - A solid compound containing water molecules combined in a definite ratio as an integral part of the crystal.
I think we see hydrated Magnesium Sulphate available as it is more stable and less reactive than anhydrous MgSO4.

Chelation is a different matter alltogether...
CHELATE - A chemical compound in the form of a heterocyclic ring, containing a metal ion attached by coordinate bonds to at least two nonmetal ions.
...which basically means (in the case of iron in our aquaria) the heavy metal is bound in a compound that can be utilised by the plants.


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post #4 of 5 (permalink) Old 03-21-2005, 07:56 PM
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Originally Posted by Stu
I think we see hydrated Magnesium Sulphate available as it is more stable and less reactive than anhydrous MgSO4.
A little more specific: anhydrous MgSO4 (no water) would readily absorb water from the air - every time you opened the container. Thus, the amount you weigh out would be MgSO4 plus an unknown amount of water - and the amount of water would change over time! So to make life easier, we buy the hydrated form so we know exactly how much water is bound in the crystals. Now when you weigh Epsom salts (MgSO4*7H2O), you know you are getting 7 water molecules for every magnesium and sulfate ion.

Bottom line though is that since we are putting it in water, the biggest difference between using anhydrous and hydrated MgSO4 is the amount you would need to weigh out to get the same amount of magnesium.



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post #5 of 5 (permalink) Old 03-21-2005, 08:56 PM Thread Starter
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Thanks a lot gyes,you've been very clear...
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