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Anhydrous ferric chloride to hydrated FeCl3.6H2O
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+ Inorganic chemistry
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Nmra Shah
Anhydrous ferric chloride to hydrated FeCl3.6H2O
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Is exposure to air enough
Depends on how exactly ·6H2O you need it. Most hydrates have rather variable composition, with exact stoichiometry (amount of water) depending on the partial pressure of water in the air.
But in general yes, if you leave the anhydrous FeCl3 in the open for long enough, you will end up with something that is identical to FeCl3·6H2O left in the same place to equilibrate (exact final composition being a function of humidity).
Depends on how exactly ·6H2O you need it. Most hydrates have rather variable composition, with exact stoichiometry (amount of water) depending on the partial pressure of water in the air.
But in general yes, if you leave the anhydrous FeCl3 in the open for long enough, you will end up with something that is identical to FeCl3·6H2O left in the same place to equilibrate (exact final composition being a function of humidity).
Depends on how exactly ·6H2O you need it. Most hydrates have rather variable composition, with exact stoichiometry (amount of water) depending on the partial pressure of water in the air.
But in general yes, if you leave the anhydrous FeCl3 in the open for long enough, you will end up with something that is identical to FeCl3·6H2O left in the same place to equilibrate (exact final composition being a function of humidity).
Depends on how exactly ·6H2O you need it. Most hydrates have rather variable composition, with exact stoichiometry (amount of water) depending on the partial pressure of water in the air.
But in general yes, if you leave the anhydrous FeCl3 in the open for long enough, you will end up with something that is identical to FeCl3·6H2O left in the same place to equilibrate (exact final composition being a function of humidity).
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