How to avoid errors when changing a hydrate to anhydride?

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When converting a hydrate to an anhydrous form, several unavoidable errors can arise during the heating and cooling process. The procedure typically involves heating the hydrate in a crucible and then cooling it in a desiccator until a constant mass is achieved. However, this method may not be universally applicable to all hydrates. One significant issue is that hydrates with low boiling points may also lose other components during heating, not just water. Additionally, after heating, the anhydrous compound can absorb moisture from the air, leading to inaccurate mass measurements. Contaminants such as dust or fingerprints on the crucible can also affect the results, depending on the precision of the balance used. Overall, while the procedure is generally effective, various factors can introduce errors that compromise the accuracy of the mass determination.
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what are the possible unavoidable errors when changing a hydrate to an anhydrous. the procedure called for heating the hydrate in a crucible a few times and cooling to room temp in a desiccator until mass measured was constant. also why wouldn't this procedure work for all hydrates? thank you for help.
 
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This procedure is fine enough way to do it, all you are doing is evaporating the water until all of it is gone (mass doesn't change, all water is gone).

I could see it not working in the case that you have a hydrate that also has a low boiling point, and would cause it to evaporate too.
 
After heating the hydrate to drive off the water, it is possible that the anhydrous would pick up water vapor from the air.
Also, there could be material (various dust particles, fingerprints, etc) on the crucible after heating it which would cause mass differences (depending on the precision of the balance.)
It is also possible that more than water is driven off when heating the crucible.
Although without viewing the actual procedure, it is hard to be certain on the sources of error.
 
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