A tank holds 10,000 kg solution of Na2CO3 at 30 degrees celsius. you want to crystalllize from this solution 3000 kg of Na2CO3H2O without any accompanying water. to wha temperature must the solution be cooled? Below is the solubility table for Na2CO3
Stacey Warren - Expert brainly.com
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An interesting question indeed.
We have a solution of Na2CO3 from which we would like to crystallize Na2CO3.H2O (monohydrate) instead of the usual decahydrate (Na2CO3.10H2O) by simple cooling.
The "conventional" method back in 1935 requires crystallization of an aqueous solution at around 34-36 deg.C (hotter than the initial solution temperature) to obtain the monohydrate . Don't know if there is a modern way that can produce the monohydrate by simple cooling below 30 deg.
Also, it is not clear if the 10000 kg solution is saturated (i.e. solid+H20 = 10000 kg), or 10000 kg of decahydrate dissolved in an appropriate amount of water.
Notice that the solubilities given are for the decahydrate (Na2CO3.10H2O).
By the way, this is a chemistry question. You would have more success (and according to OS rules) to post this question in the chemistry section.
it's a chemical engineering calculations subject :) @mathmate
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It's even better if it is a engineering question, because then you're expected to cover all bases, instead of a blind application of formulas.
Please provide your interpretations/comments to the folowing:
1. Is the 10000 kg solution saturated, or 10000kg of Na2CO3.10H2O dissolved in an appropriate amount of water.
2. when cooled from 30 deg. C, do we get crystals of the decahydrate or the monohydrate? (the latter is expected by the question). If it is decahydrate, then it needs to be heated appropriately before cooling?
Feel free to give your own views and comments on the question, i.e. show your efforts, please.