Figuring out a good recrystallizing solvent may take trial an error not only testing out different solvents (and solvent mixtures) but also testing out different concentrations. While sodium hydroxide is very soluble in water, one can recrystallize NaOH in water at high concentrations such as 60 grams NaOH in 100 mL of water. The purity may be good but the yield may be low. I would also explore alcohols such as ethanol and isopropanol which my require less concentrated solutions and result in higher yields. Two other solvents I would try would be acetonitrile and ethyl acetate. In both cases heating might be better done with a reflux set-up rather than heating on a hot plate leading to a lot of evaporation
@@fieldguide2chemistry Thanks for responding. I looked up several solubility tables and they showed that non-polar solvents would be best but then do I want the end product polluted with something like acetone or dimethylether? What I am looking at is trying to clean up hardware store sodium hydroxide. I saw due to it's solubility, it would be difficult to settle out the end product, but since I don't know what the contaminants are, I have to try to pull one or the other out.
Good video.... any day I learn something is a good day!
Your amazing....
Very good explanation
But if reactant and product both solid which solvent select for recrystallization and how to salect
Since you are choosing a solvent, which solvent should I use to dissolve and recrystalize sodium hydroxide with?
Figuring out a good recrystallizing solvent may take trial an error not only testing out different solvents (and solvent mixtures) but also testing out different concentrations. While sodium hydroxide is very soluble in water, one can recrystallize NaOH in water at high concentrations such as 60 grams NaOH in 100 mL of water. The purity may be good but the yield may be low.
I would also explore alcohols such as ethanol and isopropanol which my require less concentrated solutions and result in higher yields. Two other solvents I would try would be acetonitrile and ethyl acetate. In both cases heating might be better done with a reflux set-up rather than heating on a hot plate leading to a lot of evaporation
@@fieldguide2chemistry Thanks for responding. I looked up several solubility tables and they showed that non-polar solvents would be best but then do I want the end product polluted with something like acetone or dimethylether?
What I am looking at is trying to clean up hardware store sodium hydroxide. I saw due to it's solubility, it would be difficult to settle out the end product, but since I don't know what the contaminants are, I have to try to pull one or the other out.
What is this breaking bad?
The KOH get rid the resin. KOH not soluble in acetone
Halo how are you How mix |
😵
It appears if it were an amine the anologue would be. Ugh 😫 😮😯😯
Whats the best method for meth? Come on smarty pants, tell us that.
has nothing to do with choosing a solvent.