I want to solve approximately 50mgr PbI2 in 10ml chloroform.
Is it possible? Does anyone have experienced this?
I don't want to heat my solution up. But if I solve it with raising temperature, then cool it down, does it precipitate?
A question was asked by a Research Gate colleague 5 years ago and there were good replies "see. e.g. Professor Carlos's contribution":
https://www.researchgate.net/post/Which_organic_solvents_can_be_used_to_disolve_PbI2_or_PbCl3_crystals
Please do not use chloroform since it is harmful & I actually do not expect that lead(II) iodide will dissolve in it significantly.
The use of chloroform has been phased out in 2015 via the Montreal Agreement of 1987. See: http://www.environment.gov.au/protection/ozone/montreal-protocol
You should look for an alternative solvent. As well as depleting the ozone layer, chloroform is an excellent liver and kidney poison.
In addition to its hazardous nature of chloroform, I don't think it can dissolve PbI2. You have to think of some other solvents such as DMF or DMSO.
The best way to answer this and similar questions is to do the simple experimental work
A question was asked by a Research Gate colleague 5 years ago and there were good replies "see. e.g. Professor Carlos's contribution":
https://www.researchgate.net/post/Which_organic_solvents_can_be_used_to_disolve_PbI2_or_PbCl3_crystals
Please do not use chloroform since it is harmful & I actually do not expect that lead(II) iodide will dissolve in it significantly.
I found another relevant question that was posted 4 years ago but the Internet stopped working for ~ 2 hours here, unfortunately. Now that it returns, here is the question & the answers:
https://www.researchgate.net/post/Is_Lead_Iodide_completely_soluble_in_DMF
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