dddd said:
Thank you!
That’s interesting!
When you say more base, you mean dissolve the iodine crystals in more ethanol?
Or iodine/ethanol drops in more water?
No. Something like NaOH. Or even a weaker base, like Na
2CO
3.
dddd said:
Also would my calculation be accurate to add 10 grams of I2 to 1 liter of ethanol to make 1% solution?
No. Because % would refer either to volume % (not straightforward, volume is not conserved on addition), or mass % (mass, unlike volume, is conserved).
The density of 100% ethanol at 20 C is 789 g/l, not 990 g/l. To get 1% iodine solution, you would need to add 1 g of iodine to 99 g solvent. Thus 7,97 g iodine to 789 g (1 l) ethanol.
dddd said:
Last thing…
So do you think that I2 ethanolic solution changes when added to water or not?
Not seriously.
I tried to track down just how much of iodine is in the form of acids in pure aqueous solution.
The total solubility at 20 C is quoted in the range of 0,25 to 0,3 g iodine per 1000 g of water. All sources agree that it is overwhelmingly molecular I
2 in the absence of bases; one source that offered numbers gave less than 0,01 g/l of iodine in the acid form (under 4% of the small amount of total iodine).
In pure ethanol, the solubility is in the region of 270 g I
2 per 1000 g solvent, all of it as I
2. Adding water would still leave most of iodine as I
2.
What would change things if you add a iodide or especially, if you add a base.