Which is more soluble, sodium iodide, or sodium fluoride?
I would presume
So before we interrogate the data, why should I so presume? The iodide ion is MUCH larger than the fluoride ion. The degree of electrostatic interaction between the gegenions is
But chemistry is an experimental science, first and foremost. Are the data consistent with my (potentially) whack reasoning? Let's see.......
This site quotes a solubility of
The smaller fluoride anion in solution is also more polarizing, and potentially induces more solvent order upon solvation. Certainly, the reduced acidity of
Note that because of the size mis-match you can also get iodide salts up into solvents such as acetone. This is something that you cannot do with the lower halides......