Electrolyte strength and aqueous solubility

[Bernoull]

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Is there any direct relationship b/t the strength of an electrolyte and its solubility in water. I always thought stronger electrolytes dissolved better since electrolytic strength measures degree of dissociation in water (sorta like Ka) therefore if something completely dissociated I equated that with excellent solubility and vice versa. However I came across an EK explanation which threw a money wrench at this by pointing out the acetic acid which is highly soluble (polarity effects) is also a weak electrolyte. But then again acetic acd is molecular as opposed to ionic so it makes sense that it doesn't dissociate readily.

So my question is is there a direct relationship b/t electrolytic strength and water solutbility or at least b/t ionic electrolytic strength n solubility.

Thanks

 

[sv3]

To be an electrolyte the substance has to have some sort of solubility so if something is not soluble then it isn't an electrolyte. Beyond that things can get dicey as Ek pointed out. Something that is minimally soluble can perhaps dissociate to a greater extent than a substance that is very soluble. I would think (or like to think i should say) if this type of question showed up on the MCAT you'd get experimental data and have to figure it out. To keep it simple though dissociation is the key factor that i would focus on. Could get into trouble extending it although perhaps helpful on some sort of trick question

sv3

PS (there is no relationship that I've come across in my readings.....)

 

[Fifty 3rds]

bernoull,
I believe you already noticed the reason. Because you are dealing with an acid, it may not be as conductive as say, NaCl dissolved in water. The greater the solubility & the maximal amount of salt left in solution are probably the important points. That's an convoluted way of saying, Normality is very important when looking at conductance/electrolyte strength.