Solving Endothermic ΔHsolution: NaCl, CH3OH, C6H14, CH3CH2OH, CH3OH

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The discussion centers on predicting which substance has the most endothermic ΔHsolution among various solute-solvent combinations. Participants argue that dissolving NaCl in C6H14 is particularly challenging due to the ionic nature of NaCl and the nonpolar characteristics of C6H14. There is a debate about the definitions of "insoluble" and "impossible," with some suggesting that even minimal solubility exists in certain conditions. The conversation highlights the complexity of solubility and the varying concentrations of saturated solutions. Ultimately, the dissolution of NaCl in hexane is deemed highly unlikely, but not entirely impossible.
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Homework Statement



20. For which of the following is the ΔHsolution predicted to be the most endothermic?
(1) Dissolving NaCl in HCl
(2) Dissolving CH3OH in H2O
(3) Dissolving NaCl in C6H14
(4) Dissolving CH3CH2OH in C6H14
(5) Dissolving CH3CH2OH in CH3OH

Homework Equations



If the heat of solution is endothermic, this indicates that dissolution is unlikely to happen.

The Attempt at a Solution



It seems as if the dissolution of NaCl in C6H14 would be very hard to achieve since one is ionic and the other is the polar opposite of ionic.

Experimentally, however, my teacher argues that the dissolution of NaCl in hexane is impossible - even if you vaporize NaCl.

What's your take?
 
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Define "insoluble", define "impossible".

It is a matter of where you put the line between soluble and insoluble, as everything dissolves in everything, just concentrations of the saturated solution vary. AgCl is considered insoluble in water, yet saturated solution contains 10-5 M AgCl. No idea what are concentrations of the saturated NaCl hexane solutions, but for sure it is not just zero.
 
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