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

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SUMMARY

The discussion centers on predicting the most endothermic ΔHsolution among five scenarios involving NaCl, CH3OH, C6H14, and CH3CH2OH. Participants conclude that dissolving NaCl in C6H14 is the least favorable due to the ionic nature of NaCl contrasting with the non-polar characteristics of C6H14. The concept of solubility is debated, with emphasis on the definitions of "insoluble" and "impossible," highlighting that even substances deemed insoluble can have trace solubility. The conversation underscores the complexity of dissolution processes and the importance of concentration in defining solubility.

PREREQUISITES
  • Understanding of thermodynamic principles, specifically ΔHsolution
  • Knowledge of solubility concepts and definitions
  • Familiarity with ionic and non-polar substances
  • Basic chemistry knowledge regarding dissolution processes
NEXT STEPS
  • Research the thermodynamic principles of ΔHsolution in detail
  • Explore the solubility rules for ionic and non-polar compounds
  • Investigate the concept of saturated solutions and their concentrations
  • Examine case studies of dissolution processes in various solvents
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Chemistry students, educators, and researchers interested in thermodynamics, solubility, and dissolution processes in chemical reactions.

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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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