SO, we can safely generalize that in the vast majority of solutions involving a solid solute and a liquid solvent, the entropy change of the dissolving process is positive. Magnitudes will vary, of course, but that final value in the Gibbs-Helmholtz equation is always going to be positive.

Most people know from common experience that solids seem to dissolve better at higher temperatures (sugar and salt are both familiar examples). There are exceptions to this generalization, but there are not a lot and we don't need to think about them right now. Temperature is clearly a factor and we can control this factor to encourage (or discourage) the formation of many solutions.

What we cannot control is the enthalpy change. It's sign and magnitude therefore become interesting.

Designing an experiment around this topic means trying to sort out the likely variables that influence the enthalpy changes in the three hypothetical steps of solution formation.