1. The heat of solution of salta may either be endothermic or exothermic. What factors determine this?
2. As a solution freezes, why does the freezing temperature continue to decrease?
3. When the concentration of very dilute aqueous solutions are calculated, why are the values of molarity and molality the same?
1. Basically how much energy is need to break about the crystal lattice vs the energy produced by hydration of the resulting ions.
2. As the "pure" water freezes, the solution that is left is more concentrated in the solute; hence, a more concentrated solution lowers the freezing point.
3. Molarity =# mols/L solution; molality = # mols/kg solvent. As the # mols becomes smaller and smaller, at "infinite" dilution density of the solutins are the same because the L of solution is closer and closer to a kg of solvent.
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