Answer:
A) Decreasing solubility with increasing lattice energy.
B) Ionic compounds are more soluble in a polar solvent.
C) Increasing solubility with increasing enthalpy of hydration.
Step-by-step explanation:
A) Lattice energy is the energy contained in the crystal lattice of a compound (mostly ionic). It is also the energy that would be released if the component ions were brought together from infinity to form the compound.
For a compound to dissolve, the solvation energy that the fluid would use to work on its ions must exceed the compound's lattice energy. Hence, the higher the lattice energy, the less soluble the compound would be.
B) The 'like dissolves like' law in dissolution is very true and applicable. The law explains that polar compounds will dissolve in polar solvents and not dissolve in non-polar solvents. Only non-polar compounds will dissolve in non-polar solvents.
Ionic compounds contain positive and negative ions, making them one of the most polar sets of compounds. So, they will easily dissolve in polar solvents.
C) Enthalpies of hydration of the cations and anions represent the total enthalpy of dissolution. This is the energy released when a compound undergoes hydration. A form of salvation of the ions, the enthalpy of hydration need to match or exceed the lattice energybof the compound For the compound to be soluble. Hence, the larger the enthalpies of hydration, the more likely the compound will be soluble.
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