As we know the enthalpy of solution is equal to the addition of lattice energy and...

As we know the enthalpy of solution is equal to the addition of lattice energy and hydration energy.

Why does solubility depend on the relative magnitude of the lattice energy compared to the hydration energy?

Expert Solution

Explanation:

Hydration energy is the amount of energy released when one mole of ions undergo hydration (or) it is the energy liberated when solute is dissolved in a solvent. Mostly water is used as a solvent to describe about hydration energy.

Lattice energy is described as the energy needed to bound the crystal lattice. Even though the enthalpy of solution is equal to the addition of lattice and hydration energy, lattice energy plays an important role in deciding the melting point and thermal stability of ionic salts.

In order to form a soluble substance hydration energy should be more than lattice energy.

Example: Salts such as NaCl dissolve in water because the hydration energy is more than lattice energy. Whereas solutes like LiF is insoluble in water because it's hydration energy is less than lattice energy.

Addition of CaCl2 heats the water while dissolving. However CaCl2.6H2O cools the water upon dissolution. Cooling takes place when hydration energy cannot over come the lattice energy.

These are the reasons for the dependence of solubility more on lattice energy than on hydration energy.

queen_honey_blossom answered 2 years ago

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