Lattice enthalpies of `BeF_(2),MgF_(2),CaF_(2) and BaF_(2)` are `-2906,-2610,-2459 and -2367 kJ mol^(-1)` resoectively. Hydration enthalpies of `Be^(2+),Ca^(2+),Ba^(2+) and F^(Θ)` are `-2194,-1921,-1577,-130 and -457 kJ mol^(-1)` respectively. Which of the fluorides has the highest solublility in water?

Explanation

To determine which of the fluorides (BeF₂, MgF₂, CaF₂, and BaF₂) has the highest solubility in water, we will analyze the given lattice enthalpies and hydration enthalpies.

### Step-by-Step Solution:

1. **Understanding Lattice Enthalpy and Hydration Enthalpy**:
- Lattice enthalpy is the energy released when gaseous ions combine to form an ionic solid. A more negative lattice enthalpy indicates a stronger ionic bond, which typically means lower solubility.
- Hydration enthalpy is the energy released when ions are surrounded by water molecules. A more negative hydration enthalpy indicates that the ion is more stable in solution, which typically means higher solubility.

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