The low solubility of `BaSO_(4)` in water can be attributed to

Options

A. High lattice energy
B. Dissociation energy
C. Low lattice energy
D. Ionic bond

Answer

To solve the question regarding the low solubility of BaSO₄ in water, we can break down the reasoning step by step.

### Step-by-Step Solution:

1. **Understanding Solubility**:
- Solubility refers to the ability of a substance to dissolve in a solvent (in this case, water). The solubility of a compound is influenced by various factors, including lattice energy and hydration energy.

2. **Lattice Energy**:
- Lattice energy is the energy required to separate one mole of a solid ionic compound into its gaseous ions. A high lattice energy indicates that the ions are held together very tightly in the solid state.

3. **Hydration Energy**:
- Hydration energy is the energy released when ions are surrounded by water molecules. For a compound to dissolve, the hydration energy must be sufficient to overcome the lattice energy.

4. **BaSO₄ Characteristics**:
- Barium sulfate (BaSO₄) is an ionic compound. It has a relatively high lattice energy due to the strong electrostatic forces between the Ba²⁺ and SO₄²⁻ ions.

5. **Comparison of Energies**:
- In the case of BaSO₄, the lattice energy is significantly higher than the hydration energy provided by water molecules. This means that when BaSO₄ is added to water, the energy released from hydration is not enough to break the ionic bonds in the solid.

6. **Conclusion**:
- Therefore, the low solubility of BaSO₄ in water can be attributed to its high lattice energy, which prevents it from dissolving effectively.

### Final Answer:
The low solubility of BaSO₄ in water can be attributed to its high lattice energy.

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