Assertion: `BeSO_(4) and MgSO_(4)` are insoluble in water.
Reason: `Be^(2+) and Mg^(2+)` have low hydration enthalpies.

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion
B. If both assertion and reason are true but reason is not the correct explanation of assertion
C. If assertion is true but reason is false.
D. If both assertion and reason are false.

Explanation

To solve the question, we need to analyze both the assertion and the reason provided.

**Step 1: Analyze the Assertion**
The assertion states that BeSO₄ (Beryllium sulfate) and MgSO₄ (Magnesium sulfate) are insoluble in water.

- **Fact Check**: Both BeSO₄ and MgSO₄ are actually soluble in water. Beryllium sulfate is sparingly soluble, while magnesium sulfate is quite soluble. Therefore, the assertion is **false**.

**Step 2: Analyze the Reason**
The reason given is that Be²⁺ and Mg²⁺ have low hydration enthalpies.

- **Fact Check**: Hydration enthalpy refers to the energy released when ions are surrounded by water molecules. Beryllium and magnesium ions are small cations, which typically have high hydration enthalpies due to their small size and high charge density. Thus, the reason is also **false**.

**Step 3: Conclusion**
Since both the assertion and the reason are false, we conclude that the correct answer is that both statements are incorrect.

### Final Answer:
Both the assertion and the reason are false.

---