Which of the following can serve as a solvent for both ionic and covalent compounds?

Options

A. Liquid ammonia
B. `H_(2)O`
C. Benzene
D. `C Cl_(4)`

Answer

To determine which solvent can dissolve both ionic and covalent compounds from the given options (liquid ammonia, water, benzene, and carbon tetrachloride), we can analyze each solvent based on its polarity and ability to interact with different types of compounds.

### Step-by-Step Solution:

1. **Identify the Nature of the Solvents**:
- **Liquid Ammonia (NH₃)**: This is a polar solvent.
- **Water (H₂O)**: This is also a polar solvent.
- **Benzene (C₆H₆)**: This is a nonpolar solvent.
- **Carbon Tetrachloride (CCl₄)**: This is also a nonpolar solvent.

2. **Evaluate Solubility of Ionic Compounds**:
- Ionic compounds typically dissolve well in polar solvents due to the strong interactions between the ions and the polar molecules.
- **Water** and **Liquid Ammonia** can both dissolve ionic compounds effectively.

3. **Evaluate Solubility of Covalent Compounds**:
- Covalent compounds may dissolve in polar or nonpolar solvents, but the effectiveness depends on the specific interactions.
- **Water** has strong hydrogen bonding, which can hinder the dissolution of some covalent compounds.
- **Liquid Ammonia** has weaker hydrogen bonding compared to water, making it more effective in dissolving covalent compounds.

4. **Conclusion**:
- While both water and liquid ammonia can dissolve ionic compounds, liquid ammonia is more suitable for dissolving covalent compounds due to its lower viscosity and weaker hydrogen bonding.
- Nonpolar solvents like benzene and carbon tetrachloride are not suitable for dissolving ionic compounds.

5. **Final Answer**:
- Therefore, the solvent that can serve as a solvent for both ionic and covalent compounds is **Liquid Ammonia**.