Assertion: Alkali metals are obtained by electrolysis of molten salt and not aqueous solution.
Reason: The discharge potential of `H^(+)` ions is lower than alkali metals cation hence hydrogen is dicharged at cathode instead of metal.

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.

Answer

To solve the question regarding the assertion and reason about alkali metals and their electrolysis, we will break it down step by step.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states that alkali metals are obtained by the electrolysis of molten salts and not from aqueous solutions. This is true because when we electrolyze molten salts, the ions are free to move and discharge at the electrodes.

2. **Electrolysis of Aqueous Solutions**:
- In an aqueous solution, such as NaCl, both sodium ions (Na⁺) and hydrogen ions (H⁺) are present. When electrolysis occurs, we need to consider which ion will be discharged at the cathode.

3. **Discharge Potential**:
- The reason provided states that the discharge potential of H⁺ ions is lower than that of alkali metal cations (like Na⁺). This means that H⁺ ions are more readily discharged than Na⁺ ions during electrolysis in an aqueous solution.

4. **Electrochemical Series**:
- Referring to the electrochemical series, we find that H⁺ has a higher reduction potential compared to Na⁺. Therefore, during electrolysis of an aqueous solution, H⁺ ions will be discharged at the cathode to form hydrogen gas (H₂) instead of Na⁺ ions being discharged to form sodium metal.

5. **Conclusion**:
- Since H⁺ ions are discharged at the cathode in aqueous solutions, alkali metals cannot be obtained from the electrolysis of aqueous solutions. Instead, they are obtained from the electrolysis of molten salts where only the alkali metal cations are present and can be discharged.

6. **Final Evaluation**:
- Both the assertion and the reason are true. The reason correctly explains why the assertion is true: the presence of H⁺ ions in aqueous solutions prevents the discharge of alkali metal cations.

### Final Answer:
- **Both the assertion and reason are true, and the reason correctly explains the assertion.**

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