State True or False
The current `-` carrying ions in an electrolytic cell are not necessarily discharged at the electrodes.

Explanation

To determine whether the statement "The current carrying ions in an electrolytic cell are not necessarily discharged at the electrodes" is true or false, we can analyze the behavior of ions during electrolysis.

### Step-by-Step Solution:

1. **Understanding Electrolytic Cells**: In an electrolytic cell, an electric current is passed through an electrolyte, causing chemical reactions at the electrodes. The ions present in the electrolyte carry the current.

2. **Identifying Ions in Electrolyte**: Consider the electrolysis of sodium chloride (NaCl) in aqueous solution. The ions present in this solution are Na⁺, Cl⁻, OH⁻, and H⁺.

3. **Discharge of Ions**: Not all ions present in the solution will necessarily be discharged (i.e., undergo reduction or oxidation) at the electrodes. The discharge depends on factors such as the standard electrode potentials of the ions.

4. **Example of Discharge**:
- At the cathode (negative electrode), both H⁺ and Na⁺ ions can be reduced. However, H⁺ ions are preferentially reduced to form hydrogen gas (H₂), while Na⁺ ions do not get reduced under these conditions.
- At the anode (positive electrode), Cl⁻ ions can be oxidized to form chlorine gas (Cl₂), while OH⁻ ions do not get oxidized under these conditions.

5. **Conclusion**: Since not all current-carrying ions are discharged at the electrodes during the electrolysis of NaCl, the statement is indeed true.

### Final Answer:
The statement is **True**.