MCQ
In the electrolysis of $\text{NaCl:}$
- ✓$Cl ^{-}$is oxidised at anode.
- B$Cl ^{-}$ is reduced at anode.
- C$Cl ^{-}$ is reduced at cathode.
- D$Cl ^{-}$ is neither reduced nor oxidised.
✓
Answer
Correct option: A.
$Cl ^{-}$is oxidised at anode.
Electrolysis of an aqueous solution of table salt $(\text{NaCl}$, or sodium chloride$)$ produces aqueous sodium hydroxide and chlorine, although usually only in minute amounts. $\text{NaCl} ($aq$)$ can be reliably electrolysed to produce hydrogen. Hydrogen gas will be seen to bubble up at the cathode, and chlorine gas will bubble at the anode.
As the electricity from the battery passes through and between the electrodes, the water splits into hydrogen and chlorine gas, which collect as very tiny bubbles around the electrode tips. Hydrogen collects around the cathode and chlorine gas collects around the anode.
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