Water is oxidized and reduced at both electrodes
<h3>Further explanation
</h3>
Electrolysis utilizes electrical energy to carry out non-spontaneous redox reactions. The ions in the solution flowed by an electric current will move toward the electrode opposite the charge.
The negative ions from the solution will move towards the positive electrode, and release electrons around the positive electrode (oxidation occurs) and electrons flow to the negative pole
While around the negative electrode electron binding occurs and a reduction reaction occurs
the reaction at the cathode:
1. the reduced active metal is water, other than that the metal will be reduced
2. H⁺ of the acid will be reduced
For reactions in anode:
1. if the electrodes are not inert then the metal is oxidized
2. If inert then:
a. OH⁻ from the base will be oxidized
b. The halogen metal will oxidize
- Na⁺ (cathode)⇒metal group 1 and 2 ⇒ H₂O reduced
2H₂O(l)+2e⁻⇒ H₂(g)+2OH⁻(aq)
- SO₄²⁻ (anode)⇒acid ion(oxyacid)⇒H₂O oxidized
2H₂O(l)⇒4H⁺(aq)+O₂(g)+4e⁻
