Electrolysis of Brine
Electrolysis of concentrated solution of NaCl
The electrolysis of brine results in hydrogen (H2) and chlorine gas. It is a large-scale process
used to manufacture chlorine (Cl2). The other useful co-product is sodium hydroxide (NaOH).
At the cathode, water is reduced to hydroxide ion and hydrogen gas. (The more reactive a metal, the less readily its ion is reduced on the electrode surface.)
At the anode, chloride (Cl-) ions are preferentially oxidized to chlorine.
Reduction at Cathode :
At the anode, chloride (Cl-) ions are preferentially oxidized to chlorine.
Reduction at Cathode :
2H2O(l) + 2e– = H2(g) + 2OH-(aq)
Oxidation at Anode :
2Cl–(aq) = Cl2(g) + 2e–
Overall reaction :
2H2O(l) + 2Cl–(aq) = 2OH–(aq) + H2(g) + Cl2(g)
(The sodium ions are spectator ions)
2Cl–(aq) = Cl2(g) + 2e–
Overall reaction :
2H2O(l) + 2Cl–(aq) = 2OH–(aq) + H2(g) + Cl2(g)
(The sodium ions are spectator ions)
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