Electrolytic Production of Chlorate

NaCl + 3H₂O → NaClO₃ + 3H₂

Overview

Electrolysis of hot NaCl solution without a membrane allows chlorine produced at the anode to react with hydroxide from the cathode, forming hypochlorite that disproportionates to chlorate at 70–80°C. Sodium chlorate (NaClO₃) is the precursor to chlorine dioxide (ClO₂), the dominant bleaching agent in modern paper mills.

Participants

Role	Substance	Coefficient	State
Reactant	Sodium Chloride NaCl	1	(aq)
Reactant	Water H₂O	3	(l)

Everyday Example

The white paper in your books and notebooks was bleached using chlorine dioxide derived from electrolytically produced sodium chlorate.

Industrial Importance

About 3.6 million tonnes of sodium chlorate are produced annually, primarily for pulp bleaching, herbicides, and water treatment.

Properties

Type: Electrochemical
Reversible: No
Energy: Endothermic
ΔH: 590.0 kJ/mol

Related Reactions

Alkaline Battery Discharge Anodizing of Aluminum Cathodic Protection (Zinc Sacrificial Anode) Chlor-Alkali Electrolysis Chrome Electroplating Copper Electroplating Daniell Cell (Zinc-Copper Galvanic Cell) Electrochemical CO₂ Reduction to CO Electrochemical Machining (ECM) Electrolysis of Molten NaCl (Downs Process)

Frequently Asked Questions

What is the equation for Electrolytic Production of Chlorate?

The balanced equation is: NaCl + 3H₂O → NaClO₃ + 3H₂.

What type of reaction is Electrolytic Production of Chlorate?

Electrolytic Production of Chlorate is a electrochemical reaction.

Is Electrolytic Production of Chlorate exothermic or endothermic?

Electrolytic Production of Chlorate is endothermic (absorbs energy). The enthalpy change (ΔH) is 590.0 kJ/mol.