text: Without a membrane, the OH− ions produced at the cathode are free to diffuse throughout the electrolyte. As the electrolyte becomes more basic due to the production of OH−, less Cl2 emerges from the solution as it begins to disproportionate to form chloride and hypochlorite ions at the anode:
  Cl2 + 2 NaOH → NaCl + NaClO + H2O
  The more opportunity the Cl2 has to interact with NaOH in the solution, the less Cl2 emerges at the surface of the solution and the faster the production of hypochlorite progresses. This depends on factors such as solution temperature, the amount of time the Cl2 molecule is in contact with the solution, and concentration of NaOH.
  Likewise, as hypochlorite increases in concentration, chlorates are produced from them:
  3 NaClO → NaClO3 + 2 NaCl
  This reaction is accelerated at temperatures above about 60 °C. Other reactions occur, such as the self-ionization of water and the decomposition of hypochlorite at the cathode, the rate of the latter depends on factors such as diffusion and the surface area of the cathode in contact with the electrolyte.
  If current is interrupted while the cathode is submerged, cathodes that are attacked by hypochlorites, such as those made from stainless steel, will dissolve in unpartitioned cells.