Acids and bases can serve as electrolytes in water electrolysis besides sodium chloride.
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Reference literature confirms that most soluble acids and bases function as electrolytes, which are necessary additions for water electrolysis since pure water is an insulator.
Electrolyte
An electrolyte is a chemical that conducts electrical current. It is used in batteries to make the ions flow, producing current. Electrolytes ionize when dissolved in suitable solvents such as water. Most soluble salts, acids, and bases are electrolytes.
An electrolyte used in "electrolytic cells" carries the ions between the electrodes of the cell. Electrolytic cells may be used to extract constituent elements and compounds contained in the solution.
A correct concentration of electrolytes is important to physiology.
Related pages
- Cathode, includes anode
- Electrolysis
For example, if we try to electrolyze a solution of sodium chloride, hydrogen is produced at the cathode instead of sodium:
| | H2O + 2 e– → H2(g) + 2 OH– | E =+0.41 V ([OH–] = 10-7 M) |
| | Cl– → ½ Cl2(g) + e– | E° = –1.36 V |
| | Cl– + H2O → 2 H2(g) + ½ Cl2(g) + 2 OH– | E = –0.95 V |
[This illustration is taken from the excellent Purdue University Chemistry site]Reduction of Na+ (E° = –2.7 v) is energetically more difficult than the reduction of water (–1.23 V), so in aqueous solution the latter will prevail. Electrolysis of salt ("brine") is carried out on a huge scale and is the basis of the chloralkali industry. Electrolysis of water
Pure water is an insulator and cannot undergo significant electrolysis without adding an electrolyte. If the object is to produce hydrogen and oxygen, the electrolyte must be energetically more difficult to oxidize or reduce than water itself.
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