The simplicity with which the phenomenon of electrolysis is replicated, even in its most basic form, is perhaps proportional to its importance in today's society. In short, electrolysis involves the transformation of electrical energy into chemical energy, precisely the opposite of what occurs in an ordinary battery of a TV remote control.
Etymologically defined as "decomposition by electricity", electrolysis can take various forms, but there is always a common denominator: in order for it to occur, the process must be artificially supplied with continuous electrical current – it is therefore a provoked reaction, not a spontaneous one.
This flow of energy travels through the electrodes of an electrolytic cell, forcing electrons to participate in reactions caused by oxidation at one of the electrodes (the anode) and reduction at the other electrode (the cathode). It is through this applied electrical discharge that it is possible to decompose molecules and obtain the desired products.
Electrolysis is divided into two essential types: igneous electrolysis, in which the liquid substance is molten, without the presence of water, and aqueous electrolysis, in which a substance is dissolved in water, forming an electrolytic solution.
In an aqueous medium, if we carry out electrolysis of water we can separate oxygen from hydrogen. But if we add salt (sodium chloride) to water, resulting in brine, then it is already possible to obtain chlorine, an essential element in many activities, or even to guarantee a basic need such as drinking water.
But that's not all: from this process, called the chloralkali process, it is also possible to obtain sodium hydroxide (commonly known as caustic soda), sodium hypochlorite (a powerful disinfectant known as bleach), hydrochloric acid (commercially known as muriatic acid), as well as hydrogen, which many consider to be the energy of the future. In short, it is a set of derivatives with extensive application in domestic and industrial contexts.