Electrolysis of aqueous solution
Electrolysis of an aqueous solution involves the process of passing an electric current through the solution. This process results in the decomposition of the solute or solvent molecules into their respective ions.
During electrolysis, two electrodes are immersed in the aqueous solution. The electrode connected to the positive terminal of the power source is called the anode, while the electrode connected to the negative terminal is called the cathode.
At the anode, oxidation occurs, resulting in the release of electrons. This process can take place with either water or the solute. If water is oxidized, oxygen gas (O2) is produced, and hydrogen ions (H+) are formed.
At the cathode, reduction occurs, where the positively charged ions in the solution are reduced. This process depends on the nature of the solute. For example, if the solute is a metal ion, such as copper (Cu2+), the copper ions are reduced to solid copper metal (Cu). On the other hand, if the solute is a non-metal ion, such as chloride (Cl-), the chloride ions are reduced to chlorine gas (Cl2).
Overall, the electrolysis of an aqueous solution results in the separation of the solute or solvent molecules into their respective ions, leading to the formation of new substances at the anode and cathode. This process is commonly used in various applications, such as electroplating, water splitting, and industrial production of chemicals.