In electrolytic refining, the impure metal is made the anode, while a thin strip of pure metal is made the cathode. A solution of the metal salt serves as the electrolyte. When a current is passed through the electrolyte, the impure metal at the anode dissolves into the electrolyte, while an equivalent amount of pure metal is deposited on the cathode.
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In electrolytic refining, impure metal is made the anode, and a pure metal sheet acts as the cathode in an electrolytic cell. The metal-containing electrolyte solution allows metal cations from the anode to dissolve. These metal cations are then reduced at the cathode, forming a layer of pure metal. Simultaneously, impurities remain at the anode or fall into the electrolyte. This process is iteratively repeated to enhance purity. Electrolytic refining is vital for metals like copper, aluminum, and zinc, ensuring the removal of trace elements and impurities, resulting in high-purity metals suitable for various industrial applications.
Electrolytic refining is a process used to purify metals such as copper, silver, and gold. In this process, an electrolyte solution containing metal ions is subjected to an electric current. Two electrodes, an anode (impure metal) and a cathode (pure metal), are immersed in the electrolyte. When a direct current is passed through the cell, metal ions migrate from the anode to the cathode. At the cathode, metal ions are reduced and deposit as pure metal, while impurities either dissolve into the electrolyte or settle as a sludge. This process yields high-purity metals essential for various industrial applications.