Electroplating is plating to certain metal with other metal that is usually more durable from corrosion or stronger than original metal. The process itself use of electrochemical by which metal is deposited on the origin metal through the chemical bath.
Usually using electrode pole that is connected to the negative and the other to the positive pole. Electrode on the negative pole is called as anode and electrode that connected to positive charge is called as cathode. Metal on the solution form will turn to positive ion and on the electrochemical process this ion will attract to negative electrode or to anode and will plate anode. So metal that will be plated is placed on the anode position.
Electroplating is done in a plating bath which is usually a non-metallic tank like plastic or glass. The tank is filled by metal solution, which the metal kind will plate the anode. The The anode is a workpiece, this substrate to be plated. This is connected to the negative terminal of the power supply. Power supply is well regulated to minimize ripples as well to deliver a steady predictable current, under varying loads such as those found in plating tanks.
As current is applied, positive metal ions from the solution are attracted to the negatively charged anode and deposit on anode. As a replenishment of these deposit ions, the metal from cathode will dissolve and goes into the solution and make the ionic potential balance.
In the case using of noble metal like gold as cathode is not sacrificial (gold is not dissolve easily), but it is made out of material that does not dissolve in the electrolyte such as titanium. Practically it should be apply to the Electroplating Legal Patent for large scale production.
Electrochemical Theory:
Actually electroplating is based on the Faraday’s Laws that state as follows:
The weight of a substance formed at an electrode is proportional to the amount of current passed through the cell.
The weights of different substances produced at an electrode by the same amount of current are proportional to their equivalent weights.
Equivalent weight in an oxidation-reduction reaction is = molar weight of the compound / algebraic change in oxidation number of the atom that is oxidized or reduced.
2 FeCl2 + Cl2 ──→ 2 FeCl3
Fe valence is change on the reaction from +2 to +3. However on the reaction will:
Mn + FeSO4 ──→ Fe + MnSO4
Usually using electrode pole that is connected to the negative and the other to the positive pole. Electrode on the negative pole is called as anode and electrode that connected to positive charge is called as cathode. Metal on the solution form will turn to positive ion and on the electrochemical process this ion will attract to negative electrode or to anode and will plate anode. So metal that will be plated is placed on the anode position.
Electroplating is done in a plating bath which is usually a non-metallic tank like plastic or glass. The tank is filled by metal solution, which the metal kind will plate the anode. The The anode is a workpiece, this substrate to be plated. This is connected to the negative terminal of the power supply. Power supply is well regulated to minimize ripples as well to deliver a steady predictable current, under varying loads such as those found in plating tanks.
As current is applied, positive metal ions from the solution are attracted to the negatively charged anode and deposit on anode. As a replenishment of these deposit ions, the metal from cathode will dissolve and goes into the solution and make the ionic potential balance.
In the case using of noble metal like gold as cathode is not sacrificial (gold is not dissolve easily), but it is made out of material that does not dissolve in the electrolyte such as titanium. Practically it should be apply to the Electroplating Legal Patent for large scale production.
Electrochemical Theory:
Actually electroplating is based on the Faraday’s Laws that state as follows:
The weight of a substance formed at an electrode is proportional to the amount of current passed through the cell.
The weights of different substances produced at an electrode by the same amount of current are proportional to their equivalent weights.
Equivalent weight in an oxidation-reduction reaction is = molar weight of the compound / algebraic change in oxidation number of the atom that is oxidized or reduced.
2 FeCl2 + Cl2 ──→ 2 FeCl3
Fe valence is change on the reaction from +2 to +3. However on the reaction will:
Mn + FeSO4 ──→ Fe + MnSO4