In the copper-silver cell, why must the Cu2+ and Ag+ solutions be kept in separate in containers?
If you have a Ag electrode dipping into the mixed solution and a Cu electrode dipping into the mixed solution, you get the battery reaction up front; i.e.,
Cu + 2Ag^+ ==> Cu^2+ + Ag(s)
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The Cu2+ and Ag+ solutions in a copper-silver cell must be kept in separate containers to prevent direct mixing of the two solutions. This separation is important for maintaining the integrity of the cell and ensuring its proper functioning. Here are a few reasons why the solutions must be kept separate:
1. Electrochemical reactions: In a copper-silver cell, oxidation of copper occurs at the anode, while reduction of silver occurs at the cathode. If the solutions mix, it would allow direct contact between these two electrode reactions, which can interfere with the overall cell reaction and potential difference.
2. Cross-contamination: If the Cu2+ and Ag+ solutions mix, some Cu2+ ions from the copper solution may react with Ag+ ions, leading to the formation of insoluble copper-silver compounds. This can reduce the concentration of Cu2+ and Ag+ ions in their respective solutions, affecting the cell's performance.
3. Short-circuiting: Mixing the solutions can lead to the formation of a conductive path, allowing direct electron flow between the anode and cathode without passing through the external circuit. This would effectively short-circuit the cell, preventing continuous production of electricity.
To avoid the above issues, it is crucial to keep the Cu2+ and Ag+ solutions in separate containers, with suitable barriers or salt bridges to allow ion migration while preventing direct mixing.
To understand why the Cu2+ and Ag+ solutions must be kept in separate containers in a copper-silver cell, we need to know some basic principles of electrochemistry.
In a copper-silver cell, the two half-reactions that occur are:
1. Cu2+(aq) + 2e- → Cu(s)
2. 2Ag(s) → 2Ag+(aq) + 2e-
In the first half-reaction, copper ions (Cu2+) are reduced to copper metal (Cu) at the cathode. In the second half-reaction, silver metal (Ag) gives up electrons and oxidizes to form silver ions (Ag+) at the anode.
If the Cu2+ and Ag+ solutions were allowed to mix in the same container, a redox reaction would occur between the silver and copper ions. The copper ions would reduce the silver ions, causing silver metal to be deposited on the copper electrode and preventing the desired redox reactions from taking place. This unwanted reaction would interfere with the functioning of the copper-silver cell.
Therefore, to ensure that the desired half-reactions occur independently and to prevent any unwanted reactions between the copper and silver ions, it is necessary to keep the Cu2+ and Ag+ solutions in separate containers. This allows the electrons to flow through an external circuit, generating a current, while maintaining the integrity of the individual half-reactions.