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Electrode potential of the half Pt(s)|Hg...

Electrode potential of the half Pt(s)|Hg(l)|`Hg_(2)Cl_(2)(s)`|`Cl^(-)(aq)` can be incresed by :

A

Increasing `[Cl^(-)]`

B

decreasing `[Cl^(-)]`

C

Increasing `Hg_(2)Cl_(2)(s)`

D

decreasing `Hg(l)`

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding how to increase the electrode potential of the half-cell Pt(s)|Hg(l)|Hg2Cl2(s)|Cl^(-)(aq), we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Half-Cell Reaction**: The half-cell reaction for the calomel electrode can be represented as: \[ \text{2 Hg(l) + 2 Cl}^- \rightleftharpoons \text{Hg}_2\text{Cl}_2(s) + 2 e^- \] In this reaction, mercury (Hg) is oxidized to mercurous chloride (Hg2Cl2), and chloride ions (Cl^-) are involved. 2. **Understand the Role of Concentration**: The electrode potential can be influenced by the concentrations of the reactants and products involved in the half-cell reaction. According to the Nernst equation, the potential of the cell can be expressed as: \[ E = E^0 - \frac{0.0591}{n} \log \left( \frac{[\text{Products}]}{[\text{Reactants}]} \right) \] Here, \(E^0\) is the standard electrode potential, \(n\) is the number of electrons transferred, and the concentrations of the products and reactants are taken into account. 3. **Apply the Nernst Equation**: For the calomel electrode, the Nernst equation can be simplified to: \[ E = E^0 - \frac{0.0591}{2} \log \left( \frac{1}{[\text{Hg}]^2 \cdot [\text{Cl}^-]^2} \right) \] Since the concentration of the solid Hg2Cl2 is considered constant (1), we focus on the concentrations of Hg and Cl^-. 4. **Analyze the Effect of Concentration**: - Increasing the concentration of chloride ions \([Cl^-]\) will decrease the logarithmic term, which in turn increases the electrode potential \(E\). - Conversely, increasing the concentration of mercury \([Hg]\) would also have a similar effect. 5. **Conclusion**: Therefore, to increase the electrode potential of the half-cell, we can increase the concentration of chloride ions \([Cl^-]\). This is the correct answer to the question. ### Final Answer: The electrode potential of the half-cell can be increased by increasing the concentration of Cl^- ions. ---
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