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The hydrogen electrode is dipped in a solution of pH = 3 at 25 degree Celsius. The reduction potential of the electrode would be A) 0.177V B) 0.087V C) -0.177V D) 0.059V?
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The Hydrogen Electrode and Reduction Potential
pH of the Solution
Effect of pH on Reduction Potential
Standard Reduction Potential
Calculation of Reduction Potential
Answer: B) 0.088V
The hydrogen electrode is a reference electrode commonly used in electrochemical experiments. It consists of a platinum electrode immersed in a solution of hydrogen ions (H+). The potential of the hydrogen electrode is used as a reference against which the potentials of other electrodes can be measured. The reduction potential of the hydrogen electrode is defined as its tendency to gain electrons and be reduced.
pH of the Solution
The pH of a solution is a measure of its acidity or alkalinity. It is defined as the negative logarithm (base 10) of the hydrogen ion concentration in moles per liter (mol/L). A solution with a pH of 3 is acidic, indicating a high concentration of hydrogen ions.
Effect of pH on Reduction Potential
The reduction potential of the hydrogen electrode is affected by the pH of the solution. As the pH decreases (i.e., the solution becomes more acidic), the reduction potential of the hydrogen electrode increases. This is because the concentration of hydrogen ions in the solution increases, leading to a greater driving force for the reduction of hydrogen ions at the electrode surface.
Standard Reduction Potential
The standard reduction potential of the hydrogen electrode is defined as its reduction potential when the hydrogen ion concentration is 1 mol/L and the pressure of hydrogen gas is 1 bar. At 25 degrees Celsius, the standard reduction potential of the hydrogen electrode is 0.000 V.
Calculation of Reduction Potential
To calculate the reduction potential of the hydrogen electrode in a solution of pH 3 at 25 degrees Celsius, we can use the Nernst equation:
E = E° - (0.0592/n)log[H+]
Where E is the reduction potential, E° is the standard reduction potential, n is the number of electrons transferred in the half-reaction, and [H+] is the hydrogen ion concentration. In the case of the hydrogen electrode, n is 2 because two electrons are involved in the reduction of hydrogen ions.
Plugging in the values, we have:
E = 0.000V - (0.0592/2)log[10-3]
E = 0.000V - (0.0296)(-3)
E = 0.000V + 0.0888V
E = 0.0888V
Answer: B) 0.088V
Therefore, the reduction potential of the hydrogen electrode in a solution of pH 3 at 25 degrees Celsius is approximately 0.088V.
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The hydrogen electrode is dipped in a solution of pH = 3 at 25 degree Celsius. The reduction potential of the electrode would be A) 0.177V B) 0.087V C) -0.177V D) 0.059V?
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