The potential of an electrochemical reaction depends on the concentration of reduced and oxidised species.The change from the standard potential can be calculated with the Nernst equation.For a glass electrode, this results in:E = Ecell - 0.059 x pH VoltsYou find that the potential of a solution with unknown pH is 0.177 V higher than the potential of the calibration buffer at pH 7.What is the pH of the solution? 2 10 4 8 6
Question
The potential of an electrochemical reaction depends on the concentration of reduced and oxidised species.The change from the standard potential can be calculated with the Nernst equation.For a glass electrode, this results in:E = Ecell - 0.059 x pH VoltsYou find that the potential of a solution with unknown pH is 0.177 V higher than the potential of the calibration buffer at pH 7.What is the pH of the solution? 2 10 4 8 6
Solution
To find the pH of the solution, we can rearrange the Nernst equation to solve for pH:
pH = (Ecell - E) / 0.059
Given that the potential of the solution is 0.177 V higher than the potential of the calibration buffer at pH 7, we can substitute these values into the equation:
pH = (0.177 V) / 0.059
Solving this equation gives a pH of approximately 3. Therefore, the pH of the solution is closest to 4 from the given options.
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