A calibration curve to show how the cell potential varies with [Cu2+] may be constructed. A plot of cell potential (in V, with the same sense as in question 1) versus log10[Cu2+] should yield a straight line. What is the slope of this line?
The answer should be -0.0591/2 but it s not correct!!
To determine the slope of the line in the calibration curve, you need to use the Nernst equation, which relates the cell potential of an electrochemical cell to the concentration of the species involved.
The Nernst equation is given as follows:
E = E° - (0.0591/n) * log10([Cu2+])
In this equation, E is the cell potential, E° is the standard cell potential (which depends on the half-reactions involved), [Cu2+] is the concentration of Cu2+ ions, and n is the number of electrons involved in the half-reaction (which can be obtained from the balanced chemical equation).
To create the calibration curve, you need to measure the cell potential at different concentrations of [Cu2+]. Plotting these values of cell potential (in V) against log10[Cu2+] should result in a straight line.
However, you mentioned that the given answer of -0.0591/2 is incorrect. It's possible that you have made a mistake in the calculations or that there is an error in the problem statement or answer key you are referring to. Double-check your calculations and the information provided in the question, including any relevant values of E°, n, and [Cu2+].
If you are still facing issues with the answer, please provide me with more details or any additional information given in the question, so I can assist you further.