The cell potential of the following electrochemical cell is determined by using an unspecified concentration of acid.Calculate the pH of the acid solution,given that the measured cell potential is -0.431 V and the anode reduction potential (E°) is 0.222 V at 25 °C.
Ag(s) | AgCl(s) | Cl−(aq,1.0 M) || H⁺(aq) | H₂(g,1.0 atm) | Pt(s)

Question

Quizplus · Accepted Answer

The cell potential (E_cell) can be calculated using the Nernst equation: E_cell = E° - (RT/nF)lnQ, where E° is the standard reduction potential, R is the gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin (298K for 25°C), n is the number of moles of electrons transferred in the reaction, F is the Faraday constant (96485 C/mol), and Q is the reaction quotient. Given that the measured cell potential is -0.431 V and the standard reduction potential is 0.222 V, we can rearrange the Nernst equation to solve for Q, which is related to the concentration of hydrogen ions ([H+]) in the solution. The pH is then calculated using the formula pH = -log[H+]. The correct calculation leads to a pH of 3.53.

The Cell Potential of the Following Electrochemical Cell Is Determined