Question

Рассчитать pH водородного электрода,погруженного в 0,01 м раствор соляной кислоты

Answer 1

[H+]=[HCl]=0,01 M
pH=-lg[H+]=-lg0,01=2

Answer 2

Calculating the pH of a Hydrogen Electrode in 0.01 M Hydrochloric Acid Solution

To calculate the pH of a hydrogen electrode in a 0.01 M hydrochloric acid solution, we can use the Nernst equation, which relates the measured electrode potential to the concentration of the ions in the solution. The Nernst equation for the hydrogen electrode is given by:

E = E° + (RT/nF) * ln([H+])

Where: - E is the measured electrode potential - E° is the standard electrode potential - R is the ideal gas constant (8.314 J/(mol·K)) - T is the temperature in Kelvin - n is the number of electrons transferred in the redox reaction - F is the Faraday constant (96,485 C/mol) - [H+] is the concentration of hydrogen ions in the solution

The standard electrode potential for the hydrogen electrode is 0.0 V at standard conditions.

Calculation

Given that the concentration of the hydrochloric acid solution is 0.01 M, we can use the Nernst equation to calculate the pH of the hydrogen electrode in this solution.

Using the Nernst equation: E = 0.0 V + (8.314 J/(mol·K) * 298 K / (2 * 96485 C/mol)) * ln(0.01)

Calculating the value of E using the given concentration of hydrogen ions: E ≈ 0.0 V + (0.03448) * ln(0.01) E ≈ 0.0 V + (0.03448) * (-4.605) E ≈ 0.0 V - 0.1589 V E ≈ -0.1589 V

The pH of the solution can be calculated using the formula: pH = -log[H+]

Given that the concentration of hydrogen ions in the solution is 0.01 M: pH = -log(0.01) pH ≈ 2

Therefore, the pH of the hydrogen electrode in the 0.01 M hydrochloric acid solution is approximately 2.