“…where the quantity pH(0) = pH(eq) + 𝐴 is equal to the initial pH value of the solution, pH(eq) is the final pH value of the solution (this is the pH value for the solution that is in equilibrium with atmospheric carbon dioxide), 𝑡 is the time interval passed since the solution was prepared, and 𝜏 𝑠 is the relaxation time of the solution pH. The pH values of the solutions that were in equilibrium with atmospheric carbon dioxide, pH(eq), were determined under the following conditions: for water, the acid-base balance was equal to 7.00 at the temperature 𝑇 = 25 ∘ C and to 6.63 at 𝑇 = 50 ∘ C [1, 10,11]; for water in equilibrium with atmospheric carbon dioxide, pH = 5.63 at 𝑇 = 20 ∘ C [2, 12,13]; and, for the NaCl solution in equilibrium with atmospheric carbon dioxide, pH = 5.61 at 𝑇 = 20 ∘ C [2, 3]. In addition, the following assumptions were made: the difference between the pH of dilute aqueous NaCl solutions and the pH of water in equilibrium with atmospheric CO 2 is insignificant, and the temperature dependences of the pH of dilute NaCl solutions in equilibrium with atmospheric CO 2 are similar to that of the pH in water.…”