113. Solving a chemistry problem

For a concentration element consisting of Cu metal in CuCl2 electrolyte solutions with concentrations of 0.2 and 0.05 mol / 1000 g, calculate the EMF at 298 K. Calculate the activity by the average activity coefficient taken from the reference book or (for dilute solutions) by ionic strength. For a cell composed of a hydrogen electrode in an HCl electrolyte solution with a concentration of 3 mol/1000 g and a calomel half-cell with a KCl concentration of 0.5 mol/1000 g, calculate the emf and pH of the solution containing the HCl electrolyte. Diffuse emf is ignored. At 298 K, the standard potential of the calomel electrode (2.00(Cl)=1) is 0.2812 CuCl2, and the ionic product of water is 1.0088*10-14. Find the dissociation constants of weak electrolytes in the reference book.