For the electrode Pt, H2 (1 atm) | H+ (aq) (XM), the reduction electrode potential at 25 degrees C os -0.34V. Write the electrode reaction equation and calculate the value of X. How will you deduce the pH of the solution from this result Share with your friends Share 36 Geetha answered this The given cell isPt, H2 (1 atm) // H+(aq) (X M)At anode : 12H2 → H+ + e-At Cathode : H+ + e- →12H2Net cell reaction is12H2(1 atm) → H+(X M) + e-The Emf of the cell at std condition = Eox0 + ERed0 = 0According to Nernst equation,E = E0 - 0.0592n log [anode][cathode]-0.34 = 0 - 0.05921 log 1[H+]-0.34 = -0.0592 (log 1 -log [H+]-0.34 = -0.0592 ( -log [H+])-0.34 = -0.0592 pHpH = 0.340.0592 = 5.74 25 View Full Answer