A galvanic cell is constructed with Ag+?Ag and Fe3+?Fe2+ electrodes. Find the concentration of Ag+ at which the emf of the cell is zero at equimolar concentration of Fe2+ and Fe3+. E*Ag+/Ag= 0.80V and E*Fe3+/Fe2+= 0.77V Share with your friends Share 11 Geetha answered this The given cell isAnode : Fe2+ → Fe3+ + e-Cathode: Ag+ + e- → Ag--------------Fe2+ + Ag+→ Fe3+ + Ag------------E0 = EFe2+/Fe3+0 + EAg+/Ag0 = - 0.77 + 0.80 = 0.03 VGiven that E =0E = E0 - 0.0591n log [RHS][LHS]becomesE0 = 0.0591n log [RHS][LHS] 0.03 = 0.05911 log [Fe3+] [Ag][Fe2+] [Ag+]0.03 = 0.05911 log 1 [Ag+] {since the concentration of [Ag]= 1 and [Fe2+] = [Fe3+] }0.03 = 0.05911 log [Ag+]-10.03 = - 0.0591 log [Ag+] log [Ag+] = - 0.03 0.0591 = - 0.5076[Ag+] = A.log [- 0.5076] = 0.3107 33 View Full Answer