Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or)E=E^@ - (0.0591)/(n) log Q E^@= Standard potential and 'Q' is the reaction quotient. What is the reduction potential of a hydrogen electrode in an aqueous solution containing 0.1 M NH_4OH,(Kb=10^(-5)), ?

Nernst equation gives the variation of potential of an electrode based

1.	Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or)E=E^@ - (0.0591)/(n) log Q E^@= Standard potential and 'Q' is the reaction quotient. What is the reduction potential of a hydrogen electrode in an aqueous solution containing 0.1 M NH_4OH,(Kb=10^(-5)), ?
Answer» 0.02 V 0.03 V 0.06 V 0.01 V Solution :`E_1 = E^(0) + (0.06)/(3) LOGC , E_2 = E^(0) +(0.06)/(3) LOG ((C)/(10))` ` (E_2 -E_1) = (0.06)/(3) [log""((C)/(60))-logC] = 0.02 log((C)/(10) xx (1)/(C)) = 0.02 xx log 10^(-1) = -0.02V`