Nernest eq is
E cell = Eo cell - ( 0.059/n) log Q
where Q = 1 /[H+]^2 , given pH = 6.75 , [H+] = 10^ -6.75 = 1.78 x 10^ - 7 M
Q = ( 1/ 1.78x10^-7)^2 = 3.156 x 10^ 13
n = number of electrons involved per reduction = 2
Eo cell = 0 for H+/H2 reduction
E cell = 0 - ( 0.059/2) log ( 3.156x10^13)
= -0.37 V
If the potential of a hydrogen electrode based on the half-reaction 2 H^+ (aq) + 2...
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help please
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