The potential of hydrogen electrode of pH = 10 with respect to standard hydrogen electrode is

Options

A. `-0.0591V`
B. `-0.591V`
C. 0.2V
D. 0

Answer

B

Explanation

For, hydrogen electrode
`pH = 10 [H^(+)] = 10^(-10) M H^(+) + e^(-) = (1)/(2) H_(2)`
`E_("cell") = E^(@) - (0.0591)/(1) "log" ([H_(2)])/([H^(+)])`
`E^(@) = 0, log H_(2) = 0` because
`E_("cell") = - (0.0591)/(1) log ((1)/(10^(-10))) - 0.0591 xx 10`
`E_("cell") = - 0.591V`