ElectrochemistryMedium
Question
A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of 10−6 M hydrogen ions. The EMF of the cell is 0.118 V at 25°C. The concentration of hydrogen ions at the positive electrode is
Options
A.10−6 M
B.10−3 M
C.10−4 M
D.10−5 M
Solution
Net cell reaction: $H^{+}(C = ?) \rightleftharpoons H^{+}\left( 10^{- 6}\text{ M} \right)$
$E_{cell} = - \frac{0.059}{1}.\log\frac{10^{- 6}}{c} = 0.118 \Rightarrow C = 10^{- 4}\text{ M}$
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