A cell is containing two H electrodes. The negative electrode is in contact with a solution of `10^(-6)MH^(+)` ion. The e.m.f. of the cell is `0.118` volt at `25^(@)C` . Calculate `[H^(+)]` at positive electrode.

Explanation

To solve the problem, we need to calculate the concentration of hydrogen ions \([H^+]\) at the positive electrode of a galvanic cell containing two hydrogen electrodes. The negative electrode is in contact with a solution of \(10^{-6} M H^+\) ions, and the e.m.f. of the cell is given as \(0.118\) volts at \(25^\circ C\).

### Step-by-Step Solution:

1. **Identify the Reactions at the Electrodes:**
- At the negative electrode (anode), the oxidation reaction occurs:
\[
2H_2 \rightarrow 2H^+ + 2e^-
...