(a) The e.m.f. of the following cell at 298 K is 0.1745 V
`Fe(s) //Fe^(2+) (0.1 M) ////H^(+)(x M)//H_(2)(g) ("1 bar")//Pt (s)`
Given : `E_(Fe^(2+)//Fe)^(0) = - 0.44 V`
Calculate the `H^(+)` ions concentration of the solution at the electrode where hydrogen is being produced.
(b) Aqueous solution of copper sulphate and silver nitrate are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.

Explanation

### Step-by-Step Solution

#### Part (a)

1. **Identify the Cell Reaction**:
The cell reaction can be written as:
\[
\text{Fe}^{2+} + 2\text{H}^+ \rightarrow \text{H}_2 + \text{Fe}
...