An electric current is passed through a solution of (i) silver nitrate, (ii) solution of 10 g of copper sulphate `(CuSO_(4).5H_(2)O)` crystals in 500 mL of water, platinum electrodes being used in each case. After 30 minutes it was found that 1.307 g of silver has been deposited. What was the concentration of copper, expressed as grams of copper per litre in the copper sulphate after electrolysis ?

Explanation

To solve the problem, we will follow these steps:

### Step 1: Determine the equivalent weight of silver (Ag)
The equivalent weight of silver (Ag) can be calculated using its atomic mass. The atomic mass of silver is approximately 107.87 g/mol. Since silver has a valency of 1, its equivalent weight is:

\[ \text{Equivalent weight of Ag} = \frac{\text{Atomic mass of Ag}}{\text{Valency}} = \frac{107.87}{1} = 107.87 \, \text{g/equiv} \]
...