A lead storage cell is discharged which causes the `H_(2)SO_(4)` electrolyte to change from a concentration of `34.6%` by weight (density `1.261gml^(-1)` at `25^(@)C`) to one of `27%` by weight. The original volume of electrolyte is one litre. Calculate the total charge released at anode of the battery. Note that the water is produced by the cell reaction as `H_(2)SO_(4)` is used up. over all reaction is.
`Pb(s)+PbO_(2)(s)+2H_(2)SO_(4)(l)to2PbSO_(4)(s)+2H_(2)O(l)`

Explanation

To solve the problem, we need to calculate the total charge released at the anode of a lead storage cell during its discharge. We will follow these steps:

### Step 1: Calculate the initial mass of H₂SO₄ in the electrolyte.
Given:
- Density of H₂SO₄ solution = 1.261 g/mL
- Volume of solution = 1 L = 1000 mL
- Concentration of H₂SO₄ = 34.6% by weight

...