If 20 ml of `0.5M Na_(2).SO_(4)` is mixed with `50ml` of `0.2M H_(2)SO_(4)` & 30 ml of `0.4M Al_(2)(SO_(4))_(3)` solution. Calculate `[Na^(+)],[H^(+)].[SO_(4^(2-))],[Al^(3+)]`. [Assuming `100%` dissociation]

Explanation

To solve the problem, we need to calculate the concentrations of the ions present in the mixed solution after mixing the given volumes and molarities of the solutions. We will follow these steps:

### Step 1: Calculate the number of moles of each compound.

1. **For Na₂SO₄:**
- Molarity (M) = 0.5 M
- Volume (V) = 20 mL = 0.020 L
- Number of moles (n) = M × V = 0.5 × 0.020 = 0.01 moles
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