`10mL` of `0.3M Na_(2)SO_(4)` are mixed with `20mL` solution having initially `0.1M Ca^(2+)` and `0.1M Sr^(2+)` in it. Calculate the final `[Ca^(2+)], [Sr^(2+)]` and `[SO_(4)^(2-)]` in solution? Given `K_(sp) SrSO_(4) = 7.6 xx 10^(-7)` and `K_(sp) CaSO_(4) = 2.4 xx 10^(-5)`.

Explanation

To solve the problem, we need to calculate the final concentrations of \( \text{Ca}^{2+} \), \( \text{Sr}^{2+} \), and \( \text{SO}_4^{2-} \) ions after mixing the two solutions. Here's a step-by-step breakdown of the solution:

### Step 1: Calculate the initial concentrations of the ions after mixing
1. **Volume of Na\(_2\)SO\(_4\) solution**: 10 mL
2. **Concentration of Na\(_2\)SO\(_4\)**: 0.3 M
3. **Volume of Ca\(^{2+}\) and Sr\(^{2+}\) solution**: 20 mL
4. **Concentration of Ca\(^{2+}\)**: 0.1 M
5. **Concentration of Sr\(^{2+}\)**: 0.1 M
...