A water sample is found to contain 96 ppm of `SO_4^(2-)` and 122 ppm of `HCO+3^(ɵ)` with `Ca^(2_)` ion as the only cation.
(a). Calculate the ppm of `Ca^(2+)` in water.

Explanation

To solve the problem of calculating the ppm of \( \text{Ca}^{2+} \) in water given the concentrations of \( \text{SO}_4^{2-} \) and \( \text{HCO}_3^{-} \), we can follow these steps:

### Step 1: Understand the relationship between the ions
The problem states that \( \text{Ca}^{2+} \) is the only cation present in the water sample, and it can react with both \( \text{SO}_4^{2-} \) and \( \text{HCO}_3^{-} \). The relevant reactions are:
1. \( \text{CaSO}_4 \rightarrow \text{Ca}^{2+} + \text{SO}_4^{2-} \)
2. \( \text{Ca(HCO}_3)_2 \rightarrow \text{Ca}^{2+} + 2 \text{HCO}_3^{-} \)

### Step 2: Calculate the moles of \( \text{SO}_4^{2-} \)
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