You are provided with `500mL` of hard water, containing `0.005 mol` of `CaC1_(2)` and two `H_(2)SO_(4)` samples of `0.001M` and `0.02M` concentration. Which one or both or none can be used for precipitating `Ca^(2+)` ions.
`K_(sp)` of `CaSO_(4) = 2.4 xx 10^(-4)`.

Explanation

To determine whether either of the two H₂SO₄ samples can precipitate Ca²⁺ ions from hard water containing CaCl₂, we will follow these steps:

### Step 1: Calculate the concentration of Ca²⁺ ions in the hard water.
Given:
- Volume of hard water = 500 mL = 0.5 L
- Moles of CaCl₂ = 0.005 mol

The concentration of Ca²⁺ ions can be calculated using the formula:
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