Phosphorus occurs in nature in the form of stable phosphates. (Animal bones also contain calcuim phosphate (58%)).The important minerals are:
(i)Phosphorite, `Ca_3(PO_4)_2` (ii)Chloraptite,`Ca_3(PO_4)_2CaCl_2`
(iii)Fluoraptite, `Ca_3(PO_4)_2CaF_2`
There are some depoists of nitrates and phosphates in earth's crust.Nitrates are more soluble in water Nitrates are difficult to reduce under the laboratory conditions but microbes do it easily.Compounds of phosphorus and nitrogen are used as fertilizer.
`Ca_3(PO_4)_2CaF_2+H_2SO_4to(X)+HF`
X is -

Options

A. Triple super phosphate
B. Super phosphate
C. Phosphorite
D. Vivianite

Explanation

To solve the question, we need to determine the product \( X \) formed when fluorapatite \( \text{Ca}_3(\text{PO}_4)_2\text{CaF}_2 \) reacts with sulfuric acid \( \text{H}_2\text{SO}_4 \).

### Step-by-Step Solution:

1. **Identify the Reactants**:
The reactants are fluorapatite \( \text{Ca}_3(\text{PO}_4)_2\text{CaF}_2 \) and sulfuric acid \( \text{H}_2\text{SO}_4 \).

2. **Write the Balanced Reaction**:
The reaction can be written as:
\[ \text{Ca}_3(\text{PO}_4)_2\text{CaF}_2 + \text{H}_2\text{SO}_4 \rightarrow X + \text{HF} \]

3. **Determine the Products**:
When fluorapatite reacts with sulfuric acid, it typically produces calcium hydrogen phosphate and calcium sulfate along with hydrofluoric acid. The balanced reaction can be represented as:
\[ \text{Ca}_3(\text{PO}_4)_2\text{CaF}_2 + 7\text{H}_2\text{SO}_4 \rightarrow 3\text{Ca(H}_2\text{PO}_4)_2 + 7\text{CaSO}_4 + 2\text{HF} \]

4. **Identify \( X \)**:
From the balanced equation, we see that \( X \) corresponds to the product \( 3\text{Ca(H}_2\text{PO}_4)_2 \), which is known as superphosphate.

5. **Conclusion**:
Therefore, \( X \) is \( 3\text{Ca(H}_2\text{PO}_4)_2 \) or superphosphate.

### Final Answer:
\( X \) is superphosphate \( 3\text{Ca(H}_2\text{PO}_4)_2 \).

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