Phosphorus occurs naturally in the form of fluorapatite, CaF2 ∙ 3Ca3 (PO4) 2. The dot indicates 1 part CaF2 to 3 parts Ca3 (PO4) 2. This mineral is reacted with an aqueous solution of H2SO4 in the preparation of a fertilizer. The products are phosphoric acid, hydrogen fluoride, and gypsum, CaSO4 ∙ 2H2O. Write the balanced equation describing this process.

Question

Arely Robinson

Chemistry

15 April, 01:34

Phosphorus occurs naturally in the form of fluorapatite, CaF2 ∙ 3Ca3 (PO4) 2. The dot indicates 1 part CaF2 to 3 parts Ca3 (PO4) 2. This mineral is reacted with an aqueous solution of H2SO4 in the preparation of a fertilizer. The products are phosphoric acid, hydrogen fluoride, and gypsum, CaSO4 ∙ 2H2O. Write the balanced equation describing this process.

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Answers (1)

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Kamari Humphrey · Answer 1

CaF2 * 3Ca3 (PO4) 2 + 10 H2SO4 + 20 H2O ⇔6 H3PO4 + 2 HF + 10 CaSO4 * 2H2O

Explanation:

We have CaF2 * 3Ca3 (PO4) 2 that will react with an aqueos solution of H2SO4

This will form the following product H3PO4 + HF and CaSO4 * 2H2O

CaF2 * 3Ca3 (PO4) 2 + 10 H2SO4 + 20 H2O ⇔6 H3PO4 + 2 HF + 10 CaSO4 * 2H2O

We have on both sides:

10x Ca

2x F

6x P

84x O

40x H

10x S

The reaction cannot be more simplified