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.

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

idk i’m struggling too

the increase of protons   hope this