Question

Phosphorus occurs naturally in the form of fluorapatite, CaF2·3 Ca3(PO4)2, the dot indicating 1 part CaF2 to 3 parts Ca3(PO4)2. This mineral is reacted with an aqueous solution of sulfuric acid in the preparation of a fertilizer. The products are phosphoric acid, hydrogen fluoride, and gypsum, CaSO4·2 H2O. Balance the chemical equation describing this process. (Type your answer using the format CO2 for CO2.) CaF2·3 Ca3(PO4)2(s) + (aq) + (l) (aq) + HF(aq) + CaSO4·2 H2O(s)

Answer 1

CaF2.3Ca3(PO4)2 (s) + H2SO4(aq) ----> H3PO4(aq) + HF(aq) + CaSO4.2H2O(s) is the equation as per given words. Now we need to balance it.

First we balanace Ca by using coeffients.

CaF2.3Ca3(PO4)2 (s) + H2SO4(aq) ---> H3PO4(aq) + HF(aq) + 10CaSO4.2H2O(s)

now SO4 and PO4 units should be balanaced

CaF2.3Ca3(PO4)2(s) + 10 H2SO4(aq) ---> 6H3PO4(aq) + HF(aq) + 10CaSO4.2H2O(s)

finally we are left to balance H and F , we see if we put 2 coeffient infront of HF equation is fully balanced. we include 2H2O in reactansts side since we had aqueos medium

The final balanced eqaution is

CaF2.3Ca3(PO4)2(s) + 10 H2SO4(aq) + 2H2O(l) ----> 6H3PO4(aq) + 2HF(aq) + 10CaSO4.2H2O(s)