Amount of phosphorus in 1L water = 3.4 mg
Total volume of water = 10000 cubic m = 10000000 L
Amount of phosphrus in total water = 34000 g
Moles of phosphorus = Given Wt / Molecular Wt
= 34000 g/ 96 g/mol
= 354.2 mol
Now,
As per the balanced equation 3 mol HPO4 (2-) reacts with 5 mol of Ca(OH)2
3 mol HPO4 (2-) : 5 mol Ca(OH)2
354.2 mol : 590 mol Ca(OH)2
The Ca(0H)2 solution contains 8.5 g Ca(OH)2 in 1L solution.
Moles of Ca(OH)2 = 8.5 g/74g/mol = 0.115 mol
THus, 0.115 mol are present in 1L of solution.
Hence,
Molarity of solution = 0.115 M
Molarity of solution = Moles / Volume (L)
So,
0.115 M = 590 mol / Volume
Volume = 5130.5 L
Correct option : C
+60t 13th using the following reaction 2 -> CaOH(pan (5) 5 Ca (OHly +3 HP What...