A 12.0 M acid solution that contains 75.0% acid by mass has a density of 1.57 g/mL. What is the identity of the acid?
HCl (M = 36.5)
CH3CO2H (M = 60.0)
H3PO4 (M = 98.0)
Let the molecular weight of the acid be W.
Hence, 1000 ml 12.0 M acid solution contains 12W grams of pure acid.
Density of the solution = 1.57 g/ml
So, mass of 1000 ml of the solution = (1.57 * 1000) g = 1570 g
Again, mass of the acid in this solution = `75/100*1570` g = 1177.5 g
12W = 1177.5 g
`rArr` W = `1177.5/12` g= 98.125 g
Therefore, the identity of the acid is option (D) `H_3PO_4` (M = 98.0).