Commercial hydrochloric acid is 38 percent HCl by mass. The density is of this aqueous solution is 1.19g/cm^3?
What is the molarity of hydrochloric acid in this solution?
What mass of solution is required to give 796 milligrams of hydrochloric acid?
- Roger the MoleLv 75 months agoFavorite Answer
(1.19 g/cm^3) x (1000 cm^3 / 1 L) x (0.38) / (36.4611 g HCl/mol) = 12.4 mol/L HCl
[I'm not convinced aqueous HCl exists in such a high concentration, but that's what the given numbers say.]
(796 mg HCl) / (0.38) = 2095 mg solution