(A) Calculate the molarity of commercially availableconcentrated nitric acid reagent given the following data:
Molecular formula: HNO3
Molar mass = 63.01 g/mol
Purity/Reagent Concentrate: 70.9% (w/w)
Specific gravity @20 degrees Celsius = 1.423
(Hint: Using the specific gravity, calculate the mass of oneliter solution. Of this mass, only 70.9% is pure HNO3; theremainder being water).
(B) To make 212 mL of 0.15 M solution of nitric acid, whatvolume of the concentrated nitric acid will be needed?
Final answer: (A) Molarity of concentrated HNO3 = _ M. (B)Volume of conconcentrated HNO3 required = _ m
