Concentrated nitric acid used in the laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of solution is `1.504 g mL^(-1)` ?

Explanation

In 100 g of nitric acid solution, Mass of nitric acid = 68 g
Molar mass of HNO3 = 63 g `"mol"^(-1)`
`therefore 68 g HNO_3 = 68/63 ` mole = 1.079 mole
Density of solution = `1.504 g mL^(-1)`
Molarity of the solution = Mass of Solution/Density of solution
`= (1.079 )/(0.0665)M = 16.23 M`