Concentrated nitric acid used in 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 the solution is `1.50g mL^(-1)` ?

Explanation

`68%` nitric acid by mass means that
Mass of nitric acid = 68 g
Mass of solution = 100 g
Molar mass of `HNO_(3) = 63 g mol ^(-1)`
`therefore 68g NHO_(3) = (68)/(63) ` mole `= 1. 079` mole
Density of solution `= 1,. 504 g mL ^(-1)`
`therefore ` Volume of solution `= (100)/(1.504) mL = 66.5 mL = 0.0665L`
Molarity of the solution `= ("Moles of the solute")/("Volume of solution") ` in L `= (1.0-79)/(0.0665) M = 16.23 M`