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) ?

Concentrated nitric acid used in laboratory work is 68% nitric acid by

1.	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) ?
Answer» Solution :`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`