Concentrated nitric acid used in laboratory work is 68% nitric acid by mass inaqueous solution. What should be the molarity of such a sample of the acid ifthe density of the solution is 1.504 g mL–1?

To find the molarity of the nitric acid solution, we need to follow these steps:

1. First, we need to find the mass of nitric acid in 1000 mL of the solution. Since the density of the solution is 1.504 g/mL, the mass of 1000 mL solution is 1.504 g/mL * 1000 mL = 1504 g.

2. Since the solution is 68% nitric acid by mass, the mass of nitric acid in this 1000 mL solution is 68/100 * 1504 g = 1022.72 g.

3. Next, we need to convert this mass into moles. The molar mass of nitric acid (HNO3) is approximately 63.01 g/mol. So, the number of moles of nitric acid is 1022.72 g / 63.01 g/mol = 16.23 mol.

4. Finally, we find the molarity of the solution by dividing the number of moles of nitric acid by the volume of the solution in liters. Since 1000 mL is equal to 1 L, the molarity of the solution is 16.23 mol / 1 L = 16.23 M.

So, the molarity of the nitric acid solution is 16.23 M.