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

Explanation

To find the molarity of a concentrated nitric acid solution that is 68% by mass with a density of 1.504 g/mL, we can follow these steps:

### Step 1: Calculate the mass of the solution
Assume we have 100 g of the solution (this makes calculations easier since we can directly use the percentage).

### Step 2: Calculate the mass of HNO3 in the solution
Since the solution is 68% HNO3 by mass:
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