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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 1.504 g mL-1?

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68% nitric acid by mass means that

Mass of nitric acid = 68 g

Mass of solution = 100 g

Molar mass of HNO3 = 63 g mol-1 

68 g HNO3 = mole = 1.079 mole 

Density of solution = 1.504 g mL-1 

Volume of solution = \(\frac{100}{1.504}\) mL = 66.5 mL = 0.0665 L

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