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Concentrated nitric acid used in the laboratory work is 68% nitric 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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Molarity(M) = \(\frac{\%\,mass\,\times \,density\,\times\,10}{Molar\, mass \,of \,solute \,(HNO_3)}\)

\(\frac{68\,\times 1.504\,g\,mL^{-1}\,\times\,10}{63\,g\,mol^{-1}}\)

= 16.23 M

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