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10/09/2020 8:29 pm
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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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10/09/2020 8:30 pm
The molar mass of nitric acid is 63 g/mol.
It is given that the nitric acid used in laboratory is 68% by mass in aqueous solution.
100 g of solution contains 68 g of nitric acid or 68/63 = 1.079 moles of nitric acid.
Density of solution is 1.504 g/mL.
100 g of solution corresponds to 100/1.504 = 66.5 mL or 0.0665 L
Molarity of the solution is the number of moles of nitric acid present in 1 L of solution.
It is 1.079/0.0665 = 16.22 M
Hence, the molarity should be 16.22 g/mL.