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Concentrated nitric acid used in the laboratory work is 68% nitric acid by mass in aqueoussolution. What should be the molarity of such a sample of the acid if the density of solution is 1.504 g mL^(-1)? |
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Answer» SOLUTION :In 100 g of nitric acid solution, MASS of nitric acid = 68 g Molar mass of HNO3 = 63 g `"mol"^(-1)` `therefore 68 g HNO_3 = 68/63 ` mole = 1.079 mole DENSITY of solution = `1.504 g mL^(-1)` Molarity of the solution = Mass of Solution/Density of solution `= (1.079 )/(0.0665)M = 16.23 M` |
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