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  4. Concentrated nitric acid used for laboratory works 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 solution is 1.504 g mL- 1 ?

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Q. Concentrated nitric acid used for laboratory works 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 solution is $ \, 1.504 \, g \, mL^{- 1}$ ?

NTA AbhyasNTA Abhyas 2020Some Basic Concepts of Chemistry

Solution:

68% mass of $H N O_{3}$ means 100 g solution contains 68 g $H N O_{3}$

$\therefore $ Volume of $solution \, = \, wt. \, of \, solution \, / \, density \, =\frac{100}{1.504} \, = \, 66.49 \, mL \, $

$Molarity \, \left(M\right)=\frac{m o l e \, o f \, H N O_{3}}{v o l u m e \, o f \, s o l u t i o n \, i n \, l i t r e} \, $

$=\frac{68 \, \times 1000}{63 \times 66.49}=16.23M$