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 m L - 1 ?

Question

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 m L - 1 ?, 26.23 M, 16.23 M, 6.23 M, 46.23 M

MARKS App · Accepted Answer

68% mass of H N O 3 means 100 g solution contains 68 g H N O 3 ∴ Volume of s o l u t i o n = w t . o f s o l u t i o n / d e n s i t y = 100 1.504 = 66.49 m L M o l a r i t y M = 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 = 68 × 1000 63 × 66.49 = 16.23 M

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