Calculate the concentration of nitric acid in moles per litre in a sample which has a density, $1.41 g {m L}^{- 1}$ and the mass per cent of nitric acid in it being $69$ %.

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Solution

Mass % of the acid $= 69 %$

Density of the solution $= 1.41 g / m l$

Mass of 1 litre solution $= D e n s i t y \times V o l u m e = 1.41 \times 1000 = 1410 g$

Mass of the acid $= 0.69 \times 1410 = 972.9 g$

Moles of the acid $= \frac{w}{M} = \frac{972.9}{69} = 14.1 m o l$

Molarity of the acid $= 14.1 M$

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Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g mL−1 and the mass per cent of nitric acid in it being 69 %.

Mass % of the acid =69%Density of the solution =1.41 g/mlMass of 1 litre solution =Density×Volume=1.41×1000=1410gMass of the acid =0.69×1410=972.9gMoles of the acid =wM=972.969=14.1molMolarity of the acid =14.1M

Calculate the concentration of nitric acid in moles per litre in a sample which has a density, $1.41 g {m L}^{- 1}$ and the mass per cent of nitric acid in it being $69$ %.