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

Let the mass of solution to be $100 g$

Mass of $H N O_{3}$ = $69 g$

Moles of $H N O_{3}$ , $n = \frac{69}{M_{H N O_{3}}} = \frac{69}{63}$ = $1.095$

Volume of solution, $V = \frac{M a s s}{D e n s i t y} = \frac{100}{1.41} = 70.9 m l$

Concentration of solution $= \frac{n}{V} \times 1000$
$= 15.44 m o l^{- 1}$

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Q. Calculate the concentration of nitric acid in moles per litre in a sample which has a density.1.41 g/ml and the mass Y. of nitric acids is 69Y.

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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%.

Let the mass of solution to be 100gMass of HNO3 = 69g Moles of HNO3, n = 69MHNO3=6963 = 1.095Volume of solution, V=MassDensity=1001.41=70.9mlConcentration of solution =nV×1000=15.44mol−1

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 $69 %$ .