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

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Solution

$100$ gm of ${H N O}_{3}$ solution contains $69$ gm of ${H N O}_{3}$ by mass.

$∴$ No. of moles in $69$ gm of ${H N O}_{3} = \frac{69}{63} = 1.095$ mole

Volume of $100$ gm ${H N O}_{3}$ solution $= \frac{100 g}{1.41 g m L^{- 1}}$

$= 70.92$ mL

$= 70.92 \times 10^{- 3} L$

$∴$ Concentration of ${H N O}_{3} = \frac{1.095 m o l e}{70.92 \times 10^{- 3} L} = 15.44 m o l e L^{- 1}$

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

100gm of HNO3 solution contains 69gm of HNO3 by mass.∴ No. of moles in 69gm of HNO3=6963=1.095 moleVolume of 100gm HNO3 solution =100g1.41gmL−1 =70.92mL =70.92×10−3L∴ Concentration of HNO3=1.095mole70.92×10−3L=15.44moleL−1

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