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Q. When $800\, mL$ of $0.5\, M$ nitric acid is heated in a beaker, its volume is reduced to half and $11.5 \, g$ of nitric acid is evaporated. The molarity of the remaining nitric acid solution is $x \times 10^{-2} M$. (Nearest Integer)
(Molar mass of nitric acid is $63\, g \, mol ^{-1}$ )

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Solution:

$ n _{ HNO _3}=0.5 \times 0.8$
$ =0.4 $ mole
$\left( n _{ HNO _3}\right)_{\text {remains }}=0.4-\frac{11.5}{63}$
$ =0.4-0.1825 $
$ =0.2175 $
Molarity $=\frac{0.2175}{400} \times 1000$
$ =\frac{0.2175}{0.4} $
$ =0.5437 mole / lit . $
$\simeq 0.54 mole / lit . $
$ =54 \times 10^{-2} mol / lit .$