The density of a nitric acid solution is 1.5 | vedclass

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(D) Given: Density $(\delta)$ $= 1.5 \ g \ mL^{-1}$. Weight percentage of $HNO_3 = 68 \%$. Assume $1 \ L$ $(1000 \ mL)$ of solution. Mass of solution

Vedclass · Accepted Answer

$16.2$

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(D) Given: Density $(\delta)$ $= 1.5 \ g \ mL^{-1}$. Weight percentage of $HNO_3 = 68 \%$. Assume $1 \ L$ $(1000 \ mL)$ of solution. Mass of solution $= 	ext{density} 	imes 	ext{volume} = 1.5 \ g \ mL^{-1} 	imes 1000 \ mL = 1500 \ g$. Mass of $HNO_3 = 68 \% 	ext{ of } 1500 \ g = 0.68 	imes 1500 \ g = 1020 \ g$. Molar mass of $HNO_3 = 1 + 14 + (3 	imes 16) = 63 \ g \ mol^{-1}$. Moles of $HNO_3 = \frac{1020 \ g}{63 \ g \ mol^{-1}} \approx 16.19 \ mol$. Molarity $(M)$ $= \frac{	ext{moles of solute}}{	ext{volume of solution in } L} = \frac{16.19 \ mol}{1 \ L} = 16.19 \ M \approx 16.2 \ M$.

The density of a nitric acid solution is $1.5 \ g \ mL^{-1}$. Its weight percentage is $68 \%$. What is the approximate concentration (in $mol \ L^{-1}$) of nitric acid? $(N=14 \ u, O=16 \ u, H=1 \ u)$

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