Concentrated nitric acid used in laboratory w | vedclass

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(A) $68 \%$ nitric acid by mass means that $68 \, g$ of $HNO_3$ is present in $100 \, g$ of the solution.Molar mass of $HNO_3 = 1 + 14 + (3 	imes 16)

Vedclass · Accepted Answer

$16.23$

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(A) $68 \%$ nitric acid by mass means that $68 \, g$ of $HNO_3$ is present in $100 \, g$ of the solution.Molar mass of $HNO_3 = 1 + 14 + (3 	imes 16) = 63 \, g \, mol^{-1}$.Moles of $HNO_3 = \frac{68 \, g}{63 \, g \, mol^{-1}} = 1.079 \, mol$.Volume of solution $= \frac{	ext{mass}}{	ext{density}} = \frac{100 \, g}{1.504 \, g \, mL^{-1}} = 66.49 \, mL$.Molarity $(M) = \frac{	ext{moles of solute}}{	ext{Volume of solution in } L} = \frac{1.079 \, mol}{66.49 	imes 10^{-3} \, L} = 16.23 \, M$.

Concentrated nitric acid used in laboratory work is $68 \%$ nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is $1.504 \, g \, mL^{-1}$ (in $, M$)?

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