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Concentrated nitric acid used in laborat...

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 1.504g `mL^(-1)`?

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Mol. mass of `HNO_(3) = 1+14+3 xx 16=63`
Weight of `HNO_(3)` per 100 g of solution = 68 g
Gram moles of `HNO_(3)=(68)/(63)`, volume of solution
`=("Mass")/("Density")=(100)/(1.504)=66.49mL`
Molarity of `HNO_(3)= ("Moles of " HNO_(3))/("Volume of solution (mL)") xx 1000`
`=(68)/(63) xx (1000)/(66.49)=16.23M`
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