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Concentrated nitric acid used in laborat...

Concentrated nitric acid used in laboratory work is 68% nitric add by aqueous solution. What should be the molarity of such a sample of the add lf the density of the solution is 1.504 g `mL^(-1)` ?

Text Solution

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Mass of nitric acid= 68 g
Mass of solution = 100 g
No. of moles of `HNO_(3) = ("mass ")/("Molar mass")`
`= (68)/(63) =1.079` mol
Density of solution = 1.504 g `mL^(-2)`
Density = `("Mass")/("volume") rArr "volume " = ("mass")/("density")`
` = (100 g)/(1.504 g "mL"^(-1))`
= 66.5 mL or 0.0665 L
Molarity = `("No.of moles of solute")/("volume of solution in litres ")`
= `(1.079 "mol")/(0.09665 L )`
= 16.23 mol `L^(-1)` .
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