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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) ? |
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Answer» Solution :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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