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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 1.504 gm L^(-1) is ? |
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Answer» Solution :Concentrated NITRIC acid used in laboratory work is 68% nitric acid by mass in an aqueous solution. This MEANS that 68 g of nitric acid is dissolved in 100 g of the solution. Molar mass of nitric acid `(HNO_(3))` `= 1xx1+1xx14+3xx16` `= 63 g mol^(-1)` Then, number of moles `HNO_(3)=(68)/(63)mol` = 1.079 mol Given, DENSITY of solution `= 1.504 g mL^(-1)` Therefore, VOLUME of 100 g solution `= (100)/(1.504)mL` `= 66.49 mL` `= 66.49xx10^(-3)L` Molarity of solution `= (1.079 mol)/(66.49xx10^(-3)L)-16.23 M` |
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