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20 August, 22:02

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?

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  1. 20 August, 23:31
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    The first thing we need to do here is to recognize the unit of molarity and the units of the given percentage of nitric acid.

    Molarity is mol HNO3 / L of solution. This is our aim

    The given percentage is 0.68 g HNO3 / g solution

    multiplying this with density to convert g solution into mL solution and dividing with the molecular weight of HNO3 (63 g/mol) to convert g HNO3 to mol. Therefore we obtain

    0.016 mol / mL or 16.23 mol / L (M)
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