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Concentrated nitric acid used in the lab...

Concentrated nitric acid used in the laboratory is `68%` nitric acid by mass 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"^(-1)`?

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To find the molarity of a concentrated nitric acid solution that is 68% by mass with a density of 1.504 g/mL, we can follow these steps: ### Step 1: Calculate the mass of the solution Assume we have 100 g of the solution (this makes calculations easier since we can directly use the percentage). ### Step 2: Calculate the mass of HNO3 in the solution Since the solution is 68% HNO3 by mass: \[ ...
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Concentrated nitric acid used in the 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 solution is 1.504 g mL^(-1) ?

Concentrated nitric acid used in the laboratory work is 68% nitric acid by mass in aquequs solution. What should be molarity of such sample of the acid if the density of solution is 1.504 g mL ""^(-1) ?

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  • Concentrated nitric acid used for laboratory works 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 solution is 1.504 gmL^(-1) ?

    A
    26.23 M
    B
    16.23 M
    C
    6.23 M
    D
    46.23 M

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