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8 November, 09:44

An aqueous solution is 3.00% by mass dextrose (C6H12O6) in water. If the density of the solution is 1.0097 g/mL, calculate the molarity of dextrose in the solution.

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  1. 8 November, 09:56
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    [C₆H₁₂O₆] = 0.17M

    Explanation:

    3% by mass, means 3 g of solute in 100 g of solution.

    Density is mass / volume. This data always refers to solution.

    Solution density = Solution mass / Solution volume

    1.0097 g/mL = 100 g / Solution volume

    Solution volume = 100 g / 1.0097 g/mL → 99.03 mL

    Let's convert the mL to L, for molarity (mol/L)

    99.03 mL = 0.09903 L

    Now we have to find out the moles. Let's calculate them with the molar mass

    (mass / molar mass)

    3 g / 180 g/mol = 0.0166 mol

    Molarity is mol/L → 0.0166 mol/0.09903 L → 0.17 M
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