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15 March, 12:12

A sucrose solution is prepared to a final concentration of 0.250 M. Convert this value into terms of g/L, molality, and mass %. (Use the following values: molecular weight MWsucrose = 342.296 g/mol; density rhosol′n = 1.02 g/mL; and mass of water, mwat = 934.4 g). Note that the mass of solute is included in the density of the solution.

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  1. 15 March, 12:16
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    A. 85.6 g

    = 0.0856 kg.

    B. 0.00027 mol/g

    = 0.27 mol/kg.

    C. 8.39 %

    Explanation:

    Given:

    Molar concentration = 0.25 M

    Molar weight of sucrose = 342.296 g/mol

    Density of solution = 1.02 g/mL

    Mass of water = 934.4 g.

    Density in g/l = 1.020 g/ml * 1000ml/1 l

    = 1020 g/l

    Mass of solution in 1 l of solution = 1020 g

    Mass of solution = mass of solvent + mass of solute

    Mass of sucrose = 1020 - 934.4

    = 85.6 g of sucrose in 1 l of solution.

    A.

    Density of sucrose = mass/volume

    = molar mass/molar concentration

    = 342.296 * 0.25

    = 85.6 g/l

    Number of moles = mass/molar mass

    = 85.6/342.296

    = 0.25 mol

    B.

    Molality = number of moles of solute/mass of solvent

    = 0.25/934.4

    = 0.00027 mol/g

    C.

    % mass of sucrose = mass of sucrose/total mass of solution * 100

    = 85.6/1020 * 100

    = 8.39 %
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