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19 September, 11:10

A solution was prepared by dissolving 28.0g of KCL in 225g of water. Part A Calculate the mass percent ofKCL in the solution. Part B Calculate the mole fraction of KCL in the solution. Express the concentration numerically as a mole fraction in decimal form. Part C Calculate the molarity of in the solution if the total volume of the solution is 239. Express your answer with the appropriate units. Part D Calculate the molality of KCL in the solution. Express your answer with the appropriate units.

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  1. 19 September, 11:33
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    A. 11.1%

    B. 0.0291

    C. 1.57 M

    D. 1.67 m

    Explanation:

    A.

    Mass of KCl (solute) : 28.0 g

    Mass of water (solvent) : 225 g

    Mass of solution: 28.0 g + 225 g = 253 g

    The mass percent of KCl is:

    %KCl = (mass of KCl/mass of solution) * 100%

    %KCl = (28.0 g/253 g) * 100%

    %KCl = 11.1%

    B.

    The molar mass of KCl is 74.55 g/mol. The moles of KCl are:

    28.0 g * (1 mol/74.55 g) = 0.376 mol

    The molar mass of water is 18.02 g/mol. The moles of water are:

    225 g * (1 mol/18.02 g) = 12.5 mol

    The total number of moles is 0.376 mol + 12.5 mol = 12.9 mol.

    The mole fraction of KCl is:

    X (KCl) = moles of KCl / total moles

    X (KCl) = 0.376 mol / 12.9 mol

    X (KCl) = 0.0291

    C.

    The volume of the solution is 239 mL (0.239 L).

    The molarity of KCl is:

    M = moles of KCl / liters of solution

    M = 0.376 mol / 0.239 L

    M = 1.57 M

    D.

    The molality of KCl is:

    m = moles of KCl / kilograms of solvent

    m = 0.376 mol / 0.225 kg

    m = 1.67 m
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