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28 August, 09:15

When 4.31 g of a nonelectrolyte solute is dissolved in water to make 635 mL of solution at 28 °C, the solution exerts an osmotic pressure of 945 torr. What is the molar concentration of the solution?

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  1. 28 August, 09:21
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    Molar concentration is 0.050 M

    Explanation:

    Osmotic pressure -

    Osmotic pressure is pressure applied to stop the flow of solvent across a semipermeable membrane, from its high concentration to its low concentration, it is a type of colligative property, i. e., it depends on the number of moles of solute.

    Osmotic pressure can be calculated from the formula -

    π = CRT

    π = Osmotic pressure (in atm)

    C = molarity of the solution

    R = universal gas constant (0.082 L. atm / K. mol)

    T = temperature (Kelvin)

    From the question,

    π = 945 torr

    since,

    760 torr = 1 atm

    1 torr = 1 / 760 atm

    945 torr = 1 / 760 * 945 atm

    945 torr = 1.24 atm

    Temperature = T = 28°C

    (adding 273 To °C to convert it to K)

    T = 28 + 273 = 301 K

    Using the equation of osmotic pressure,

    π = CRT

    C = π / RT

    putting the

    C = 1.24 atm / 0.082 L. atm / K. mol * 301 K

    C = 1.24 / 24.68

    C = 0.050 M

    Hence,

    The Molar concentration is 0.050 M.
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