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March 30, 2017

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hellppp please i have a test on this on mondayy im so screwed
A solid mixture contains MgCl2 and NaCl. When 0.5000 g of this solid is dissolved in enough water to form 1.000 L of solution, the osmotic pressure at 25°C is observed to be 0.4010 atm. What is the mass percent of MgCl2 in the solid? (Assume ideal behavior for the solution.)

  • Chemistry - ,

    Osmotic pressure is given by:
    π = MRT
    π = osmotic pressure in atm
    Mi = moles of particles/liter <- unknown
    R = 0.0821 L.atm/K.mol
    T = 298 K

    • Substitute and solve for Mi to moles of ions per liter.
    • Divide M by 3 to get the overall molarity, M, in terms of MgCl2 formula units.
    • Multiply M by the molar mass of MgCl2 to get grams / liter which is equal to grams/(1000mLs)
    • Divide by 10 to get grams / 100 mLs = ___%

    (NOTE: We assume the density of the solution is close to 1.00 g/mL, so that grams/100mLs is about the same as the mass % )

  • Chemistry - ,

    Osmotic pressure is given by:
    π = MRT
    π = osmotic pressure in atm
    Mi = moles of particles/liter <- unknown
    R = 0.0821 L.atm/K.mol
    T = 298 K

    • Substitute and solve for Mi to moles of ions per liter.
    • Divide Mi by 3 to get the overall molarity, M, in terms of MgCl2 formula units/L.
    • Multiply M by the molar mass of MgCl2 to get grams / liter which is equal to grams/(1000mLs)
    • Divide by 10 to get grams / 100 mLs = ___%

    (NOTE: We assume the density of the solution is close to 1.00 g/mL, so that grams/100mLs is about the same as the mass % )

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