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6 June, 09:08

A new non-electrolyte molecular is discovered. When 241 mg of the molecular is dissolved in 250.0 mL of water, it has an osmotic pressure of 0.072 atm at 25 oC. What is the molar mass of the molecular

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  1. 6 June, 09:28
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    Molar mass = 32.62g/mol

    Explanation:

    Mass = 24mg

    Volume = 250.0ml

    Osmotic pressure = 0.072 atm

    Temperature = 25 oC = 298 K (Converting to Kelvin temperature)

    Mass concentration = Mass / Volume

    Mass concentration = 24 mg / 250 ml = 0.096 mg/ml = 0.096 g / L

    This means that in 1L, there are 0.096g of the non electrolyte.

    Molar mass = Mass / Moles

    Finding the Molarity using osmotic pressure and temperature

    p = MRT

    Where M = n / v

    M = p / RT

    M = 0.072 / (0.0821 L atm/mol K) (298K)

    M = 0.072 / 24.4658

    M = 0.002943M

    Find the moles of solute from molarity by multiplying by the liters of solution. Since our calculation is base on 1L,

    moles = Molarity * Volume

    moles = 0.002943M * 1

    moles = 0.002943 mol

    Molar mass = Mass / Moles

    Molar mass = 0.096g / 0.002943 mol

    Molar mass = 32.62g/mol
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