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17 June, 14:05

When 3.24 g of a nonelectrolyte solute is dissolved in water to make 955 mL of solution at 22 °C, the solution exerts an osmotic pressure of 973 torr. What is the molar concentration of the solution? concentration: M How many moles of solute are in the solution? moles of solute: mol What is the molar mass of the solute? molar mass: g / mol

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  1. 17 June, 16:02
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    The molar concentration is 0.0529 M

    We have 0.0505 moles solute

    The molar mass of the solute is 64.16 g/mol

    Explanation:

    Step 1: Data given

    Mass of the nonelectrolyte solute = 3.24 grams

    Volume of water = 955 mL

    Temperature = 22 °C = 295 K

    Osmotic pressure = 973 torr = 973 / 760 = 1.28026 atm

    Step 2: Calculate mass water

    Mass water = 955 mL * 1g/mL

    Mass water = 955 grams = 0.955 kg

    Step 3: Calculate the molar concentration

    π = i*M*R*T

    ⇒with π = the osmotic pressure = 1.28026 atm

    ⇒with i = the van't Hoff factor = 1

    ⇒with M = the molar concentration

    ⇒with R = the gas constant = 0.08206 L*atm/mol*K

    ⇒with T = the temperature = 295 K

    M = 1.28026 / (0.08206*295)

    M = 0.0529 M

    Step 4: Calculate moles solute

    Molar concentration = moles / volume

    Moles solute = Molar concentration * volume

    Moles solute = 0.0529 M * 0.955 L

    Moles solute = 0.0505 moles

    Step 5: Calculate molar mass

    Molar mass = mass / moles

    Molar mass = 3.24 grams / 0.0505 moles

    Molar mass = 64.16 g/mol

    The molar concentration is 0.0529 M

    We have 0.0505 moles solute

    The molar mass of the solute is 64.16 g/mol
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