When 4.96 g of a nonelectrolyte solute is dissolved in water to make 485 ml of solution at 27 °c, the solution exerts an osmotic pressure of 827 torr. what is the molar concentration of

concentration = 0.044 moles / L

Explanation:

The mass of non electrolyte solute dissolved in water =4.96 grams

The volume of water taken = 485mL = 0.485 L

the temperature = 27°C = 300 K

osmotic pressure = 827 torr =

The osmotic pressure is related to molar concentration as:

osmotic pressure = concentration X R X T

Where

R = gas constant = 0.0821 L atm/molK

Putting values

1.09 = concentration X 0.0821 X 300

concentration = 0.044 moles / L

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