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Concentration, mass, volume or temperature from osmotic pressure

This type of question, asked 7 times: 3 May 2023 S2, 19 Apr 2025 S2, 21 Apr 2025 S1, 13 Apr 2026 S2, 18 Apr 2026 S1, 20 Apr 2026 S1, 12 May 2026 S1. All 7 questions below, oldest first.

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  1. Question 1

    3 May 2023 S2

    61
    What mass of solute (molar mass 58 g mol−158\text{ g mol}^{-1}) is to be dissolved in 2.5 dm3 H2O2.5\text{ dm}^3\, \text{H}_2\text{O} to generate osmotic pressure of 0.245 atm at 300 K? [R=0.0821 dm3 atm K−1 mol−1][R=0.0821\text{ dm}^3\text{ atm K}^{-1}\text{ mol}^{-1}]

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  2. Question 2

    19 Apr 2025 S2

    84
    Calculate the concentration of an aqueous solution of non-electrolyte at 300 K if its osmotic pressure is 12 atm . [R=0.0821 atmdm3 K−1 mol−1]\left\lbrack R = 0.0821\text{ }atmdm^{3}{\text{ }K}^{- 1}{\text{ }mol}^{- 1} \right\rbrack

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  3. Question 3

    21 Apr 2025 S1

    84
    Calculate the temperature of 0.05 M sucrose solution in Kelvin if the osmotic pressure of the solution is 1.5 atm. [R=0.0821dm3 atm K−1 mol−1]\left\lbrack R = 0.0821dm^{3}\text{ }atm{\text{ }K}^{- 1}{\text{ }mol}^{- 1} \right\rbrack

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  4. Question 4

    13 Apr 2026 S2

    21
    An aqueous solution has an osmotic pressure of 4.924.92 atm at 300300 K. Calculate the molarity of the solution. (R=0.082(R = 0.082 L atm mol−1 K−1)\mathrm{mol^{-1}\,K^{-1}})

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  5. Question 5

    18 Apr 2026 S1

    22
    4040 gram nonelectrolyte solute having molar mass 180 g mol−1180\ \mathrm{g\,mol^{-1}} dissolved in water has osmotic pressure 22 atm at 300300 K. Calculate the volume of solution. (R=0.0821 atm mol−1K−1\mathrm{R} = 0.0821\ \mathrm{atm\,mol^{-1}K^{-1}})

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  6. Question 6

    20 Apr 2026 S1

    24
    Calculate the mass of nonvolatile solute dissolved in 0.3 dm30.3\ \mathrm{dm^3} water having osmotic pressure 0.10.1 atm at 300300K. [Molar mass of solute = 328 g mol−1328\ \mathrm{g\,mol^{-1}}, R = 0.082 dm3atm K−1mol−10.082\ \mathrm{dm^3atm\,K^{-1}mol^{-1}}]

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  7. Question 7

    12 May 2026 S1

    20
    Calculate the temperature of the solution in which a solution containing 1010 g solute in 0.4 dm30.4\ \mathrm{dm^3} has an osmotic pressure of 3.43.4 atm. [Molar mass of solute =180 g mol−1= 180\ \mathrm{g\,mol^{-1}}, R=0.082 atm dm3 K−1mol−1R = 0.082\ \mathrm{atm\,dm^3\,K^{-1}mol^{-1}}]

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