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anonymous

  • one year ago

1. Determine the osmotic pressure of a solution that contains 0.020 g of a hydrocarbon solute (molar mass = 340 g/mol) dissolved in benzene to make a 350-mL solution. The temperature is 20.0°C. A)3.1 torr B)1.0 torr C)2.9 torr D)0.21 torr E)1.4 torr 2. Which of the following solutions would have the highest osmotic pressure? A)0.2 M C6H12O6, glucose B)0.15 M MgBr2, magnesium bromide C)0.2 M CH3OH, methanol D)0.2 M C12H22O11, sucrose E)0.15 M KBr, potassium bromide

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  1. anonymous
    • one year ago
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    1. PV=nRT 2. Osmotic pressure=molarity multiplied by the number of ionic element. Ex: NaCl has 2 \[Na ^{+}, Cl ^{-}\] \[AlCl _{3} \] has 4 ions \[Al ^{3+},Cl ^{-},Cl ^{-}, Cl ^{-}\]

  2. anonymous
    • one year ago
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    The equation is not working for me, but do you understand?

  3. anonymous
    • one year ago
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    P is pressure in atm V is volume in liters n is the number of moles R is a constant which is 0.082 Temperature is in Kelvin.

  4. aaronq
    • one year ago
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    The formula for osmotic pressure is: \(\huge \sf\Pi=iMRT \) \(\sf \Pi\) is Osmotic pressure \(\sf i\) is the van't hoff constant \(\sf M\) is molarity \(\sf R\) is the gas constant \(\sf T\) is the absolute temperature

  5. anonymous
    • one year ago
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    Sorry, I meant to wrote osmotic pressure formula for this problem. We do not need to know the temperature or r because they are the same.

  6. aaronq
    • one year ago
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    For 2. you dont need it - clearly it's dependent on \(i\), but for 1. you do need to use the whole formula including the temperature.

  7. anonymous
    • one year ago
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    Yes, I referred to 2 only since that is the one asking for osmotic pressure.

  8. aaronq
    • one year ago
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    #1. is asking about osmotic pressure... "1. Determine the osmotic pressure of a solution.."

  9. aaronq
    • one year ago
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    >_>

  10. anonymous
    • one year ago
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    Oh yea but still. I said to use PV=nRT for problem 1 meaning temperature would be used. I never mentioned temperature or gas constant for the problem 2 because I forgot to put it there.

  11. anonymous
    • one year ago
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    thank you guys

  12. anonymous
    • one year ago
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    No problem.

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