Colligative Properties Worksheet - Answer Key

 

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  1. What is a colligative property?

    These properties, in particular, depend on the number, not identity, of solute particles in an ideal solution.

    2.  

     

  2. What are three examples of colligative properties?

      3.  

    1. Boiling Point Elevation

      2.  

    2. Freezing Point Depression

      3.  

    3. Osmotic Pressure

     

     

     

  3. How does adding a solute affect the boiling point of a solvent?

    It increases the boiling point

    4.  

     

     

  4. How does adding a solute affect the freezing point of a substance?

    It lowers the freezing point. 

    5.  

     

     

  5. What is osmotic pressure?

    The pressure that just stops osmosis. 

      6.  

    1. What does isotonic mean?

      This occurs when two substances have identical osmotic pressures.

     

     

     

  6. What is the Van’t Hoff Factor?

    The Van’t Hoff factor takes into account the number of particles present in solution if the compound dissolved breaks into ions.

    7.  

     

  7. What is the equation for determining the

      8.  

    1. Boiling Point Elevation

      ΔT =       ikbmsolute

      2.  

    2. Freezing Point Depression

      ΔT =       ikfmsolute

      3.  

    3. Osmotic Pressure

      π =       iMRT

     

     

  8. A solution is prepared by dissolving 27.0 g of urea [(NH2)2CO], in 150.0 g of water.  Calculate the boiling point of the solution.  Urea is a
    non-electrolyte.    kb=0.51 (°C kg)/mol.

    T = 101.53 oC

    9.  

     

  9. What mass of glycerin (C3H8O3), a nonelectrolyte, must be dissolved in 200.0 g of water to give a solution with a freezing point of -1.50°C?

    mass = 14.8 g

    10.  

     

  10. Consider the following

    0.010 m Na3PO4 in water 

    0.020 m CaBr2 in water

    0.020 m KCl in water

    0.020 m HF in water (HF is a weak acid)

      11.  

    1. Assuming complete dissociation of soluble salts, which solution(s) would have the same boiling point as 0.040 m C6H12O6 in water? (non-polar electrolyte).

      Na3PO4 and  KCl

      2.  

    2. Which solution would have the largest freezing point depression?

      CaBr2.

     

     

  11.  From the following :

    pure water

    solution of C6H12O6 (χ = 0.01) in water

    solution of NaCl (χ = 0.01) in water

    solution of CaCl­2 χ = 0.01) in water

    Choose the one with the following:

      12.  

    1. Highest freezing point

      Pure water. 

      2.  

    2. Lowest freezing point

      CaCl2

      3.  

    3. Highest Boiling Point

      CaCl2

      4.  

    4. Lowest Boiling Point

      Pure water. 

      5.  

    5. Highest Osmotic Pressure

      CaCl2­

     

     

  12. Determine the boiling point for a solution of 20.0 g of NaCl and 40.0 g CaF2 in 1.00 L of H2O.  The Kb for water is 0.51 oC kg/mol and the density equals 1.00 g/cm3.

    T = 101.1 oC

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