Quiz: Freezing and Boiling Points

1. For a liquid solvent, adding solute particles will __________ the freezing temperature.
a. increase
b. decrease
c. not affect
2. Boiling point elevation means the solution will have a boiling point that is __________ than the pure solvent.
a. the same value
b. lower
c. higher
3. Changes in boiling and freezing points of ionic solutions are based on
a. only the molarity
b. only the molality
c. the number of total particles dissolved in the solvent
4. Given the K f for water is 1.86°C/m, a 2.2 m solution of glucose will have a freezing point of
a. 4.09°C
b. –4.09°C
c. 1.18°C
5. How many grams of NaCl should be added to 500 g of water to produce a solution which freezes at –5.00oC? (The K f for water is 1.86°C/m.)
a. 39.3 g NaCl
b. 1.34 g NaCl
c. 78.6 g NaCl
6. When 1.0 moles of CaCl2 dissolves in water, how many moles of particles are produced?
a. 1.0
b. 2.0
c. 3.0
7. What is the boiling point of a 1.0 molal solution of glucose and acetic acid if the normal boiling point of acetic acid is 118.1°C? (The K b of acetic acid is 3.07°C/molal.)
a. 115.03°C
b. 118.1°C
c. 121.17°C
8. 100.0 g of an unknown molecular substance is added to 1.000 kg of water. The solution has a freezing point of –0.543°C. What is the molar mass of the unknown substance? K f = 1.86.
a. 342.5 g/mol
b. 292.0 g/mol
c. 101.0 g/mol

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