Solubility Worksheet With Answers Page 7
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841) A 0.15 m aqueous solution of a weak acid has a freezing point of -0.31 °C. What is the percent
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ionization of this weak acid at this concentration? The molal freezing-point-depression constant of
water is 1.86 °C/m.
A) 35
B) 31
C) 11
D) 89
E) 17
42) Determine the fraction of ionization of HX if a solution prepared by dissolving 0.020 mol of HX in
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115 g of water freezes at -0.47 °C. The molal freezing-point-depression constant of water is
1.86 °C/m.
A) 1.45
B) 0.044
C) 0.30
D) 0.45
E) 0.348
43) Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO 4 . Assume i = 2.0 for
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MgSO 4 . The molal freezing-point-depression constant of water is 1.86 °C/m.
A) 0.000
B) -0.028
C) -0.056
D) -0.084
E) -0.17
44) A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in
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enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C.
What is the van't Hoff factor (i) for the unknown solute?
A) 0
B) 0.99
C) 1.98
D) 2.98
E) 0.630
45) George is making spaghetti for dinner. He places 4.01 kg of water in a pan and brings it to a boil.
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Before adding the pasta, he adds 58 g of table salt to the water and again brings it to a boil. The
temperature of the salty, boiling water is __________°C.
It is a nice day at sea level so that pressure is 1.00 atm. Assume negligible evaporation of water.
K b for water is 0.52°C/m.
A) 100.26
B) 100.00
C) 100.13
D) 99.74
E) 99.87
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