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Assuming that CaCl2 (MW = 111.0 g/mol) dissociates 100% in
solution, what mass of CaCl2 is required to lower the freezing
point of 500.0 g water to -5.0 oC? [Kf = 1.86 oC Kg /mol]
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Question 2 (10 points) Calculate the freezing point of a solution that contains 5.78 g of glucose, a non- electrolyte, dissolved in 130 g of water. Note: Kf for water is 1.86°C/m
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Calculate the freezing point of a solution that contains 68.4
g of sucrose (table sugar, 342 g/mol) in 300. g of water. One mole
of sucrose is 342 g. Kf for H2O =
1.86°C/m.
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What is the normal boiling point of an aqueous solution that has a freezing point of 1.04 degree C. K_f for water 1.86 degree C/m.
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The experimentally measured freezing point of a 1.50 m aqueous
solution of CaCl2 is -6.70°C. The freezing point
depression constant for water is Kf =
1.86°C/m. Assume the freezing point of pure water is
0.00°C.
The experimentally measured freezing point of a 1.50 m aqueous
solution of CaCl2 is -6.70°C. The freezing point
depression constant for water is Kf =
1.86°C/m. Assume the freezing point of pure water is
0.00°C.
What is the predicted freezing point if there were no...
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What is the expected freezing point of a 0.0750 m solution of
LiBr in water?
(Kf for water is 1.86 °C/m.)
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What is the expected freezing point depression and
freezing point of a
0.20m solution of
the strong electrolyte calcium chloride,
CaCl2? Kf = 1.86°C/m
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calculate the freezing point of a solution of 25 mL of CH3OH (d=
0.792 g/mL) in 325 mL of water (d=1.00g/mL, Kf= 1.86 degrees
celcius/m).
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What is the freezing point of a solution of 12.8 g of
C10H8 dissolved in 500 g of benzene? The
normal freezing point of pure benzene is 5.48 oC and its
Kf is 5.12 oC/m.
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What is the freezing point and boiling point in Celsius of a
solution 400 g of ethylene glycol (MW=62 g/mol) dissolved in 500 g
of water?
The molal freezing point depression
constant for water is 1.86 C/m
The molal boiling point elevation
constant of water is 0.512 C/m
Please explain steps