Inorganic Chemistry
Metallurgy Solutions
<Chapter 9
Freezing-Point Depression and Boiling-Point Elevation
6 of 11
A Review Constants Periodic Table
The changes in boiling point (AT) or freezing point (AT)
in degrees Celsius from a pure solvent can be determined
from the equations given here, respectively
AT m x Kb
moles of solute
kilograms of solvent
x Kb
Since pure water boils at 100.00 °C, and since the addition of solute increases boiling point, the boiling point of an aqueous
solution. To, will be
moles of solute
AT: m x K
kilograms of solvent
x Ki
where m is the molality of the solution, and Ky and Kf are
the boiling-point-elevation and freezing-point-depression
constants for the solvent, respectively. For water,
To = (100.00+ AT) °C
Since pure water freezes at 0.00 °C, and since the addition of solute decreases freezing point, the freezing point of an aqueous
solution, I will be
Ti = = (0.00 - AT) °C
Kp = 0.512
°C kg solvent
mol solute
Part A
KA
= 1.86
°C. kg solvent
mol solute
What is the boiling point of a solution made using 785 g of sucrose, C12H22011, in 0.275 kg of water, H2O?
Express your answer to five significant figures and include the appropriate units.
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