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6 Nov 2019

Using data from the table, calculate the freezing and boilingpoints of each of the following solutions.


Part A. 18.0g ofdecane, C10H22, in 52.5gCHCl3


Part B. 0.42mol ethyleneglycol and 0.12molKBrin 130gH2O


CHCl3

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Keith Leannon
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8 Aug 2019

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Related questions

Calculate the molality of each of the following solutions:

a.14.3 g of sucrose (C12H22O11) in 676 g of water

b.7.20 moles of ethylene glycol (C2H6O2) in 3546 g of water

Please show math and not just copy and paste from other websites thank you!

Using data from the table below, calculate the freezing and boiling points of 2.04 g KBr and 4.82 g glucose (C6H12O6) in 188 g H2O. Given: Kb of H2O: 0.51 C/m; Kf of H2O: 1.86 C/m.I'm not really looking for the answer (though I won't complain if you provide it), I'm just confused as to what I need to do if I have a solution with two solutes.I know I need to use the equation Delta(Tb)=Kb*m*i and Delta(Tf)=Kf*m*i.I know how to figure it out if it's only 1 solute but I'm confused as to what to do if I have two solutes.(By the way, I put this under my course ENGR 202; it's actually for ENGR 106 but it wasn't wanting to load that course. Anyways, that's trivial.

The boiling point and freezing points of a solution differs from those of the pure liquid. This can be explained in terms of vapor pressure. Since the vapor pressure of the solvent above the solution is lower, a higher temperature is needed to reach a point where the vapor pressure of the liquid meets the required 1 atm, and the boiling point is elevated. The lower vapor pressure changes the entire phase diagram for the solvent, and the resulting change pushes the triple point of the solution to a lower temperature value. The solid-liquid phase equilibria curve is related to the location of the triple point, and the freezing point is also lower.

The change in the boiling point for a solution containing a molecular solute, ΔTb, can be calculated using the equation

ΔTb=Kb⋠m

in which m is the molality of the solution and Kb is the molal boiling-point-elevation constant for the solvent. The freezing-point depression, ΔTf, can be calculated in a similar manner using

ΔTf=Kf⋠m

in which m is the molality of the solution and Kf is the molal freezing-point-depression constant for the solvent.

Ethylene glycol, the primary ingredient in antifreeze, has the chemical formula C2H6O2. The radiator fluid used in most cars is a half-and-half mixture of water and antifreeze.

Part A

What is the freezing point of radiator fluid that is 50% antifreeze by mass?
Kf for water is 1.86 ∘C/m.

Express your answer to three significant figures and include the appropriate units.

Part B

What is the boiling point of radiator fluid that is 50% antifreeze by mass?
Kb for water is 0.512 ∘C/m.

Express your answer to one decimal place and include the appropriate units.

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