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Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution. choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution. benzene, kb = 2.53°c/m water, kb = 0.512°c/m acetic acid, kb = 3.07°c/m carbon tetrachloride, kb = 5.03°c/m diethyl ether, kb = 2.02°c/m

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Dejanras
Answer is: carbon tetrachloride has the greatest boiling point elevation.
The boiling point elevation is directly proportional to the molality of the solution according to the equation: ΔTb = Kb · b.
ΔTb -  the boiling point elevation.
Kb - the ebullioscopic constant.
b - molality of the solution.
So the highest boiling poing elevation will be for solution with highest ebullioscopic constant because molality is the same.
ardni313

Carbon tetrachloride, CCl₄ Kb = 5.03 ° c / m, would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution  

Further explanation  

Colligative properties are the properties of a solution that do not depend on the type of solute but only on the concentration of the solute.  

Colligative properties of electrolyte solutions differ from non-electrolyte solutions because electrolyte solutions contain a greater number of particles because electrolytes break down into ions. So the colligative properties of electrolytes is greater than non-electrolytes.  

The term used in the colligative properties

  • 1. molal  

that is, the number of moles of solute in 1 kg of solvent  

[tex]\large{\boxed{\bold{m=mole. \frac{1000}{ mass\:of\:solvent (in\:grams)}}}[/tex]

  • 2. mole fraction  

the ratio of the number of moles of solute to the mole of solution  

[tex]\large{\boxed{\bold{Xa=\frac{na}{na+nb} }}[/tex]

  • 3. Vapour pressure  

Vapor pressure depends on the mole fraction of the components in the solution  

Pa = Xa. P °  

Pa = vapor pressure component A  

P ° = pure vapor pressure  

Xa = mole fraction A  

ΔP = P ° - P where  

ΔP = change in vapor pressure  

  • 4. Boiling point and freezing point  

Solutions from volatile substances have a higher boiling point and lower freezing point than the solvent  

ΔTb = Tb solution - Tb solvent  

ΔTb = boiling point elevation  

[tex]\large{\boxed{\boxed{\bold{\Delta Tb\:=\:Kb.m}}}[/tex]

ΔTf = Kf.m  

Kb = molal boiling point constant

Kf = molal freezing point constant  

m = molal solution  

From the Boiling Point Elevation Equation shows that the value of the change in the boiling point of the solution depends on:  

• 1. The concentration of the solution is molal  

• 2. molal boiling point constant value  

Of the compounds in question, carbon tetrachloride (CCl₄), has the largest Kb of 5.03 ° c / m, so that the boiling point changes are greatest because the amount of molal concentration of the solution to be made is equal to = 0.1 m  

Learn more  

Raoult's law  

https://brainly.com/question/10165688  

The vapor pressure of benzene  

https://brainly.com/question/11102916  

The freezing point of a solution  

https://brainly.com/question/8564755  

https://brainly.com/question/4593922  

https://brainly.com/question/1196173  

Keywords: Freezing Point Depression, Boiling Point Elevation, Colligative Properties  

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