Choose the aqueous solution that has the highest boiling point. these are all solutions of nonvolatile solutes and you should assume ideal van't hoff factors where applicable. choose the aqueous solution that has the highest boiling point. these are all solutions of nonvolatile solutes and you should assume ideal van't hoff factors where applicable. a. 0.100 m li₂so₄
b. 0.100 m kno₂
c. 0.200 m c₃h₈o₃
d. 0.060 m li₃po₄e. they all have the same boiling point.

0.100 m

Explanation:

=  Elevation in boiling point

i = Van'T Hoff factor  

= boiling point constant

m = molality

1. For 0.100 m

i= 3 as it is a electrolyte and dissociate to give 3 ions.

Thus concentration of ions =

2. For 0.100 m

i= 2 as it is a electrolyte and dissociate to give 2 ions.

Thus concentration of ions =

3. For 0.200 m

i= 1 as it is a non electrolyte and do not dissociate to give ions.

4. For 0.060 m

i= 4 as it is a electrolyte and dissociate to give 4 ions.

Thus concentration of ions =

Thus as concentration of ions is highest for and the boiling point will be highest.

0.060 m Li₃PO₄ has the highest boiling point

Solution properties are the properties of a solution that don't depend on the type of solute but only on the concentration of the solute.

Solution 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 Solution properties of electrolytes is greater than non-electrolytes.

The term is used in the Solution properties

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

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

ΔTb = Tb solution - Tb solvent

ΔTb = boiling point elevation

Kb = molal boiling point increase

Kf = molal freezing point constant

m = molal solution

For electrolyte solutions there is a van't Hoff factor = i

n = number of ions from the electrolyte

α = degree of ionization, strong electrolyte α = 1, for non electrolytes i = 1

so the boiling point formula becomes:

[tex] \ rm \ Delta T_f = K_b \ times m \ times i [/ tex]

All solutions in the problem have the same solvent -> assuming water (The same [tex] \ rm K_b [/ tex]) so that what affects the value of [tex] \ rm \ Delta T_b [/ tex] is the value of i and m

Assuming the degree of electrolyte ionization α = 1, the magnitude i is determined by the number of ions produced by the electrolyte (n)

 a. 0.100 m Li₂SO₄

 Li₂SO₄ ---> 2Li ++ SO₄²⁻ → 3 ions

m x i = 0.1 x 3 = 0.3

b. 0.100 m KNO₂

KNO₂ ---> K⁺ + NO₂⁻ → 2 ions

m x i = 0.1 x 2 = 0.2

c. 0.200 m C₃H₈O₃

Non-electrolyte solution, i = 1

ΔTb = Kb .m (based only on concentration m)

m x i = 0.2 x 1 = 0.2 or m only = 0.2

d. 0.060 m Li₃PO₄

Li₃PO₄ ---> 3Li⁺ + PO₄ ³⁻ → 4 ions

m x i = 0.06 x 4 = 0.24

Li₃PO₄ has the highest number of m x i, so it has the highest [tex] \ rm \ Delta T_b [/ tex] and the highest boiling point.

colligative properties

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Raoult's law

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The vapor pressure of benzene

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The freezing point of a solution

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