Question

# Which one of the following aqueous solutions will have the highest boiling point? Pleae provide workings....

Which one of the following aqueous solutions will have the highest boiling point? Pleae provide workings.

Select 1:

a. 0.200 mol kg-1 KCl(aq)

b. 0.200 mol kg-1 Na3PO4(aq)

c. 0.200 mol kg-1 NH4NO3(aq)

d. 0.200 mol kg-1 Na2SO4(aq)

We have the eqution,

where, = elevation in boiling point

i = Van't Hoff Factor

m = molarity

Kb = molal elevation constant

Thus,

i m

Assume 100% dissociation

a) im(KCL) = 0.200 * i

KCL K + + Cl -

Here, i = 2

Therefore, im(KCL) = 0.4

b)  im(Na3PO4) = 0.200 * i

Na3PO4 3 Na+ + PO4 -3

Here, i = 4

Therefore, im(KCL) = 0.8

c) im(Na3PO4) = 0.200 * i

NH4NO3 NH4+ + NO3 -

Here, i = 2

Therefore, im(NH4NO3) =0.4

d) im(Na2SO4) = 0.200 * i

Na2SO4 2 Na + + SO4 2-

Here, i = 3

Therefore, im(Na2SO4) =0.6

Hence, greater the value of im, greater will be the value of elevation in boiling point so boiling point.

Therefore, 0.200 M Na3PO4 will have the highest boiling point.

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