Choose the aqueous solution below with the highest freezing point. these are all solutions of nonvolatile solutes and you should assume ideal van't hoff factors where applicable. choose the aqueous solution below with the highest freezing point. these are all solutions of nonvolatile solutes and you should assume ideal van't hoff factors where applicable.

a. 0.200 m ba(no3)2
b. 0.200 m mg(clo4)2
c. 0.200 m hoch2ch2oh
d. 0.200 m na3po3

0.200 m of HOCH2CH2OH has the highest freezing point.

The freezing point of a solution is always lower than the freezing point of the pure solvent. This is called the freezing point depression. It is a colligative property

We can see that all the solutions have the same molality, if that is the case, then the freezing point of the solution would depend on the  number of particles present in solution.

The solution that has the lowest number of particles in solution will have the highest freezing point. Therefore, 0.200 m HOCH2CH2OH has the highest freezing point.

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c. 0.200 m HOCH2CH2OH

Explanation:

The collective properties of solvents expressed that the freezing point of water is lowered when solute particles are dissolved in it.

When more particles are dissolved, the more the freezing point is deepened and lowered.

Here, all the molarities are equal, the deciding factor in measuring the lowering will be which substance produces the fewest particles in solution; then we relate it to lowering of the freezing point.

Ba(NO3)2 ---> Ba2+ + 2NO3(1-)

1 mol releases 3 mol of ions.

Mg(ClO4)2 ---> Mg2+ + 2ClO4(1-)

1 mol releases 3 mol of ions.

HOCH2CH2OH is covalent and doesn't ionize.

1 mol in water is just 1 mol of molecules.

Na3PO3 ---> 3Na+ + PO3(1-)

1 mol releases 4 mol ions.

The substance that produces the fewest particles in solution is the 0.200 m HOCH2CH2OH