Calculate the aqueous solution with the highest freezing point. These are all so

Question

Calculate the aqueous solution with the highest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal Van't Hoff factors where applicable
a) .200 m Ca(ClO4)2
b).200 m K3PO3
c) .200 m HOCH2CH2OH
d) .200 m Ba(NO3)2
e) All of these have the same freezing point

Explanation / Answer

The freezing point of water is lowered when solute particles are dissolved in it. The more particles are dissolved, the more the freezing point is lowered. Since all the molarities are equal, the deciding factor will be which substance produces the fewest particles in solution; that is, produces the least lowering of the freezing point. Ca(Cl04)2 ---> Ca2+ + 2ClO4(1-) 1 mol releases 3 mol of ions. K3PO3 ---> 3K+ + PO3(3-) 1 mol releases 4 mol of ions. HOCH2CH2OH is covalent and doesn't ionize. 1 mol in water is just 1 mol of molecules. Ba(NO3)2 ---> Ba2+ + 2NO3(1-) 1 mol releases 3 mol ions. The substance that produces the fewest particles in solution is the 0.200 m HOCH2CH2OH.

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