19. Choose the aqueous solution below with the highest freezing point. These are

Question

19. Choose the aqueous solution below with the highest freezing point. These are all solutions of non- volatile solutes and you should assume ideal van't Hoff factors where applicable. A. 0.200 m Ca(ClO4)2, B. 0.200 m K3PO3, C. 0.200 m HOCH2CH2OH, D. 0.200 m Ba(NO3)2, The answer is C but how od you get that?

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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