K f is the freezing point depression constant. It depends only on the SOLVENT. 1

Question

Kf is the freezing point depression constant. It depends only on the SOLVENT.

1) Match the following aqueous solutions with the appropriate letter from the column on the right.

Highest freezing point

2) Match the following aqueous solutions with the appropriate letter from the column on the right.

3) Match the following aqueous solutions with the appropriate letter from the column on the right.

Tf is the decrease in the freezing point = Tf(solution) - Tf(pure solvent) m is the molality of the solution = (# moles solute / kg solvent) i is the "van't Hoff" factor = (# moles of solute particles / mole of solute) For nonelectrolytes: i = 1 For strong electrolytes: i = number of (cations + anions) For weak electrolytes: 1 < i < number of (cations + anions)

Explanation / Answer

Solution :-

The colligative properties such as freezing point depression and boiling point elevation are dependent on the total particle concentrations of the solution.

There considering if the substance is electrolyte or not we need to calculate the total particle concentration of each solution and then using the concentrations we can determine the order.

Table 1 )

0.22m AgCH3COO * 2 = 0.44m        = Third lowest freezing point

0.14 m MgCl2 * 3 = 0.42 m              = highest freezing point

0.17 m (NH4)2SO4 * 3 = 0.51 m       = Lowest freezing point

0.47m sucrose * 1 = 0.47 m             = Second lowest freezing point

Table 2 )

0.16 m CuCl2*3 =0.48 m         = Second lowest freezing point

0.10m Cr(NO3)3 * 4 = 0.40 m = highest freezing point

0.15m MgCl2*3 = 0.45 m        = Third lowest freezing point

0.50 m urea *1 = 0.50 m         = lowest freezing point

Table 3 )

0.14 m ZnBr2*3 = 0.42m         = highest freezing point

0.16 m BaBr2 * 3 = 0.48 m    = Second lowest freezing point

0.15 mFeI2 *3 = 0.45m = third lowest freezing point

0.50m sucrose*1 =0.50m     = lowest freezing point

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