Question

Which one of the following aqueous solutions would have the lowest freezing point? Explain your reasoning....

Which one of the following aqueous solutions would have the lowest freezing point? Explain your reasoning.

0.030M HCl 0.025M Mg(NO3)2 0.020M BaCl2 0.025 M HC2H3O2

Homework Answers

Answer #1

0.030M HCl on dissociation gives two ions

0.025M Mg(NO3)2 on dissociation gives three ions

0.020M BaCl2 on dissociation gives three ions

0.025 M HC2H3O2 on dissociation gives only one ion (weak acid)

Freezing point lowering is a colligative property, so its magnitude depends on the number of particles (ions or molecules) in a given volume of the solution. The given aqueous solutions of the ionic salts dissociates in solution, we get 2, 3, 3 and 1 ions, respectively. 0.025M Mg(NO3)2  and 0.020M BaCl2 both have same number of ions on dissociation, so let us consider the molality. Molality of 0.025M Mg(NO3)2 is more (freezing point lowering α molality). Therefore 0.020 M BaCl2 will have the lowest freezing point.

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