A) KCI
B) \[{{C}_{6}}{{H}_{12}}{{O}_{6}}\]
C) \[A{{l}_{2}}{{(S{{O}_{4}})}_{3}}\]
D) \[{{K}_{2}}S{{O}_{4}}\]
Correct Answer: C
Solution :
\[\Delta {{T}_{f}}\] (freezing point depression) is a colligative property and depends upon the van't Hoff factor (i) i.e., number of ions given by the electrolyte in aqueous solution. \[\Delta {{T}_{f}}=i\times {{K}_{f}}\times m\] where, \[{{K}_{f}}\] = molal freezing point depression constant. m = molality of the solution \[\therefore \]\[{{K}_{f}}\] and m are constant, \[\Delta {{T}_{f}}\propto i\] [a] \[KCl(aq){{K}^{+}}(aq)+C{{l}^{-}}(aq),\] (Total ions = 2 thus, i = 2) [b] \[{{C}_{6}}{{H}_{12}}{{O}_{6}}no\,ions[i=0]\] [c] \[A{{l}_{2}}{{(S{{O}_{4}})}_{3}}(aq)2A{{l}^{3+}}+3SO_{4}^{2-}\] [Total ions =5, thus, i = 5] [d] \[{{K}_{2}}S{{O}_{4}}(aq)2{{K}^{+}}+SO_{4}^{2-}\] [Total ions = 3, t Thus, i = 3] Hence, \[A{{l}_{2}}{{(S{{O}_{4}})}_{3}}\] will exhibit largest freezing point depression due to the highest value of i.
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