A) KCl
B)
C)
D) \[{{K}_{2}}S{{O}_{4}}\]
Correct Answer: C
Solution :
| [c] \[\Delta {{T}_{f}}\] (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, \[\Delta {{T}_{f}}\propto i\] |
| \[KCl(aq){{K}^{+}}(aq)+C{{l}^{-}}(aq),\] |
| (Total ions = 2 thus, i = 2) |
| \[{{C}_{6}}{{H}_{12}}{{O}_{6}}no\,ions[i=0]\] |
| \[A{{l}_{2}}{{(S{{O}_{4}})}_{3}}(aq)2A{{l}^{3+}}+3SO_{4}^{2-}\] |
| [Total ions = 5, thus, i = 5] |
| \[{{K}_{2}}S{{O}_{4}}(aq)2{{K}^{+}}+SO_{4}^{2-}\] |
| [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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