First slide

General discussion of solutions

Question

Increasing amount of solid HgI₂ is added to 1 L of an aqueous solution containing 0.1 mol KI. Which of the following graphs do represent the variation of freezing point of the resulting solution with the amount of HgI₂ added?

Moderate

A
B
C
D

Solution

When HgI₂ is added to KI:
$H g I_{2} + 2 K I \to K_{2} H g I_{4} - 0.05 0.1 - - 0.05$
$\Rightarrow$ 0.05 moles of HgI₂are required for its complex reaction with KI.
Thus, as HgI₂ is being added, the number of solute molecules will decrease causing $∆ T_{f}$ to decrease $\Rightarrow$ (Causing T_f to increase). When whole of KI has been converted to $K_{2} H g I_{4}$ further addition of HgI₂does not change T_f since it is a sparingly soluble salt.

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