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The freezing point of an aqueous saturated solution of $I_2$ is – 0.0024$^{\large\circ}$C. More than this can dissolve in a KI solution because of the following equilibrium $I_{2(aq)}+I_{aq}^-AI_{3(aq)}^-$ 0.1 M KI solution dissolves 12.5 g/L of I2. Calculate the equilibrium constant $K_c$ for the above equilibrium. Also calculate the freezing point of the resulting solution. Assume molarity to be equal to molality and also assume that conc. of $I_2$ in all saturated solutions is same. [$K_f$ for water =$1.86Kkgmol^{-1}]$

1 Answer

Hence (B) is the correct answer.
answered Jun 19, 2014 by sreemathi.v

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