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# A compound crystallises as follows:Ions “A“ are at corners of a cubic unit cell and “B“ ions at face centres of a cubic unit cell and “C“ ions in 1/4$^{th}$ of the total tetrahedral void. Assuming if this is dissolved, only the ions in the tetrahedral voids are dissociated completely in water, which one of the following statements is true. (Assuming all are univalent ions) and also A and C are cations and B is an anions.

$\begin{array}{1 1}(A)\;\text{Boiling point of same concentration of }AlCl_3\text{ solution (100% dissociation) will be greater than that of this solution.}\\(B)\;\text{Boiling point of same concentration of }Ca_3(PO_4)_2\text{ solution (100% dissociation) will be greater than that of this solution.}\\(C)\;\text{Boiling point of same concentration of sucrose will be greater than this solution}\\(D)\;\text{Data insufficient to predict.}\end{array}$

Compound is $AB_3C_2$
$AB_3C_2\rightarrow [AB_3]^{2-}+2[C]^+$