Question

Three different compounds ($A,B$ and $C$) are known to have the empirical formula, $CrC{l}_3\cdot 6H_{2}O\left(X\right)$. When it is exposed to a dehydrating agent, $A$ loses 2 moles of water per mole of the compound $\left(X\right)$. $B$ loses 1 mole of water and compounds $C$ loses no water. Then which is most conducting in aqueous solution?

• A. $A$
• B. $B$
• C. $C$
• D. All are equal

Answer 1

Answer: (C)

$C$

$\stackrel{A}{\left[Cr\right(H_{2}O{)}_{4}C{l}_2]}Cl\cdot 2H_{2}O$

$\stackrel{B}{\left[Cr\right(H_{2}O{)}_{5}Cl]}C{l}_2\cdot H_{2}O$

$\stackrel{C}{\left[Cr\right(H_{2}O{)}_6]C{l}_3}$

The complex which will give maximum ions on dissociation is most conducting in aqueous solution.

So $C$ is the most conducting aqueous solution as it gives 4 ions in solution.