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The 0.0001 molal solution of a complex A...

The `0.0001` molal solution of a complex `AB_(10)` has the freezing point of `-0.0015^(@)C` in water. Assuming `100%` dissociation of the complex, find the proper representation of the complex `[K_(f)(H_(2)O=1.86Km^(-1))]`
(a) `[AB_(8)]`
(b) `[AB_(3)]B_(7)`
(c )` [AB_(7)]B_(3)`
(d) `[AB_(5)]B_(5)` .

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Text Solution

Verified by Experts

The correct Answer is:
b
At `100%` dissociation van t Hoff vactor if `I = n` (no of ions from the complex
Now `deltaT_(f)|=iK_(f)m`
`implies i = n= (|DeltaT_(f)|)/(K_(f)m) = (0.0015)/(1.86 xx 0.0001) = 8`
implies Thus there should be 8 ions in solution
implies The compound should be `[AB_(3)]B_(7))` .
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