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The depression in freezing point for 0.0...

The depression in freezing point for 0.01 m aqueous solution of `K_x[Fe(CN)_6]` is 0.0744 K. The molal depression constant for solvent is 1.86 K kg `mol^(–1)`. If the solute undergoes complete dissociation, what is the correct molecular formula for the solute?

A

`K_2[Fe(CN)_6]`

B

`K_3[Fe(CN)_6]`

C

`K[Fe(CN)_6]`

D

`K_4[Fe(CN)_6]`

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaT_b = iK_f m`
`0.0744 = i xx 1.86 xx 0.01`
`rArr` i = 4
So, n = 4
Formula is `K_3 [Fe(CN)_6]`.
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