The depression in freezing point for 0.01 m aqueous solution of Kx[F e(C N)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?

Question

The depression in freezing point for 0.01 m aqueous solution of Kx[F e(C N)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) K2[F e(C N)6] (B) K3[F e(C N)6] (C) K[ Fe ( CN )6] (D) K4[F e(C N)6]

Tardigrade Admin · Accepted Answer

Δ Tb=i K f m 0.0744= i × 1.86 × 0.01 ⇒ i =4 So, n =4 Formula is K3[ Fe ( CN )6]

Q. The depression in freezing point for $0.01 m$ aqueous solution of $K_{x} [F e (CN)_{6}]$ is $0.0744 K$ . The molal depression constant for solvent is $1.86 K k g m o l^{- 1}$ . If the solute undergoes complete dissociation, what is the correct molecular formula for the solute?

$K_{2} [F e (CN)_{6}]$

$K_{3} [F e (CN)_{6}]$

$K [F e (CN)_{6}]$

$K_{4} [F e (CN)_{6}]$

$Δ T_{b} = i K_{f} m$
$0.0744 = i \times 1.86 \times 0.01$
$\Rightarrow i = 4$
So, $n = 4$
Formula is $K_{3} [F e (CN)_{6}]$

Q. The depression in freezing point for 0.01m aqueous solution of Kx​[Fe(CN)6​] is 0.0744K. The molal depression constant for solvent is 1.86Kkgmol−1. If the solute undergoes complete dissociation, what is the correct molecular formula for the solute?

K2​[Fe(CN)6​]

K3​[Fe(CN)6​]

K[Fe(CN)6​]

K4​[Fe(CN)6​]