Molal depression constant for a solvent is 4.0 kg mol-1. The depression in the freezing point of the solvent for 0.03 mol kg-1 solution of K2SO4 is: (Assume complete dissociation of the electrolyte)

Question

Molal depression constant for a solvent is 4.0 kg mol-1. The depression in the freezing point of the solvent for 0.03 mol kg-1 solution of K2SO4 is: (Assume complete dissociation of the electrolyte) (A) 0.12 K (B) 0.36 K (C) 0.18 K (D) 0.24 K

Tardigrade Admin · Accepted Answer

Kf = 4 K-kg/mol m = 0.03 mol/kg i = 3 Δ Tf = iKf × m Δ Tf = 3 × 4 × 0.03 = 0.3 6K

Q. Molal depression constant for a solvent is $4.0 k g m o l^{- 1}$ . The depression in the freezing point of the solvent for $0.03 m o l k g^{- 1}$ solution of $K_{2} S O_{4}$ is : (Assume complete dissociation of the electrolyte)

0.12 K

0.36 K

0.18 K

0.24 K

$K_{f}$ = $4 K - k g / m o l$
$m = 0.03 m o l / k g$
$i = 3$
$Δ T_{f} = i K_{f} \times m$
$Δ T_{f} = 3 \times 4 \times 0.03 = 0.36 K$

Q. Molal depression constant for a solvent is 4.0kgmol−1. The depression in the freezing point of the solvent for 0.03molkg−1 solution of K2​SO4​ is : (Assume complete dissociation of the electrolyte)