Question

Calculate the depression in freezing point of a 0.2 molal solution if kf for water is 1.86 K kg mol-1. (

Answer 1

Answer:

0.372

Explanation:

∆Tf = m*Kf

∆Tf = m*Kf = 0.2*1.86

∆Tf = m*Kf = 0.2*1.86 =0.372K

Answer 2

Answer:

The depression in the freezing point of a 0.2m solution is 0.372K.

Explanation:

The formula to find depression in the freezing point is:

Δ$T_{f} = K_{f} * molality$

Where,

$K_{f}$ is called molal depression constant

The values given to us are:

$K_{f} = 1.86Kkgmol^{-1}$

$Molality = 0.2 m$

Now we substitute these values in the formula.

$T_{f} = 1.86 * 0.2 = 0.372 K$

The depression in the freezing point will be 0.372K of the solution of 0.2m.