Question

How molar mass of a non-volatile solute is related to the depression in freezing point? Derive an equation.

Answer 1

The pure solvent freezing point is as per the molecules sticky form that can stay in the solid form and the time that takes to turn back to liquid will fall out equal.

However, the temperature of the Tf - non-volatile will be less than the Tf0 - pure solvent freezing point,

Hence, Tf0 – Tf = delta Tf

Answer 2

$\Delta T_f=i\times K_f\times \frac{\text{mass of non volatile solute}}{\text{molar mass of non volatile solute}\times \text{weight of solvent in kg}}$

Explanation:

Depression in freezing point is given by:

$\Delta T_f=i\times K_f\times m$

$\Delta T_f=T_f-T_f^0$ = Depression in freezing point

i= vant hoff factor

$K_f$ = freezing point constant

m= molality

Molality is defined as the number of moles of solute dissolved per kg of the solvent.

$\Delta T_f=i\times K_f\times \frac{\text{mass of non volatile solute}}{\text{molar mass of non volatile solute}\times \text{weight of solvent in kg}}$

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