A water solution containing an unknown quantity of a nonelectrolyte solute is found to have a freezing point of

–0.23°C. What is the molal concentration of the solution?​

The molal concentration of the solution is approximately 0.124 molal

Explanation:

The given parameters are;

The reduced freezing point of the water = -0.23°C

For freezing point depression of a solution, we have;

= · b·i

Where;

= The freezing point depression

= Cyroscopic constant (The freezing-point depression constant) = 1.86° Cm⁻¹ for water

b = The molality of the solution

i = van't Hoff factor = 1

Therefore;

=

Where;

= The freezing point of pure water = 0°C

= The freezing point of the solution = -0.23°C

∴ = = 0°C - (-0.23°C) = 0.23 °C

From, = · b·i, we have;

0.23°C = 1.86°C/m × b × 1

∴ b  = (0.23°C/1.86°C/m) ≈ 0.124 molal

Therefore, the molal concentration of the solution, b ≈ 0.124 molal.

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