Question:

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If $K_f$ for water is $ 1.86^{\circ} C/m$, the freezing point of the solution will be -

Updated On: Jul 19, 2024
  • $-0.24^{\circ} C$
  • $-0.18^{\circ} C$
  • $-0.54^{\circ} C$
  • $-0.36^{\circ} C$
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The Correct Option is A

Solution and Explanation

$i = 1 - \alpha + n\alpha$
$ i = 1 - 0.3 + 2 (0.3)$
$i = 1.3$
$ \Delta T_f = iK_f m$
$ = 1.3 \times 1.86 \times 0.1$
$\Delta T_f = + 0.24^{\circ} C$
Freezing point of solution = - 0.24�C
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Concepts Used:

Solutions

A solution is a homogeneous mixture of two or more components in which the particle size is smaller than 1 nm.

For example, salt and sugar is a good illustration of a solution. A solution can be categorized into several components.

Types of Solutions:

The solutions can be classified into three types:

  • Solid Solutions - In these solutions, the solvent is in a Solid-state.
  • Liquid Solutions- In these solutions, the solvent is in a Liquid state.
  • Gaseous Solutions - In these solutions, the solvent is in a Gaseous state.

On the basis of the amount of solute dissolved in a solvent, solutions are divided into the following types:

  1. Unsaturated Solution- A solution in which more solute can be dissolved without raising the temperature of the solution is known as an unsaturated solution.
  2. Saturated Solution- A solution in which no solute can be dissolved after reaching a certain amount of temperature is known as an unsaturated saturated solution.
  3. Supersaturated Solution- A solution that contains more solute than the maximum amount at a certain temperature is known as a supersaturated solution.