Question:
What would be the freezing point of aqueous solution containing $17\, g$ of $C _{2} H _{5} OH$ in $1000\, g$ of water?
What would be the freezing point of aqueous solution containing $17\, g$ of $C _{2} H _{5} OH$ in $1000\, g$ of water?
Updated On: Jun 23, 2023
- $ 0.34^{\circ} C $
- $ 0.0^{\circ} C $
- $ -\,0.34^{\circ} C $
- $ -\,0.69^{\circ} C $
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The Correct Option is D
Solution and Explanation
Molality of $C _{2} H _{5} OH$ (non-electrolyte) solution
$=\frac{17 g / 46 \times 1000 g}{1000 g \text { water }} $
$=0.369 $
$\Delta T_{f} =k_{f} \times m $
$=1.86 \times 0.369=0.686$
Freezing point of the solution
$=0^{\circ} C -0.686^{\circ} C$
$=-0.69^{\circ} C$
$=\frac{17 g / 46 \times 1000 g}{1000 g \text { water }} $
$=0.369 $
$\Delta T_{f} =k_{f} \times m $
$=1.86 \times 0.369=0.686$
Freezing point of the solution
$=0^{\circ} C -0.686^{\circ} C$
$=-0.69^{\circ} C$
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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:
- Unsaturated Solution- A solution in which more solute can be dissolved without raising the temperature of the solution is known as an unsaturated solution.
- 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.
- Supersaturated Solution- A solution that contains more solute than the maximum amount at a certain temperature is known as a supersaturated solution.