Types Of Solutions

Concept: Chemistry (Solutions) - Colligative Properties.

Step 1: Define Colligative Properties. Colligative properties are properties of solutions that depend solely on the number of solute particles present, regardless of their chemical identity.

Step 2: Identify the standard colligative properties.
• Relative Lowering of Vapour Pressure: The decrease in vapor pressure upon adding a non-volatile solute.
• Elevation of Boiling Point: The increase in boiling temperature.
• Depression of Freezing Point: The decrease in freezing temperature.
• Osmotic Pressure: The pressure needed to stop osmosis.

Step 3: Compare the options. While elevation of boiling point is a colligative property, the boiling point itself is a characteristic physical property of a substance and is not colligative. $ $

Step 1: Use formula: $ =80 =80 =0.08 $

The expression for the osmotic pressure of the solution is shown below.

Here, is the osmotic pressure,
is the molar concentration,
is mass of solute,
is the molar mass of solute,
is the volume of the solution in liter,
is the ideal gas constant and
is the absolute temperature.


The osmotic pressure of the solution is atm.

Molarity (M) is defined as: Given: Moles of NaCl = 0.5 mol
Volume of solution = 250 mL = 0.25 L Option (b) is correct.

Among the given gases, carbon dioxide is the most soluble in water. This is due to its ability to react with water to form carbonic acid: This reaction increases its solubility significantly compared to other gases like oxygen, nitrogen, and hydrogen, which are relatively non-reactive and only physically dissolve in water.

Concept: The Van’t Hoff factor ( ) represents the number of particles formed when one formula unit of a solute dissociates in solution.

Step 1: Write the dissociation reaction of .

Step 2: Count the number of ions produced. Total ions produced:

Step 3: Determine the Van’t Hoff factor.

Concept: The Van't Hoff factor ( ) represents the number of particles into which a substance dissociates in solution. It is used in colligative properties such as boiling point elevation, freezing point depression, and osmotic pressure.

Step 1: Understanding non-electrolytes. A non-electrolyte is a substance that does not dissociate into ions when dissolved in water. It remains as whole molecules in solution.

Step 2: Value of Van't Hoff factor. Since a non-electrolyte does not dissociate, the number of particles in solution remains the same as the number of molecules dissolved. Thus,

Step 3: Conclusion. Therefore, the Van't Hoff factor for a non-electrolyte is .

Concept: The osmotic pressure of a dilute solution is given by the van't Hoff equation: where
• = osmotic pressure
• = molar concentration
• = gas constant
• = temperature in Kelvin

Step 1: Convert the temperature to Kelvin.

Step 2: Substitute the values in the formula.

Step 3: Calculate the osmotic pressure. Thus,

Concept: The osmotic pressure of a dilute solution is given by the formula where

Step 1: Convert temperature to Kelvin.

Step 2: Substitute the values.

Step 3: Calculate osmotic pressure. Thus,

Concept: Osmotic pressure is given by the formula where
• = molar concentration
• = gas constant
• = temperature in Kelvin For non-electrolytes like glucose, the Van't Hoff factor .

Step 1: Convert temperature into Kelvin.

Step 2: Substitute values into the formula.

Step 3: Simplify the expression.

Step 1: Understanding the Question:
The question asks for the Van't Hoff factor ( ) for the electrolyte (assuming "KSO" is a typo for Potassium Sulfate, , as it is a common exam example) when dissolved in water. The Van't Hoff factor represents the degree of dissociation of a solute.

Step 2: Key Formula or Approach:
For strong electrolytes that dissociate completely in dilute solutions:
For an electrolyte that dissociates into and , the number of ions is .

Step 3: Detailed Explanation:
When Potassium Sulfate ( ) dissolves in water, it dissociates into its constituent ions as follows:
- Number of potassium ions ( ) = 2
- Number of sulfate ions ( ) = 1
Total number of ions produced = .
Assuming complete dissociation (ideal solution), the Van't Hoff factor is equal to the number of ions produced.
Therefore, .

Step 4: Final Answer:
The Van't Hoff factor for a solution of in water is 3.

Concept: The Van't Hoff factor ( ) represents the number of particles formed when one formula unit of a solute dissociates in solution. For strong electrolytes that dissociate completely in water, the Van't Hoff factor equals the total number of ions produced.

Step 1: Write the dissociation of potassium sulfate in water.

Step 2: Count the total number of ions formed. From one formula unit of :
• potassium ions
• sulfate ion Total ions formed:

Step 3: Determine the Van't Hoff factor. Thus, the Van't Hoff factor for in water is