Solutions

K (or 374.918 K if considering the boiling point of water as 373.15 K)
Step 1: Boiling Point Elevation Formula The boiling point elevation is given by: where, (for water), molal, = van’t Hoff factor.

Step 2: Calculation of Van't Hoff Factor The dissociation of is: Total particles before dissociation = 1, Total particles after dissociation = 5. Degree of ionization is given as 60% (0.6).

Step 3: Calculate Boiling Point Elevation If the boiling point of water is taken as 373.15 K,

gas has a higher value because a higher means lower solubility of the gas in liquid.
Step 1: Understanding Henry’s Law Constant ( ) Henry’s law states that: where is the concentration of the gas in liquid, is Henry’s law constant, and is the partial pressure of the gas.

Step 2: Relationship Between and Solubility Since is more soluble in water than , it has a lower value. Thus, has a higher .

Blood cells shrink.
Step 1: Understanding Hypertonic Solutions A solution with more than 0.9% NaCl is hypertonic compared to the fluid inside blood cells.

Step 2: Effect on Blood Cells Due to osmosis, water moves out of the blood cells into the hypertonic solution to balance the concentration gradient. This leads to shrinking (crenation) of blood cells.

K (or 374.918 K if considering the boiling point of water as 373.15 K)
Step 1: Boiling Point Elevation Formula The boiling point elevation is given by: where, (for water), molal, = van’t Hoff factor.

Step 2: Calculation of Van't Hoff Factor The dissociation of is: Total particles before dissociation = 1, Total particles after dissociation = 5. Degree of ionization is given as 60% (0.6).

Step 3: Calculate Boiling Point Elevation If the boiling point of water is taken as 373.15 K,

Blood cells shrink.
Step 1: Understanding Hypertonic Solutions A solution with more than 0.9% NaCl is hypertonic compared to the fluid inside blood cells.

Step 2: Effect on Blood Cells Due to osmosis, water moves out of the blood cells into the hypertonic solution to balance the concentration gradient. This leads to shrinking (crenation) of blood cells.

gas has a higher value because a higher means lower solubility of the gas in liquid.
Step 1: Understanding Henry’s Law Constant ( ) Henry’s law states that: where is the concentration of the gas in liquid, is Henry’s law constant, and is the partial pressure of the gas.

Step 2: Relationship Between and Solubility Since is more soluble in water than , it has a lower value. Thus, has a higher .

Complete and Balanced Chemical Equations
(1) Thermal Decomposition of Potassium Permanganate: (2) Dichromate-Iodide Reaction:

To solve the problem, we need to understand what happens to the molar mass of a solute when association occurs in a solution.

1. Understanding Association in Solutions:
Association refers to the process in which solute molecules or ions combine to form larger aggregates or clusters, typically due to intermolecular forces such as hydrogen bonding. This happens mostly in polar solvents like water, where molecules like acids, bases, or other solutes tend to form dimers, trimers, etc.

2. Effect on Molar Mass:
When association occurs, the apparent molar mass of the solute will appear to be greater than the actual molar mass. This is because the association leads to fewer particles in solution (fewer particles are dissociated), and hence, the observed colligative properties (such as freezing point depression or boiling point elevation) will be less than expected for the number of particles, which makes the calculated molar mass higher.

3. Key Concept:
Abnormal molar mass refers to the measured molar mass that is higher than the expected value due to association. For example, when a dimer is formed, the apparent molar mass will be double the actual molar mass of the solute.

Final Answer:
In case of association, the abnormal molar mass of the solute will increase.

Here's the explanation:

1. Understanding Osmosis:
Osmosis is the natural movement of water molecules from a region of higher water concentration (lower solute concentration) to a region of lower water concentration (higher solute concentration) through a semi-permeable membrane. This process aims to equalize water concentrations on both sides of the membrane.

2. Reverse Osmosis:
Reverse osmosis is the opposite process where water is forced to move from an area of lower water concentration to higher water concentration, requiring the application of external pressure.

3. Analyzing the Mango Scenario:
When an unripe mango is placed in a concentrated salt solution:

• The salt solution has a lower water concentration (higher solute concentration) than the mango's interior
• Water naturally moves out of the mango (higher water concentration) into the salt solution (lower water concentration)
• This water loss causes the mango to shrivel

4. Process Identification:
Since this involves the natural movement of water from high to low concentration areas without external pressure, it is regular osmosis, not reverse osmosis.

Conclusion:
The correct explanation is that the mango loses water due to osmosis.

Final Answer:
The correct answer is (D) it loses water due to osmosis.

1. Definition of Azeotrope:
An azeotrope is a mixture of two or more liquids that boil at a constant temperature and have a fixed composition, such that the vapor produced has the same composition as the liquid mixture. Azeotropes behave like pure substances during boiling and cannot be separated into their individual components by simple distillation.

2. Azeotrope formed by Negative Deviation from Raoult's Law:
When a mixture exhibits a negative deviation from Raoult's law, the intermolecular forces between the molecules of the two liquids are stronger than those in the individual components. As a result, the boiling point of the mixture is lower than that predicted by Raoult's law, and the vapor has a different composition than the liquid. This leads to the formation of a minimum boiling azeotrope.

Example:
An example of an azeotrope formed by a negative deviation from Raoult's law is the mixture of hydrochloric acid (HCl) and water. This mixture forms a minimum boiling azeotrope with a boiling point of 108°C and a composition of approximately 20% HCl and 80% water.