Solutions

Hence, mol of
mole of

At V.P.
of water,

As the colligative properties depend only upon the number of particles of solute, so if the non-volatile solute dissociates or associates in the solution, the value of colligative properties deviates ie, abnormal colligative properties are obtained.

According to Raoult's law, Relative lowering of vapour pressure mole fraction of solute or

or

Molality,

or
or or torr

When blood cells are placed in pure water, then the water molecules rapidly move into blood cells so that the blood .cells will expand and eventually burst.

When a solution containing non-volatile solute is diluted with water, its vapour pressure increases.

Addition of a non-volatile solute in a volatile ideal solvent decreases the vapour pressure of the solvent because if a non-volatile solute is added to the solvent temperature falls (since dissolution of a solute is an endothermic process) and thus, vapour pressure of the solution is lower than that of the pure solvent.

Desalination of sea water can be done by reverse osmosis i.e., by applying pressure greater than osmotic pressure on pure water so that water from saline water flow through a semipermeable membrane and this water can be used for drinking purposes.

Mass of solution
Mass of glucose
Mass of solvent
mass of solute glucose,
mass of solvent molar mass of solute


Freezing point of the solution

Depression of freezing point is given as
For water

The properties of a dilute solution which depends only upon the number of particles present in a solution and their concentration are called colligative properties. There are following four colligative properties
[a] relative lowering of vapour pressure
[b] elevation in boiling point of the solvent
[c] depression in freezing point
[d] osmotic pressure

Given, density of
Molarity . Volume of
Volume needed
First of all we find mass of methanol (i.e. given mass)
Molarity
Molarity
Molar mass of

Given mass or
Again denstiy


or

For , increases continuously with increase of pressure at

No. of moles of benzene
No. of moles of benzoic acid

A mixture of chloroform and aceton shows negative deviations from Raoult�s law due to formation of hydrogen bonding between the two molecules. Hence, a slight decrease in volume takes place

Step 1: Understand the behavior of electrolytic solutions.
For electrolytic solutions, the conductivity depends on the concentration of ions in the solution.
As the solution is diluted, the ions become more spread out, and their mobility increases, leading to an increase in conductance.
Step 2: Identify the correct statement.
When an electrolyte is diluted, its conductance increases due to the increase in ion mobility, even though its concentration decreases.

Step 1: Understand the relationship between ionic product and solubility product.
The ionic product is the product of the concentrations of ions in a solution.
The solubility product is the equilibrium constant for the dissolution of a salt in a solvent.
Step 2: Conditions for precipitation.
Precipitation occurs when the ionic product exceeds the solubility product, indicating that the solution is supersaturated and the excess ions will form a precipitate.

Step 1: Understanding Molar Ionic Conductivity
The molar ionic conductivity of an ion is influenced by its size and the ability to move through the solvent.
As the size of the ion increases, the molar ionic conductivity typically increases because larger ions experience less friction in solution.
Step 2: Explanation of the Trend
is the smallest ion in the group, so it has the lowest molar ionic conductivity.

is larger than and has a higher molar ionic conductivity.

is larger than , so its molar ionic conductivity is higher.
is the largest ion in the group, so it has the highest molar ionic conductivity.

Step 3: Conclusion
Thus, the correct order of molar ionic conductivities is .