State Raoult’s law for dilute solutions?

Answer:

The relative lowering of vapour pressure is equal to the mole fraction of solute in solution.
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Define Van’t Hoff factor ‘i’?

Answer:

van’t Hoff factor, to account for the extent of dissociation or association. This factor i is defined as:


i=Normal molecular massObserved molecular mass

For association ‘i’ is less than unity and for dissociation ‘i’ is greater than unity.
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Define an ideal solution.

Answer:

The solutions which obey Raoult’s law over the entire range of concentration are known as ideal solutions. The ideal solutions have two other important properties. The enthalpy of mixing of the pure components to form the solution is zero and the volume of mixing is
also zero, i.e.,
ΔmixH = 0, ΔmixV = 0

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Differentiate between molarity and Molality?

Answer:

Molarity: Molarity (M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of solution,


Molarity = Number of moles of soluteVolume of solution in litres

express unit in L-1

Molality: Molality (m) is defined as the number of moles of the solute per kilogram (kg) of the solvent and is expressed as:

Molality = Number of moles of soluteMass of solvent in kilograms

Express unit in Kg-1

molality are independent of temperature, whereas molarity is a function of temperature. This is because volume depends on temperature and mass does not.

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What is the Van’t Hoff factor of a compound which undergoes tetramerisation in an organic solvent?


Answer:
The van't hoff factor is an integer based on the number of particles that substance will dissociate into.
A compound undergoes tetramerisation have 
Van’t Hoff factor, i = 4.
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