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Long Answer Type

111. Define vapour pressure of a liquid. What happens to the vapour pressure of a liquid when (a) a volatile solute dissolves in it and (b) a non-volatile solute dissolves in it?

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Short Answer Type

112. What is osmotic pressure? How is it dependent on the number of moles of a solute?

Answer:

The minimum excess pressure that has to be applied on the solution to prevent the entry of the solvent in to the solution through the semi-premeable membrane is called the osmotic pressure. It is given by:

osmotic pressure is proportional to the molarity, C of the solution at a given temperature T. Thus:
Π = C R T
Here Π is the osmotic pressure and R is the
gas constant.
Π = (n2 /V) R T

where

π

is the osmotic pressure.
n is the number of moles of solute.
v is volume of solution.
r is the universal gas constant.
T is the absolute temperature.

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113. State Raoult’s law. If AT is the elevation of boiling point of a solvent and m is the number of moles of solute per kg of solvent, what is the realationship between T and m?

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114.

(a) What are non-ideal solution?
(b) What role does the molecular interaction play in deciding the vapour pressure of solutions (i) alcohol and kerosene (ii) Chloroform and acetone.

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115. Why do colligative properties of an electrolyte solution of a given concentration are found to be larger than those of a non-electrolyte solution of the same concentration?

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116. Explain the following phenomena:
(i) Hemolysis
(ii) Crenation.

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117. Why do we observe abnormal molecular masses?

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118. How does osmotic pressure depend on molality of the solution?

179 Views

Long Answer Type

119. The molar mass of acetic acid determined from the measurement of a colligative property is greater than its formula molar mass. Explain why?

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Short Answer Type

120. Explain why solvent-solvent, solute-solute and solute-solvent interactions are important in determining the extent to which a solute dissolves in a solvent.

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