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Solutions

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?

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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?

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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.

Answer:

The process of a solute dissolving in a solvent is called dissolution. Dissolution depend on the temperature because increasing temperture dissolution is also increase.
Dissolution also depend on the nature of the solute and solvent.

In the dissolution process, solute-solute, solvent-solvent interactions are established. The solubility of a solute thus, depends on the strength of new solute-solvent interactions relative to the strengths of solute-solute and solvent-solvent interactions.

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