WorksheetsQuiz on Raoult’s Law and Colligative Properties
Total questions: 20
Worksheet time: 20mins
Raoult's law for a solution of volatile liquids states that the partial vapour pressure of each component is directly proportional to its:
Molarity
Molality
Mole fraction
Mass percentage
In a binary solution of volatile liquids, the total vapour pressure is given by:
$$ P_{total} = P_1 + P_2 $$
$$ P_{total} = x_1P_1^0 + x_2P_2^0 $$
$$ P_{total} = x_1x_2P_1^0 $$
$$ P_{total} = x_1P_1^0 - x_2P_2^0 $$
According to Raoult’s law, for a solution of non-volatile solute in a volatile solvent, the vapour pressure of the solution is:
Higher than the pure solvent
Equal to the pure solvent
Lower than the pure solvent
Unaffected
If a solution follows Raoult’s law over the entire range of concentration, it is called:
Non-ideal solution
Ideal solution
Azeotrope
Saturated solution
An ideal solution has which of the following properties?
∆Hmix ≠ 0
∆Vmix = 0
Both i and ii
None of these
A mixture of which of the following is nearly an ideal solution?
Ethanol and Water
Benzene and Toluene
Acetone and Chloroform
Water and HCl
If the observed vapour pressure of a binary solution is greater than that predicted by Raoult's law, the solution shows:
No deviation
Positive deviation
Negative deviation
Constant deviation
In a solution of phenol and aniline, deviation from Raoult’s law is:
Positive
Negative
Zero
Unpredictable
Minimum boiling azeotrope is formed by a solution showing:
Positive deviation from Raoult’s law
Negative deviation from Raoult’s law
No deviation
All of the above
Which type of intermolecular force is responsible for negative deviation from Raoult's law?
Weaker solute-solvent forces than pure components
Stronger solute-solvent forces than pure components
Van der Waals only
London dispersion only
Colligative properties depend on:
The nature of solute particles
The number of solute particles
The density of solute particles
Colour of solute
Which of the following is NOT a colligative property?
Lowering of vapour pressure
Depression of freezing point
Molar conductivity
Osmotic pressure
Relative lowering of vapour pressure is equal to:
Mole fraction of solvent
Mole fraction of solute
Product of mole fractions of solute and solvent
Square of mole fraction of solute
Which of the following will cause an elevation in boiling point for a solution?
Addition of a non-volatile solute
Removal of solvent
Addition of volatile solute
Increase in atmospheric pressure
For dilute solutions, the depression in freezing point is directly proportional to:
Volume of solvent
Molality of solution
Molarity of solution
Normality of solution
Osmotic pressure ($$ \Pi $$) for dilute solutions is related to molarity $$ C $$ and temperature $$ T $$ as:
$$ \Pi = nRT $$
$$ \Pi = CRT $$
$$ \Pi = MRT $$
$$ \Pi = P/RT $$
The unit of ebullioscopic constant (K_b) is:
K kg mol⁻¹
K L mol⁻¹
K mol L⁻¹
K mol kg⁻¹
The addition of urea to water causes:
Increase in vapour pressure
Decrease in freezing point
Decrease in boiling point
No effect on boiling point
For a salt that dissociates completely into three ions in solution, the expected van’t Hoff factor $$ i $$ is:
1
2
3
4
The experimentally determined molar mass of a solute that associates in solution is:
Lower than its actual value
Equal to its actual value
Higher than its actual value
Cannot be determined
