CHAPTER 02 SOLUTION MARKS 05
2001 set I
Q1 What do you understand by colligative properties?Write them. 03M
Q2 (a)Show graphically that the freezing point of a liquid will be depressed when a non
volatile solute is dissolved in it. 02M
(b)The freezing point of a solution containing 0.3gm of acetic acid in 30.0gm of benzene is
lowered by 0.450C.calcualte the vant Hoff factor (Kf for benzene = 5.12KKgmol-) 03M
Q3 One litre aqueous solution of sucrose (mm =342gmmol -) weighting 1015gm is found to record
on osmotic pressure of4.82 atm at 293K. What is the molarity of the sucrose solution?(R=
0.0821 atm mol-K-) 3M
2001 set II
Q1 (a) Show graphically how the vapour pressure of solvent and a solution in it of a nonvolatile
solute change with temperature . Show on this graph the boiling points of the solvent and
solution . Which is higher and why? 02M
(b) A solution containing 3.00g of BaCl2 in 250g of water boils at 100.0830C.Calculate the
value of vant hoff factor and molality of BaCl 2 in this solution.( Kbfor water =0.52KKmol- molar
mass of BaCl2 =208.3gmol-) 3M
2002
Q1 Calculate the number of moles of methanol in 5 litre of its 2m solution. If the density of
the solution is 0.981Kg/l (Molecular mass of methanol = 32.0gmmol -) 02M
Q2 Explain with suitable diagram and appropriate example, why some non ideal solution
shows negative deviations. 03M
2003 SET 1
Q1 An aqueous solution containing 1.248g of BaCl 2(mm = 208.34gmol-) in 100 g of water
boils at 100.08320C.Calcualate the degree of dissociation of BaCl 2 (Kb for water is 0.52KKgmol-) 03M
Q2 What are ideal non ideal solutions.Explain with the suitable diagram the behavior of
ideal solution OR 05M
Assuming complete dissociation, Calculate the expected freezing point of a solution ,
prepared by dissolving 6.00g of Glaubers salt (NaSO 4.10H2O) in 0.100Kg of water)Kf = 1.86KKgmol-
05M2003set IIQ1 What is meant by Vant Hoff factor? The osmotic pressure of a 0.0103 molar
solution of
an electrolyte is found to be 0.70 atm at 27 0C. Calculate the Vant Hoff factor (R = 0.082Latm-
mol-K-) What conclusion do you draw about the molecular state of the solute in the solution? 5
2004
Q1 What is the sum of the molecular fraction of all the components in the 3 component System 1M
Q2 Define following terms(i)Mole fraction (ii) molarity 02M
Q3 The elements A and B form purely covalent compounds having molecular formulae AB 2 and
AB4. When dissolved in 20g of benzene 1gm of AB 2 lowers the freezing point by 2.3K whereas
1gm of AB4 lowers it by 1.3K .The molar depression constant for benzene is 5.1KKgmol -.
Calculate the atomic mass of A and atomic mass of B. 3M
2005
Q1 Calculate the molality of a solution containing 20.7g of K2CO3. Dissolved in 500ml of
solution assume density is 1g/ml3 2M
Q2 What would be the value of Vant Hoff factor for a dilute solution of K 2SO4 in water 1M
Q3 State Henrys law for solubility of a gas in a liquid. Explain the significance of Henrys law
, constant(KH). at the same temperature , hydrogen is mole soluble in water than helium. Which
will have a higher value of KH and why? 3M
2006
Q1 Define mole fraction .1M Q2. Define an ideal solution. 1M
Q3 (a)Urea forms an ideal solution in water. Determine the vapour pressure of an aqueous
soln containing 10% by mass of urea at 40 0C vapour pressure of water at 40 0C is 55.3 mmHg.3M
(b)Why is freezing point depression of 0.1 M NaCl solution twice that of 0.1 M glucose solution.1M
2007
Q1. State the condition resulting in reverse osmosis. 1M
Q2 A 0.1539 molal aqueous solution of cane sugar (M=342 g mol -) has a freezing point of 271K
while the freezing point of pure water is 273.15K. What will be the freezing point of on aqueous
solution containing 5g of glucose (M=180 g mol-) per 100 g of solution. 3M
2008
Q1 State Raoult’s law for solution for volatile liquids components. Taking a suitable example.
Explain the meaning of deviation from Raoult’s law. 2M
Q2 Define osmotic pressure and describe how the molecular mass can be determined on the basis of
osmotic pressure measurement. 02M
2008 comportment
1State the law, correlating the pressure of a gas and its solubility in a liquid. State an application of this
law.
2State Raoults law for Solution of volatile liquid components. Taking a suitable example explain the
meaning of (+) deviation.
3A Solution containing 8 gm of a substance in 100 gm of diethyl ether boils at 36.86 C whereas pure
ether boils at 35.600C. Determine the mole mass of solute Kb=2.02 KKg/ mol)
4Calculate the temp. at which a soln containing 54 gm of glucose in 250 g of water will freeze
(Kf=1.)
2009
Q1 a) Define i) Mole fraction ii) Vant Hoff factor 2M
b) 100mg of a protein is dissolved in enough water to make 10ml of a solution. If this solution
has an osmotic pressure of 13.3mm Hg at 25 0 C. What is the molar mass of the protein?
R=0.0821 Latm mol- k-) and 760 mm Hg=1atm 3M
OR
What do you know by 1) Colligative properties and 2) Molality of solution 2M
b) What con. of nitrogen should be present in a glass of water at room temperature?
Assume a temp of 250C, total pressure is 1 atm and mole fraction of Nitrogen in air is 0.78. K H is
8.42 X10-7M/mmHg for nitrogen. 3M
2010
Q1 Differentiate between molarity & molality. 1M
Q2 Define the terms - Osmosis and Osmotic pressure. What is the advantage of using osmotic pressure
as compared to other colligative properties for the determination of molar masses of solutes in
Solution . 2M
Q3 What mass of ethylene glycol (M=62.0g/mol) must be added to 5.50kg of water from 0 0C to -100C
(Kf for water = 1.86kg/mol) 3M
Q4 15g of an unknown molecular substance was dissolved in 450g of water. The resulting solution
freezes at -0.340C. What is the molar mass of the substance (K f for water is 2.86KKg mol-)3M
Q5 What mass of NaCl (58.5g/mol) must be dissolved in 65g of water to lower the freezing point by 7 .
2001 set I
Q1 What do you understand by colligative properties?Write them. 03M
Q2 (a)Show graphically that the freezing point of a liquid will be depressed when a non
volatile solute is dissolved in it. 02M
(b)The freezing point of a solution containing 0.3gm of acetic acid in 30.0gm of benzene is
lowered by 0.450C.calcualte the vant Hoff factor (Kf for benzene = 5.12KKgmol-) 03M
Q3 One litre aqueous solution of sucrose (mm =342gmmol -) weighting 1015gm is found to record
on osmotic pressure of4.82 atm at 293K. What is the molarity of the sucrose solution?(R=
0.0821 atm mol-K-) 3M
2001 set II
Q1 (a) Show graphically how the vapour pressure of solvent and a solution in it of a nonvolatile
solute change with temperature . Show on this graph the boiling points of the solvent and
solution . Which is higher and why? 02M
(b) A solution containing 3.00g of BaCl2 in 250g of water boils at 100.0830C.Calculate the
value of vant hoff factor and molality of BaCl 2 in this solution.( Kbfor water =0.52KKmol- molar
mass of BaCl2 =208.3gmol-) 3M
2002
Q1 Calculate the number of moles of methanol in 5 litre of its 2m solution. If the density of
the solution is 0.981Kg/l (Molecular mass of methanol = 32.0gmmol -) 02M
Q2 Explain with suitable diagram and appropriate example, why some non ideal solution
shows negative deviations. 03M
2003 SET 1
Q1 An aqueous solution containing 1.248g of BaCl 2(mm = 208.34gmol-) in 100 g of water
boils at 100.08320C.Calcualate the degree of dissociation of BaCl 2 (Kb for water is 0.52KKgmol-) 03M
Q2 What are ideal non ideal solutions.Explain with the suitable diagram the behavior of
ideal solution OR 05M
Assuming complete dissociation, Calculate the expected freezing point of a solution ,
prepared by dissolving 6.00g of Glaubers salt (NaSO 4.10H2O) in 0.100Kg of water)Kf = 1.86KKgmol-
05M2003set IIQ1 What is meant by Vant Hoff factor? The osmotic pressure of a 0.0103 molar
solution of
an electrolyte is found to be 0.70 atm at 27 0C. Calculate the Vant Hoff factor (R = 0.082Latm-
mol-K-) What conclusion do you draw about the molecular state of the solute in the solution? 5
2004
Q1 What is the sum of the molecular fraction of all the components in the 3 component System 1M
Q2 Define following terms(i)Mole fraction (ii) molarity 02M
Q3 The elements A and B form purely covalent compounds having molecular formulae AB 2 and
AB4. When dissolved in 20g of benzene 1gm of AB 2 lowers the freezing point by 2.3K whereas
1gm of AB4 lowers it by 1.3K .The molar depression constant for benzene is 5.1KKgmol -.
Calculate the atomic mass of A and atomic mass of B. 3M
2005
Q1 Calculate the molality of a solution containing 20.7g of K2CO3. Dissolved in 500ml of
solution assume density is 1g/ml3 2M
Q2 What would be the value of Vant Hoff factor for a dilute solution of K 2SO4 in water 1M
Q3 State Henrys law for solubility of a gas in a liquid. Explain the significance of Henrys law
, constant(KH). at the same temperature , hydrogen is mole soluble in water than helium. Which
will have a higher value of KH and why? 3M
2006
Q1 Define mole fraction .1M Q2. Define an ideal solution. 1M
Q3 (a)Urea forms an ideal solution in water. Determine the vapour pressure of an aqueous
soln containing 10% by mass of urea at 40 0C vapour pressure of water at 40 0C is 55.3 mmHg.3M
(b)Why is freezing point depression of 0.1 M NaCl solution twice that of 0.1 M glucose solution.1M
2007
Q1. State the condition resulting in reverse osmosis. 1M
Q2 A 0.1539 molal aqueous solution of cane sugar (M=342 g mol -) has a freezing point of 271K
while the freezing point of pure water is 273.15K. What will be the freezing point of on aqueous
solution containing 5g of glucose (M=180 g mol-) per 100 g of solution. 3M
2008
Q1 State Raoult’s law for solution for volatile liquids components. Taking a suitable example.
Explain the meaning of deviation from Raoult’s law. 2M
Q2 Define osmotic pressure and describe how the molecular mass can be determined on the basis of
osmotic pressure measurement. 02M
2008 comportment
1State the law, correlating the pressure of a gas and its solubility in a liquid. State an application of this
law.
2State Raoults law for Solution of volatile liquid components. Taking a suitable example explain the
meaning of (+) deviation.
3A Solution containing 8 gm of a substance in 100 gm of diethyl ether boils at 36.86 C whereas pure
ether boils at 35.600C. Determine the mole mass of solute Kb=2.02 KKg/ mol)
4Calculate the temp. at which a soln containing 54 gm of glucose in 250 g of water will freeze
(Kf=1.)
2009
Q1 a) Define i) Mole fraction ii) Vant Hoff factor 2M
b) 100mg of a protein is dissolved in enough water to make 10ml of a solution. If this solution
has an osmotic pressure of 13.3mm Hg at 25 0 C. What is the molar mass of the protein?
R=0.0821 Latm mol- k-) and 760 mm Hg=1atm 3M
OR
What do you know by 1) Colligative properties and 2) Molality of solution 2M
b) What con. of nitrogen should be present in a glass of water at room temperature?
Assume a temp of 250C, total pressure is 1 atm and mole fraction of Nitrogen in air is 0.78. K H is
8.42 X10-7M/mmHg for nitrogen. 3M
2010
Q1 Differentiate between molarity & molality. 1M
Q2 Define the terms - Osmosis and Osmotic pressure. What is the advantage of using osmotic pressure
as compared to other colligative properties for the determination of molar masses of solutes in
Solution . 2M
Q3 What mass of ethylene glycol (M=62.0g/mol) must be added to 5.50kg of water from 0 0C to -100C
(Kf for water = 1.86kg/mol) 3M
Q4 15g of an unknown molecular substance was dissolved in 450g of water. The resulting solution
freezes at -0.340C. What is the molar mass of the substance (K f for water is 2.86KKg mol-)3M
Q5 What mass of NaCl (58.5g/mol) must be dissolved in 65g of water to lower the freezing point by 7 .
