VASANTH KUMAR G SOLUTIONS GPUC FOR GIRLS, PUTTUR

Test, Mid-Term question of Different district 15. Which of the following is NOT a colligative
1. Solubility of a substance is depends on property?
a) Nature of solute b) Temperature a)Lowering of vapour pressure (pᵒ–p) b).EBP (∆Tb)
c) Pressure d) all of these c) DFP (∆Tf) d) OP ( )
2. Raw mangoes shrivel into pickels when placed in the 16. Desalination of sea water is done by _______
concentrated solution NaCl due to (a) What is the effect of the following on the solubility
a) Osmosis b) Reverse Osmosis of a gas in a liquid? (i) Temperature (ii) Pressure
c) Osmotic pressure d) Pressure 17. Unit of molarity is;
3. Which of the following is a colligative property? a) moles/litre b) moles/kg
a) Osmosis b) Osmotic pressure c) kg/moles d)millimoles/gram
c) Optical activity d) Boiling point 18. Camphor dissolved in nitrogen gas is an example
4. Out of molality (m), molarity (M), parts per million for solution of the type;
(ppm) and mole fraction (x), which of this is temperature a)Liquid in liquid b) Solid in liquid
dependent? a) M b) x c) m d) ppm c) Solid in solid d) Solid in gas
5. The values Kb and Kf are are depends upon the nature 19. The maximum amount of a solute that can be
a) solution b) solvent c) solute d) none of the dissolved in a given amount of solvent at a given
above temperature is called __________
6. The ratio of number of moles of the solute per kilogram 20.Explain the effect of temperature on
of the solvent is ________. i) Solubility of gas in Liquid
7. State Henry’s law. Write its mathematical form ii) Solubility of Solid in Liquid with Exothermic and
8. Define Van’t Hoff factor (i). Give the value of ‘i’ for endothermic dissolution processes.
complete dimerization of all the molecules of ethanoic 21.A solution in which no more solute can be dissolved
acid in benzene at the same temperature and pressure is called
a) Unsaturated solution b) dilute solution
9. What is binary solution? Identify solute and solvent in a
b) Super saturated solution d) saturated solution
binary solution of ethanol.
22.In the phenomenon of osmosis, the membrane
10. Derive a relationship between RLVP of dilute solution
allow passage of
and molar mass of the non-volatile solute present in
a) Solute only b) Solvent only
volatile solvent.
c) both solute and solvent d) none of these
11.Calculate the mole fraction of urea (molar mass = 60 g
23.When non volatile solute is added to volatile
mol-1 ) in aqueous solution containing 40% of urea by
solvent, the boiling point of solvent
mass.
a)Increases b)decreases
12. Calculate the boiling point of the solution containing
2.34 g of non-volatile solute (molar mass = 58.0 g mol-1 ) in
c) remain same d) none of these
40 g of benzene. [Given: The boiling point and 24.Raw mangoes shrivel when pickled in brine
Ebullioscopic constant of pure benzene are 353.23 K and solution due to_____
2.53 K kg mol-1 respectively]. 25. Define Molarity. How does molarity varies with
13. At 373K, 0.31 mol of heptane is mixed with 0.26mol temperature?
of octane forms an ideal solution. Calculate the vapour 26. On mixing equal volume of acetone and ethanol,
pressure of this ideal solution. [Given: vapour pressure of what type of deviation from Raoult’s law is expected?
pure heptane and octane are 105.2 kPa and 46.8 kPa 27. What is the effect of rise in temperature on the
respectively]. solubility of gases in liquids?
14. Which of the following concentration term is 28.Write any three differences between ideal and non-
independent of temperature? ideal solution.
a. Volume percent b. Molarity
c. Molality d. Mole fraction
VASANTH KUMAR G
29. Heptane and octane form an ideal solution at 373K, the 46. Give two reason why molar mass of polymers,
vapour pressure of the two liquid components are proteins and biomolecule are more often determined
105.2Kpa and 46.8 kPa respectively. What will be the by measuring osmotic pressure rather than other
vapour pressure of a mixture of 26.0g of heptane and 35g colligative properties
of octane ? 47.The ratio of number of moles of the solute per
30.The value of Van’t Hoff fator (i) for Ethanoic acid in kilogram of the solvent is
benzene is nearly a)2 b) 1 c)0.5 d)3 a) Molarity b) Mole fraction
31. Because of low concentration of O2 in the blood and c)Parts per million d) Molality
tissues of people living at high altitude suffer from a 48.Oxygen dissolved in water is an example for___
disease called ______ 49.On what factors the value of colligative property
32. If 3.42g of solute dissolved in 500mL of a solvent depends
exerts the osmotic pressure is 0.4925atm at 270C. a)Number of atoms b) Number ions
Calculate the molar mass of the solute (R=0.0821 lit.atm c)Number of solute particles d) Number of moles
mol-1 K-1) 50.Van’t Hoff factor for a solution is more than one
34.15g of unknown, non-volatile compound raises the (> 1). It indicates
boiling point of 75g benzene(C6H6) by 0.2750C. Calculate a)dissociation b) association
the molecular mass of the unknown compound.(Kb for c) Multiplication d)division
benzene=5.1 K Kg mol-1) 51.which of the following statement is not correct
35.What is osmotic pressure? What will happen if pressure according to Henry’s law
greater than osmotic pressure is applied on the solution 1 1
a)KH ∝ b) KH ∝
𝑆𝑜𝑙𝑢𝑏𝑖𝑙𝑖𝑡𝑦 𝑆𝑜𝑙𝑢𝑏𝑖𝑙𝑖𝑡𝑦
separated by semipermeable membrane from the solvent? 1
36. When does a liquid boil? c)KH ∝ T d) T∝
𝑆𝑜𝑙𝑢𝑏𝑖𝑙𝑖𝑡𝑦
52.The van’t Hoff’s factor for glucose solution is
37.10gm of an organic substances was dissolved in two
a)0 b) 1 c) 2 d)0.5
litres of water gave an osmotic pressure of 0.59 atm at
53._____ in gold is the example for solid soution
70C. Calculate the molar mass of the substances(R=0.082L
54. The antifreeze is used in car radiator is
atm mol-1 K-1)
55.The law which indicates the relationship between
38.If Solute is present in trace amounts, then concentration
solubility of a gas in liquid and pressure is
is expressed in ___
a)Raoult’s law b) Henry’s law
39.Mention the factors on solubility of liquid solutions are
c) Lowering of vapour pressure d) van’t Hoff law
depends when the solute is. a) gas b) solid
56. The osmotic pressure of a solution can be
40. Give an example for gaseous solution in which solute
increased by
is a) gas b) solid c) liquid
a) increasing the volume
41.When doew Raoult’s law become a special case of
b) Increasing the number of solute molecule
Henry’s Law?
c) decreasing the temperature
a)KH < P10 b)KH > P10 c) KH =P10 d) None of these
d) removing semipermeable membrane
42. The Cryscopic Constant Kf depends on
57. Colligative property of a dilute solution depennds
a) Nature of solute b) Nature of solute particles
on
c) Nature of solvent d) all the above
a)Nature of solute b) nature of solute particles
43. Wilted flowers revive when placed in fresh water due
c) nature of solvent d) Number of solvent molecule
to a) Osmosis b) reverse osmosis
58. The value of Van’t Hoff factors for KCl, NaCl,
c) diffusion d) effusion
and K2SO4 respectively are
44.The process for purification of sea water is
a)2,2,& 2 b)2,2 & 3 c)1,1 &2 d)1,1 &1
called_______
59. Isotonic solution have same___
45. How does the boiling point of solvent vary, when a
60.The elevation in boiling point for one molal
non-volatile soute is dossolved in it? Give reason
solution of a solute in a solvent is called
VASANTH KUMAR G
a) Cryoscopic constant b) Freezing point constant 6) Low concentration of oxygen in the blood and
c) Molal Ebullioscopic constant tissues of people living at high altitude is due to _____
d) Molal depression constant .[NCERT]
61.If the solute dissociate then molecular mass is (a) low temperature (b) low atmospheric pressure
a) Increases c) Decreases (c) high atmospheric pressure
b) First increases then decreases d) Remains unchanged (d) both low temperature and high atmospheric
62.Desalination of sea water is application of ___ pressure
63. At a given temperature and pressure Nitrogen gas is 7) A molal solution is one that contains one mole of a
more soluble in water than Helium gas. Which one of solute in
them has higher value of KH. (a) 1000 g of the solvent (b) 1 L of the solvent
a) Helium b) Nitrogen c) Both a and b d) Neither a nor b (c) 1 L of the solution (d) 22.4 L of the solution
64.The cryoscopic constant Kf depends on 8) An ideal solution is formed when its components
a)nature o solute b)number of solute particles (a) have no volume change on mixing
c)nature of solvent d) all the above (b) have no enthalpy change on mixing
65.Wilted flowers revive when placed in fresh water due (c) have both the above characteristics
to a)Osmosis b) reverse osmosis (d) have high solubility
c) diffusion d) effusion 9) A liquid mixture boils without changing constituent
66.Benzene in ______ is an example for ideal solution. is called
Some Practice MCQS a) Stable structure complex b) Binary liquid mixture
1. If molality of the dilute solution is doubled, the value of c) Zeotropic liquid mixture
molal depression constant Kf will be [NEET 2017] d) Azeotropic liquid mixture
a) doubled b) halved c) tripled d) unchanged 10. During depression of freezing point in a solution
2. When an electrolyte is dissociated in solution, then the following are in equilibrium
Van’t Hoff’s factor (i) is (KCET-14) a) liquid solvent, solid solvent
a) > 1 b)<1 c) =0 d) =1 b) liquid solvent, solid solute
3.The Vant Hoff’s factor ‘i’ accounts for c) liquid solute, solid solute
a) extent of solubility of solute d) liquid solute, solid solvent
b) extent of dissociation of solute 11. Isotonic solutions are solutions having the same
c) extent of dissolution of solute (KCET-15)
d) extent of mobility of solute a) Surface tension b) Vapour pressure
4) Match the items given in Column I with the type of b) Osmotic pressure d) Viscosity
solutions given in Column II. [NCERT] 12.When the pure solvent diffuses out of the solution
through the semi-permeable membrane then the
process is called
a) Osmosis b) Reverse osmosis
c)Sorption d) Dialysis
13. All form ideal solution except
a)C6H6 and C6H5CH3 b) C2H5 Cl and C2H5I
c) C6H5 Cl and C6H5Br d) C2H5 I and C2H5OH
14.Which one of the following is incorrect for ideal
solution? [NEET 2016]
5) A non-ideal solution was prepared by mixing 30 ml a)ΔHmix =0 (b) ΔUmix =0 (c) ΔGmix =0
chloroform and 50 ml acetone. The volume of mixture (c) ΔP=P obs -P calculated by Raoult s law = 0
will be
a) > 80 ml b)< 80 ml c) = 80 ml d) ≥ 80 ml
 VASANTH KUMAR G SOLUTION GPUC FOR GIRLS, PUTTUR

Preparatory 2024 17. Define azeotropic mixture. Give an example for

1.Soda water is an example for minimum boiling azeotropes
a) Binary solution b) Quaternary solution 18.Give reason
c) Tertiary soution d) Not a solution i) Blood cell when placed in water swells (Osmosis)
2.Red-blood cell shrinks, when it is placed in a ii) Depression in freezing point of 0.1M aqueous
a) Hypotonic solution b) Hypertonic solution NaCl is nearly twice that of 0.1M glucose solution (
c) Isotonic solution d) saturated solution NaCl dissociate into two ions(Na+ &Cl-) number of
3. Give reason particle double where as glucose is non-electrolyte
a) soda water and soft drinks are sealed under high pressure does not dissociate)
(to increase the solubility of gas) 19. Increasing the temperature of an aqueous solution
b) The i-value or aqueous KCl is more than ethanol in will cause
benzene (because dissociation of KCl) a) decrease in molarity b) decrease in molality
4. Write any three differences between positive and c) decrease in mole fraction
negative deviation of Non-ideal solutions. d) decrease in mass %(w/w)
5.Acetic acid dissolved in benzene shows molecular mass 20.A solution of acetone in ethanol shows___
of a) 30 b) 60 c) 120 d) 180 deviation from Raolut’s law (positive)
6.The solubility gas in liquids____ with the increase in 21. State Raoult’s law. Write its mathematical
temperature. (decreases) expression
7. Relative lowering of vapour pressure is equal to the 22.Write any three characteristics of ideal solutions.
a) Mole fraction of the solute 23. Acetic acid dissolved in benzene shows a
c) Molarity of the solution molecular mass of a) 30 b) 60 c) 120 d) 180
b) Mole fraction of the solvent 24.Solubility of gas in liquid is
d) Molality of the solution a)increases with increase in temperature
8. If solute is present in trace amounts, then conc is (b) Decreases with increase in temperature
expressed in_____(ppm/parts per million) (c) Unaffected on changing the temperature
9. Mention any two applications of Henry's law (d) Decreases with increase in pressure
10. What is the SI unit of molality.(mol/Kg) 26.State Henry's law, write its Mathematical forn.
11.Which of the following modes of expressing How does Henry's constant varies with the solubility?
concentration is dependent of temperature? 27. If blood cell is placed in a solution containing less
a) Molarity b) Mole fraction than 0.9%(mass/volume) sodium chloride, then the
c)Parts per million d) Molality cell will___(swell)
12. The relationship between mole fraction of gas in 28. What is the value of Van’t Hoff factor for
solution and partial pressure over the solution is given Na2SO4(Assuming complete dissociation) (3/Three)
by___(Henry’s law) 29.The boiling point is lowest for the equimolar
13. Define azeotropic mixture. Give an example for aqueous solution containing
maximum boiling azeotropes a) NaCl b)C6H12O6 c) BaCl2 d) La(NO3)3
14. What are hypertonic solutions? Give an example 30.A solution in which no more solute can be
15. The dissolution of gas in a liquid is governed by dissolved is called___ solution (saturated)
a) raoult’s law b) henry’s law 31.Type of the solution obtained when copper
c) Boyle’s law d) Van’t Hoff factor dissolved in gold is
16. Solubility of a gas in liquid___ with decrease in a) Solid in solid solution b) Gas in gas solution
temperature (Increases) c) Liquid in liquid solution d) None of these
32. ____ law behind the dissolution of CO2 gas in soft
under high pressure (Henry’s)
33. On mixing equal volumes of acetone and ethanol, what 48.What is the effect of increase in temperature on
type of deviation from Raoult’s law is expected?(positive) the solubility of a solid in liquid, if the process of
34. Low concentration of oxygen in the blood and tissues dissolution is a) exothermic (decreases)
of people living at high altitude is due to ______(low b) endothermic (Increases)
atmospheric pressure) 49. According to Henry’s law partial pressure of the
35. Mixture of acetone and ethanol shows positive gas in the vapour phase is proportional to its
deviation from raoult’s law. Give reason. (Ethanol- a) Molarity b) Molality
Acetone interaction is weaker than ethanol-ethanol c)Mole fraction d) Mass percentage
interaction) 50. The solutions which show a larger positive
36. The Van’t Hoff factor I for a dilute aqueous solution of deviation from Raoult;s law are
sucrose is a)Zero b) One c) Two d) Three called____azeotropes (Minimum boiling)
37. A solution in which no more solute can be dissolved at 51. If the solute dissociates in solution, Van’t Hoff
the same temperature and pressure is called____ factor is a)>1 b) 0 c) <1 d)=1
solution.(saturated) 52. The semi permeable membrane used in the
38. Negative deviation from Raoult’s law is observed in reverse osmosis is _____(Cellulose acetate)
which of the following binary liquid mixture 53. Aquatic species are more comfortable in cold
a) Etahnol & acetone b) Benzene+Toluene water rather than in warm water. This is due to
c) Acetone+Chloroform d)Acetone and carbon disulphide a) solubility of oxygen is more in warm water.
39. The van’t Hoff factor for acetic acid in benzene is____ b) solubility of oxygen is more in cold water.
40. What happens to the solubility of a gas in a liquid with c) solubility of gases increases with decrease of
increase in temperature ? Give reason. (Decreases, temperature. d) both (b) and (c)
because solubility of a gas in a liquid is Exothermic 54. How does the boiling point of solvent varies,
41.What type of a azeotrope is formed by negative when a non-volatile solute is dissolved in it? Give
deviation from raoult’s law? Give an example (Maxium reason. (Boiling point increases, because adding
boiling azeotrope, 68% HNO3 +32% H2O) non-volatile solute vapour pressure of solvent
42. Which of the following conditions is not satisified by decreases)
an ideal Solution?
a)∆Hmixing=0 b)∆Vmixing=0 Practice Mcqs
c) Raoult’s law is obeyed
d) Formation of an azeotropic 1.When does Raoult’s law become a special case of
43. Osmotic pressure can be increased by___(increase in Henry’s Law?
concentration/Temperature) a) KH < P10 b)KH > P10
44. Molarity is b) c) KH =P10 d) None of these
a) Moles of solute/litre of solvent 2. The Cryscopic Constant Kf depends on
b) Moles of solute/litre of solution a) Nature of solute b) Nature of solute particles
c) Grams of solute /litre of solution c) Nature of solvent d) all the above
d) Moles of solute/kg of solvent 3. Wilted flowers revive when placed in fresh water
45. The unitless concentration term is______ due to
a)Mole freaction b) Mass percent a) Osmosis b) reverse osmosis
c)Molarity d) Both a & b c) diffusion d) effusion
46. Desalination of sea water can be done 4.The process of purification of sea water is
by_____(Reverse Osmosis) called_______(desalination)
47. Van’t Hoff factor for NaCl(assuming complete 5. Camphor dissolved in nitrogen gas is an example
dissociation) is_______(2/Two) for solution of the type;
a)Liquid in liquid b) Solid in liquid
c) Solid in solid d) Solid in gas
VASANTH KUMAR G
6. Which of the following is a colligative property? 7.At 200C, the vapour pressure of pure liquid A is 22
a) Osmosis b) Osmotic pressure mm of Hg and that of pure liquid B is 75 mm of Hg.
c) Optical activity d) Boiling point What is the mole fraction of these two components in
7. Out of molality (m), molarity (M), parts per million a solution that has a vapour pressure of 48.5mm of Hg
(ppm) and mole fraction (x), which of this is temperature at this temperature( assuming ideal behaviour)
dependent? a) M b) x c) m d) ppm
8.12.6 g of non -electrolyte is dissolved in 75g of
8. The values Kb and Kf are are depends upon the nature
water. The freezing point of this solution is 271.9K.
a) solution b) solvent c) solute d) none of the
Calculate molar mass of the solute.(Freezing point of
above
pure water & molar depression constant of water are
9.In the phenomenon of osmosis, the membrane allow
273.15K & 1.86 K Kg mol-)
passage of
a) Solute only b) Solvent only 9.32g of unknown molecular solid is dissolved in
c) both solute and solvent d) none of these 500g of water. The resulting solution freezes at 271.15
10. A solution in which no more solute can be dissolved at K. calculate the molar mass of this molecular
the same temperature and pressure is called solid.(Given; Kf for water is 1.86 K Kg mol-1
a) Unsaturated solution b) dilute solution
b) Super saturated solution d) saturated solution 10.800 cm3 of an aqueous solution of protein contains
Preparatory -24 (problems) 2.12 g of the protein. The osmotic pressure of such a
𝑀 solution at 300 K is found to be 3.89 × 10-3 bar.
1.Calculate the osmotic pressure of 5 %( ) solution of
𝑉 Calculate molar mass of protein. (R = 0.0823 L bar
urea at 300K(Molar mass of urea is 60g/mol) mol K-1).
2. 18gm of Glucose (C6H12O6) is dissolved in 1 Kg of
water in a saucepan. At what temperature will water boil 11.The vapour pressure of pure benzene at a certain
at 1.013 bar ? (kb for water is 0.52 K Kg mol-1, Molecular temperature is 0.850 bar. When a non-volatile, non
mass of glucose is 180 g/mol, B.P of water is 1000C) electrolyte solid weighing 0.5 grams is added to 39
3. An aqueous solution of glucose is 10% by mass of grams of benzene (Molar mass 78 grams). Vapour of
glucose at 303K, the vapour pressure of pure water at the solution is 0.845 bar. What is the molar mass of
303K is 32.8mm of Hg. What is the vapour prssure of the solid substance?
solution? 12. Vapour pressure of pure Chloroform(CHCl3) and
4. an aqueous solution of 0.6g of a solute X in 27.1 g of pure dichloromethane (CH2Cl2) at 298K are 200
water freezes at 272.187K. If the cryosccopic constant of mmHg and 415 mmHg respectively. Total vapour
water is 1.86 K Kg mol-1. Calculate the molecular mass of pressure of the binary s0oolution prepared by mixing
X CHCl3 and CH2Cl2 at 298K is 348 mmHg. Calculate
5. Vapour pressure of dichloromethane (molar Mass = partial vapour pressure of more volatile component
119.5g/mol) and chloroform (molar Mass 85g/mol) at and its mole fraction in vapour phase of the solution.
298K are 200 and 415 mm Hg respectively. Calculate the 13. Boiling point of water at 750mm Hg is 99.630C.
Vapour pressure of the solution prepared by mixing 25.5g How much sucrose [molar mass 342 g mol-1] is to be
dichloromethane and 40g of chloro form at 298 K added to 500 grams of water such that the solution
boils at 1000C[Given Kb=0.52K kg mol-1]
6.Vapour pressure of benzene is 200mm of Hg. When 2 14. Solubility of a gas in water 0.001m STP.
gram of a non-volatile dissolved in 78 grams of benzene. Determine its Henry’s law constant.
Benzene has Vapour pressure of 195mm of Hg. Calculate 15. The vapour pressure of water is 12.3kPa at 300K.
the molar mass of the solute.(molar mass of benzene is 78 Calculate Vapour pressure of 1 molal solution of a
g mol- non-volatile solute in it.

VASANTH KUMAR G
16. The mixture of 95% ethyl alcohol & 5% water by 4)Write any three differences between ideal and non-
volume shows which type of azeotrope? ideal solution
a) Maximum boiling azeotrope 5)The boiling point of benzene is 353.23 K. When 1.80
b)Minimum boiling azeotrope g of a non-volatile solute was dissolved in 90 g of
c) Bothe Minimum and maximum boiling azeotrope benzene, the boiling point is raised to 354.11 K.
d) None of the above Calculate the molar mass of the solute. Kb for benzene
17.If Henry’s Constant (KH) value increase the solubility of is 2.53 K kg mol–1
gas in liquid is____(decreases) 6)Vapour pressure of compound ‘A’ (molar mass 120
18. Calculate the mass of urea(NH2-CO-NH2) required to g/mol) and compound ‘B’ ( Molar mass 85 g/mol) at
making 2.5 Kg of 0.25 molal aqueous solution
298 K are 200 mm Hg and 415 mm Hg respectively.
Board Exam- 2014 to 2024 Calculate the vapour pressure of the solution prepared
2024 by mixing 26.0 g of compound ‘A’ and 40 g of
Exam-1 compound ‘B’ at 298 K
1) If the process of dissolution of a solid in liquid is an Exam-3
endothermic, its solubility 1)Van’t Hoff factor (i) for complete dissociation of
a) decrease with increase in temperature K2SO4 a) 0 b) 1 c) 2 d) 3
b) remains same at all temperature 2) The solubility of a solid in a liquid _____ with
c) increase with increase in temperature temperature for endothermic process
d) increase with decrease in temperature 3) State Henry’s law. Write an application of it
2) The number of moles of solute present in one 4) It is not possible to separate the componenets of
kilogram of the solvent is called____ azeotropes by fractional distillation. Give reason
3) What type of deviation from Raoult’s law is observed, 5) Calculate the mole fraction of NaOH and water if 4g
when equal volume of ethanol and acetone are mixed of NaOH is dissolved in 90 g of water (Molar mass of
together? Mention the reason for it NaOH= 40 g mol-1 , Molar mass of water= 18 g mol-1
4) What is Reverse Osmosis? Mention one of its 6) A non-electrolyte solute with molar mass 256 g mol-
application. 1
dissolved in 100 g of benzene lowered the freezing
5) State Henry’s Law point of benzene by 0.40 K. The freezing point
6) Calculate the mole fraction of benzene in a solution depression constant o benzene is 5.2 K Kg mol -1. Find
contatining 30% by mass in carbon tetrachloride, (Molar the mass of solute dissolved.
mass of benzene= 78 g/mol, Molar mass of carbon A-2023
tetrachloride=154 g/mol) 1) A binary liquid mixture that forms maximum boiling
7) 1.00 g of a non-electrolyte solute dissolved in 50g of azeotrope at a specific composition is
benzene lowered the freezing point of benzene by 0.40K. a) Ethanol + Water b) n - Hexane + n- Heptane
the freezing point depression constant of benzene is 5.12K
c) Benzene + Toluene d) Nitric acid + Water
Kg mol-1. Find the molar mass of the solute.
2)The value of van’t Hoff factor (i) for ethanoic acid in
Exam-2 benzene is nearly a) 2 b) 1 c) 0.5 d) 0
1)To determine molar mass of biomolecules and 3)Because of low concentration of O2 in the blood and
Polymers, which Colligative property based method has tissues of people living at high altitudes, suffer from a
advantage over other methods? disease called ________
a) Relative lowering of vapour pressure 4) 450cm3 of an aqueous solution of a protein contains
b) Elevation of boiling point 1.0g of the protein. The osmotic pressure of such a
c) Depression in freezing point d) Osmotic pressure solution at 310K is found to be 3.1 X 10−4 bar.
2)___ is number of moles of solute dissolved in one litre Calculate the molar mass of the protein. (R =
of solution 0.083Lbar mol-1 K -1).
3) What happens to solubility of gas in liquid when 5) State Raoult’s law of relative lowering of vapour
i) Pressure is increased ii) Temperature is increased pressure. Write its mathematical form.
VASANTH KUMAR G
S-2023 2) Sodium chloride solution having concentration
1) Which of the following is a colligative property? greater than 0.9% (mass/volume) is not safe to inject
a) Osmosis b) Osmotic pressure intravenously - Give reason.
c) Optical activity d) Boiling point 3) Give any two differences between ideal and non-
2) Which of the following term is dependent on ideal solutions.
temperature? a) Molarity b) Mole fraction 4) 31g of an unknown material is dissolved in 500g
c) Molality d) Mass percentage (w/w) of water. The resulting solution freezes at 271.14K.
3) 1.00g of a non-electrolyte solute dissolved in 50g of Calculated the molar mass of the material. [Given: Kf
benzene lowered the freezing point of benzene by 0.40K. for water = 1.86 K kg mol-1 & Tof for water = 273K]
the freezing point depression constant of benzene is 5) What are azeotropes?
5.12Kkgmol-1 . Find the molar mass of the solute. 6) Which type of azeotrope shows a large deviation
4) Define Van’t Hoff factor (i). give the value of ‘i’ for from Raoult’s law?
complete dimerization of all the molecules of ethanoic A– 2020
acid in benzene 1) How does the size of blood cells change when
S-2023(second supplementary) placed in an aqueous solution containing more than
1)The ratio of number of moles of the solute per kilogram 0.9% (m/v) sodium chloride?
of the solvent a)Molarity b) Mole fraction 2) How does the volume change on mixing two
c)Parts per million d) Molality volatile liquids to form an ideal solution?
2) The liquid solution in which solute is liquid is, 3) 31 g of an unknown molecular material is
a) Ethanol dissolved in water dissolved in 500 g of water. The resulting solution
b) Oxygen dissolved in water freezes at 271.14K. Calculate the molar mass of the
c) CO2 dissolved in water material. [Given: Kf for water = 1.86 KKgmol-1 , of
d) Glucose dissolved in water water = 273K].
3) ___ are the constant boiling binary mixture having 4) What is reverse osmosis? Mention its use.
same composition in liquid and vapour phase S– 2020
4) 0.3 L of an aqueous solution contains 1.89 g of the 1) Define molality.
protein . At 300 K, the osmotic pressure of this solution 2) The KH values for Nitrogen gas (N2) at 293K and
was found to be 2.57 x 10-3 bar. Calculate the molar mass 303K are 76.48Kbar and 88.84Kbar respectively.
of the protein. [R= 0.083 L bar mol-1 K-1) Among these two given temperatures, at which
5) State Henry’s law. Give its Mathematical form. temperature Nitrogen gas is more soluble in water?
A-2022 3) 1.00g of a non-electrolyte solute is dissolved in
1) Mention one practical utility of reverse osmosis. 50g of benzene lowers the freezing point of benzene
2) At constant temperature, different gases have different by 0.4K. The freezing point depression constant for
KH – value. What does this statement suggest? benzene is 5.12KKgmol-1 . Find the molar mass of
3) Define molarity (M). How does molarity vary with solute.
temperature? 4) State Henry’s law. Write its mathematical form.
4) On dissolving 3.46g of solute in 100g of water, the A – 2019
boiling point of solution was raised to that of pure water 1) How does the size of blood cells change when
by 0.12K. Calculate the molar mass of the non–volatile placed in an aqueous solution containing more than
solute. (Given: Kb of water is 0.51Kkgmol-1 ) 0.9% (m/v) sodium chloride?
5) What type of deviation from Raoult’s law is observed 2) How does the volume change on mixing two
When equal volume of ethanol and acetone are mixed? volatile liquids to form an ideal solution?
Mention the reason for it. 3) 31 g of an unknown molecular material is
S-2022 dissolved in 500 g of water. The resulting solution
1) State Henry’s law freezes at 271.14K. Calculate the molar mass of the
material. [Given: Kf for water = 1.86 KKgmol-1 , of
VASANTH KUMAR G water = 273K].
4) What is reverse osmosis? Mention its use. S– 2017
S – 2019 1) State Raoult’s law of a binary solution for two
1) Write the unit of molarity of solution. volatile liquid components.
2) At a given temperature, oxygen gas is more soluble in 2) Van’t Hoff factor for a solution is more than one.
water than Nitrogen gas. Which one of them has higher What is the conclusion drawn from it.
value of KH? 3) On dissolving 2.34 g of non-electrolyte 3) The vapour pressure of pure benzene at a certain
solute in 40 g of benzene the boiling point of solution was temperature is 0.850 bar. A non-volatile, non-
higher than benzene by 0.81 K. Kb value for benzene is electrolyte solid weighing 0.5 g, when added to 39.0
2.53 K kg mol-1. Calculate the molar mass of solute. [Molar g of benzene (molar mass of benzene 78 g mol-1 )
mass of benzene is 78 g mol- vapour pressure of the solution then is 0.845 bar.
4) State Henry’s law. What is the molar mass of the solid substance?
5) How solubility of a gas in liquid changes with increase 4) What is Reverse Osmosis? Mention its one
in temperature? practical utility.
A- 2018 A – 2016
1) State Henry’s law. 1) State Raoult’s law for liquid mixtures.
2) Van’t Hoff’s factor for a solution is less than one, what is 2) Define molality
the conclusion drawn from it. 3) 200 cm3 of an aqueous solution of a protein
3) The boiling point of benzene is 353.23 K when 1.80g of contains 1.26 g of protein. The osmotic pressure of
a non volatile, non-ionising solute was dissolved in 90 g of such a solution at 300 K is found to be 2.57 × 10-3
benzene, the boiling point is raised to 354.11K. Calculate bar. Calculate the molar mass of the protein.
the molar mass of the solute. [Given Kb for benzene = 2.53 Re-Exam A – 2016
K kg mol-1 ] 1) Name the law behind the dissolution of CO2 gas
4) Define i) Molality of a solution. ii) Isotonic solutions. in soft drinks under high pressure.
S – 2018 2) Ornamental gold containing copper is an example
1) State Henry’s law. for what type of solution?
2) In a binary solution, mole fraction of one component is 3) 5.8 g of a non volatile solute was dissolved in 100
0.068. What is the mole fraction of another component? g of carbon disulphide (CS2). The vapour pressure of
3) 5.8 g of non-volatile, non-electrolyte solute was the solution was found to be 190 mm. of Hg.
dissolved in 100 g of carbon disulphide (CS2). The vapour Calculate the molar mass of the solute given the
pressure of the solution was found to be 190mm of Hg. vapour pressure of pure CS2 is 195 mm. of Hg
Calculate molar mass of the solute. Given: Vapour pressure [Molar mass of CS2 = 76 g mol-1 ]
of pure CS2 is 195mm of Hg and molar mass of CS2 is 4) Mention any two difference between ideal and non
76g/mol. ideal solutions.
4) Mention any two differences between ideal and non- S – 2016
ideal solutions. 1) What are ideal solutions?
A– 2017 2) What is the effect of rise in temperature on the
1) How does molarity varies with temperature? solubility of gases in liquids?
2) 10mL of liquid ‘A’ is mixed with 10 mL of liquid ‘B’, 3) 300 cm3 of an aqueous solution of a protein 2.12 g
the volume of the resultant solution is 19.9 mL. What type of the protein, the osmotic pressure of such a solution
of deviation expected from raoult’s law? 3) a) 1.0 g of non- at 300 K is found to be 3.89 × 10-3 bar. Calculate the
electrolyte solute dissolved in 50 g of benzene lowered the molar mass of the protein.(R = 0.0823L bar mol-1 K-1
freezing point of benzene by 0.4 K. Find the molar mass of 4) state Henry’s law.
the solute. [Given: Freezing pont depression constant of 5) Soda water bottles are sealed under high pressure.
benzene = 5.12 K. kg mol-1 ] Give reason.
3) How solubility of a gas in liquid varies with
i) Temperature and ii) Pressure.
VASANTH KUMAR G
A– 2015
1) At a given temperature and pressure nitrogen gas is more
soluble in water than Helium gas. Which one of them has
higher value of KH?
2) On mixing equal volumes of acetone and ethanol, what
type of deviation from Raoult’s law is expected?
3) A solution containing 18 g of non-volatile non-
electrolyte solute is dissolved in 200 g of water freezes at
272.07 K. Calculate the molecular mass of solute. Given:
Kf = 1.86K kg/mol freezing point of water = 273k
4) Define isotonic solution. What happens when the blood
cells is dipped in a solution containing more than normal
saline concentration?
S – 2015
1) On what factor the value of colligative property
depends?
2) Give an example for liquid solution in which solute is
gas.
3) The boiling point of benzene is 353.23K when 1.80 g of
a non-volatile, non-ionising solute was dissolved in 90 g of
benzene, the boiling point is raised to 354.11K. Calculate
the molar mass of the solute. [Given Kb for benzene = 2.53
K kg mol-1 ]
4) Write two differences between ideal and non-ideal
solutions.
A– 2014
1.Define the term ‘molarity’
2. Mention the enthalpy of mixing (∆mix H) value to form
an ideal solution.
3. On dissolving 2.34 g of solute of 40 g of benzene, the
boiling point of solution was higher than that of benzene
by 0.81 K, Kb value for benzene is 2.53 K kg mol-1 .
Calculate the molar mass of the solute.
4.State Henry’s law. Write its mathematical form.
S – 2014
1) What is binary solution?
2) Define molarity.
3) The vapour pressure of pure benzene at certain
temperature is 0.850 bar. A non-volatile, non-electrolyte
solid weighing 0.5 grams when added to 39 grams of
benzene (molar mass 78 grams), vapour pressure of the
solution, then is 0.845 bars. What is the molar mass of the
solid substance? 3m
4) What happens to the solubility of a gas in a liquid with
increase in temperature?