Q.1 Which of the following solutions would
have the highest osmotic pressure -
[AIPMT-91]
(1) NaCl (2) Urea
(3) BaCl2 (4) Glucose
Q.2 Which
of the following solution has the highest boiling point - [AIPMT-91]
(1)
0.1 M glucose (2) 0.1 M BaCl2
(3)
0.1 M NaCl (4) 0.1 M Urea
Q.3 Which
of the following is a colligative property - [AIPMT-92]
(1)
Viscosity (2)
Surface tension
(3)
Optical rotation (4) Osmotic
pressure
Q.4 The
compound whose 0.1 M solution has maximum osmotic pressure at 25°C will be -
[AIPMT-94]
(1)
CaCl2 (2) KCl
(3)
Glucose (4) Urea
Q.5 Which
of the following salt has the same value of Vont Hoff’s factor as that of K3[Fe(CN)6] [AIPMT-94]
(1)
Al2(SO4)3 (2) NaCl
(3)
Al(NO3)3 (4)
Na2SO4
Q.6 According
to raoult’s law the relative lowering of vapour pressure for a solution is
equal to - [AIPMT-95]
(1)
Moles of solute
(2)
Mole fraction of solvent
(3)
Moles of solvents
(4)
Mole fraction of solute
Q.7 The
relationship between osmotic pressure at 273 K when 10 g glucose (P1) 10 g urea (P2) and 10 g sucrose (P3) are dissolved in 250 ml of water is - [AIPMT-96]
(1)
P1 > P2 > P3 (2)
P3 > P1 > P2
(3)
P2 > P1 > P3 (4)
P3 > P2 > P1
Q.8 The
vapour pressure of an ideal solution having 0.2 Mole non-volatile solute &
0.8 mole solvent, is 60 mm. The vapour pressure of pure solvent at this
temperature will be - [AIPMT-96]
(1)
120 mm (2) 150 mm
(3)
60 mm (4) 75 mm
Q.9 Vapour
pressure of CCl4 at 25°C is 143 mm Hg. 0.5 gm of a non-volatile
solute (mol. wt. 65) is dissolved in 100 ml of CCl4. Find the vapour pressure of the
solution. (Density of CCl4
1.58 gm/cm3) [AIPMT-96]
1.58 gm/cm3) [AIPMT-96]
(1)
141.93 mm (2) 94.39
mm
(3)
199.34 mm (4) 143.9
mm
Q.10 The
vapour pressure decreases by 10 mm of Hg when solute’s mole fraction in a
solution is 0.2. If the vapour pressure decreases is 20 mm of Hg then the mole
fraction of solute will be - [AIPMT-98]
(1)
0.2 (2) 0.4 (3) 0.6 (4)
0.8
Q.11 5%
solution of sucrose is isotonic with 1% solution of a compound ‘A’ then the
molecular weight of compound ‘A’ is - [AIPMT-98]
(1)
32.4 (2) 68.4
(3)
121.6 (4) 34.2
Q.12 The
vapour pressrue of benzene at a certain temperature is 640 mm of Hg. A
non-volatile and electrolytic solid weighting 2.175 g is added to 39.08 g of
benzene. If the vapour pressure of the solution is 600 mm of Hg. What is the
molecular weight of the solid substance ?
[AIPMT-99]
(1)
79.82 (2) 65.25
(3)
59.60 (4) 49.50
Q.13 From
the colligative properties of solution which one is the best method for the
determination of mol. wt. of proteins & polymers - [AIPMT-2001]
(1)
Osmotic pressure
(2)
Lowering in freezing point
(3)
Lowering in V.P.
(4)
Elevation in B.Pt.
Q.14 Pure
water can be obtain from sea water by -
[AIPMT-2001]
(1)
Centrifugation (2) Plasmolysis
(3)
Reverse osmosis (4) Sedimentation
Q.15 A
solution contains non volatile solute of molecular mass M2. Which of the following can be used to
calculate the molecular mass of solute in terms of osmotic pressure - [AIPMT-2002]
(1) M2 = VRT (m2/π) (2)
M2 = RT/ π (m2/v)
(3) M2 = (m2/V) πRT (4) M2 = (m2/v)
(π/RT)
Note
: m2 ¾® mass of solute
V ¾® Volume of
solution
p ¾® Osmotic
pressure
Q.16 A
solution containing components A and B follows Raoult’s law [AIPMT-2002]
(1)
A – B attraction force is greater than
A – A and B – B
A – A and B – B
(2)
A – B attraction force is less than A – A
and B – B
(3)
A – B attraction force remains same as A – A and B – B
(4)
Volume of solution is different from sum
of volume of solute and solvent
Q.17 Formation
of a solution from two components can be considered as - [AIPMT-2003]
(i)
Pure solvent ® separated solvent
molecules, DH1
(ii)
Pure solute ®
separated solute molecules, DH2
(iii)
Separated solvent and solute molecules ® solution, DH3
Solution so
formed will be ideal if -
(1)
DHsoln =
DH1 +
DH2 +
DH3
(2)
DHsoln =
DH1 +
DH2 –
DH3
(3)
DHsoln =
DH1 –
DH2 –
DH3
(4)
DHsoln =
DH3 –
DH1 –
DH2
Q.18 Which
one of the statements given below concerning properties of solutions, describes
a colligative effect - [AIIMS-2003]
(1)
boiling point of pure water decreses by the addition of ethanol
(2)
vapour pressure of pure water decreases by the addition of nitric acid
(3)
vapour pressure of pure benzene decreases by the addition of naphthalene
(4)
boiling point of pure benzene increases by the addition of toluene
Q.19 The
average osmotic pressure of human blood is 7.8 bar at 37°C. What is the
concentration of an aqueous NaCl solution that could be used in the blood
stream - [AIIMS-2004]
(1)
0.16 mol/L (2)
0.32 mol/L
(3)
0.60 mol/L (4)
0.45 mol/L
Q.20 Camphor
is often used in molecular mass determination because - [AIPMT-2004]
(1)
It has a very high cryosopic constant
(2)
It is volatile
(3)
It is solvent for organic substances
(4)
It is readily available
Q.21 The
vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr, respectively.
The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol
of Q would be - [AIPMT-2005]
(1)
68 torr (2) 140
torr
(3)
72 torr (4) 20 torr
Q.22 A
solution of urea (mol. mass 56 g mol–1)
boils at 100.18°C at the atomospheric pressure. If Kf and Kb for water are 1.86 and 0.512K kg mol–1 respectively, the above solution will freeze
at - [AIPMT-2005]
(1)
–6.54°C (2)
–0.654°C
(3)
6.54°C (4) 0.654°C
Q.23 A
solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressures of
the pure hydrocarbonds at 20°C are 440 mmHg for pentane and 120 mmHg for
hexane. The mole fraction of pentane in the vapour phase would be -
[AIPMT-2005]
(1)
0.200 (2) 0.478
(3)
0.549 (4)
0.786
Q.24 A
solution containing 10g per dm3 of urea (molecular mass = 60g mol–1) is isotonic with a 5% solution of a
nonvolatile solute. The molecular mass of this nonvolatile solute is -
[AIPMT-2006]
(1)
250g mol–1 (2) 300g mol–1
(3)
350g mol–1 (4) 200g mol–1
Q.25 1.00g
of a non-electrolyte solute (molar mass 250g mol–1)
w was dissolved in 51.2g of benzene. If the freezing point depression constant,
Kf of benzene is 5.12 K kg mol–1, the freezing point of benzene will be
lowered by - [AIPMT-2006]
(1)
0.4 K (2) 0.3 K
(3)
0.5 K (4) 0.2 K
Q.26 A
solution of acetone in ethanol - [AIPMT-2006]
(1)
shows a positive deviation from Raoult’s law
(2) behaves like a near
ideal solution
(3)
Obey Raoult’s law
(4)
shows a negative deviation from Raoult’s law
Q.27 During
osmosis, flow of water through a semipermeable membrane is - [AIPMT-2006]
(1)
from both sides of semipermeable
membrane with equal flow rates
(2)
from both sides of semipermeable
membrane with unequal flow rates
(3)
from solution having lower concentration
only
(4)
from solution having higher concentration
only
Q.28 A
5% solution (by mass) of cane sugar in water has freezing point of 271 K and
freezing point of pure water is 273.15K. The freezing point of a 5% solution
(by mass) of glucose in water is - [AIIMS-2006]
(1)
271 K (2) 273.15 K
(3)
269.07 K (4)
277.23 K
Q.29 A
mixture of ethyl alcohol and propyl alcohol has a vapour pressure of 290 mm at
300 K. the vapour pressure of propyl alcohol is 200 mm. If the mole fraction of
ehtyl alcohol is 0.6, its vapour pressure (in mm) at the same temperature will
be [AIEEE-2007]
(1)
300 (2) 700
(3)
360 (4) 350
Q.30 0.5
molal aqueous solution of a weak acid (HX) is 20% ionised. If Kf for water is 1.86 K kg mol–1, the lowering in freezing point of the
solution is - [AIPMT-2007]
(1)
–0.56 K (2) –1.12 K
(3)
0.56 K (4) 1.12 K
Q.31 A 0.0020 M aqueous solution of an ionic
compound Co(NH3)5(NO2)Cl
freezes at – 0.00732ºC. Number of moles
of ions which 1 mole of ionic compound produces on being dissolved in
water will be : (kf =
– 1.86ºC/m) [AIPMT-2009]
(1) 1 (2) 2 (3)
3 (4) 4
Q.32 An aqueous solution is 1.00 molal in KI.
Which change will cause the vapour pressure of the solution to increase? [AIPMT-2010]
(1) addition of NaCl
(2) addition of Na2SO4
(3) addition of 1.00 molal KI
(4) addition of water
Q.33 A solution of sucrose (molar mass = 342 g
mol–1) has been
prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point
of the solution obtained will be : (Kf for water = 1.86 K kg mol–1)
[AIPMT-2010]
(1) –0.372°C (2) –0.520°C
(3) + 0.372°C (4) – 0.570°C
Q.34 The freezing point depression constant for
water is –1.86ºCm–1. If 5.00 g Na2SO4 is dissolved in 45.0g H2O, the freezing point is changed by
–3.82ºC. Calculate the Van’t Hoff factor for Na2SO4
(1) 0.381 (2) 2.05 [AIPMT-2011]
(3)
2.63 (4)
3.11
Q.35 The Van’t Hoff factor i for a compound
which
undergoes dissociation in one solvent and association in other solvent is respectively :
undergoes dissociation in one solvent and association in other solvent is respectively :
[AIPMT-2011]
(1)
greater than one and greater than one
(2)
less than one and greater than one
(3)
less than one and less than one
(4)
greater than one and less than one
thank u sir very much
ReplyDeletethanks sir so much
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