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The boiling point of an azeotropic mixture of water and ethanol is less than that of water and ethanol.  The mixture shows
(1) No deviation from Raoult's law
(2) Positive deviation from Raoult's law
(3) Negative deviation from Raoult's law
(4) That the solution is unsaturated

An aqueous solution of non-electrolyte 'A' with molecular mass 60 contains 6 g in 500 mL and has a density equal to 1.05 g $m{L}^{-1}$.  The molality of solution  is
(1) 1.25
(2) 0.19
(3) 0.25
(4) 0.30

The vapour pressure of benzene and pure toluene at 70$°$C are 500 mm and 200 mm Hg respectively.  If they form an ideal solution. What is the mole fraction of benzene in a mixture boiling at 70$°$C at a total pressure of 380 mm Hg?
(1) 0.20
(2) 0.40
(3) 0.60
(4) 0.80

At a given temperature, total vapour pressure (in Torr) of a mixture of volatile components A and B is given P = 120 - 75 $x_B$.  Hence vapour pressure of pure A and B respectively (in Torr) are
(1) 120, 75
(2) 120, 195
(3) 120, 45
(4) 75, 45

Equal volumes of 0.1 M $AgN{O}_3$ and 0.2 M  NaCl are mixed. The concentration of $N{O}_3^{-}$ ions in the mixture will be:

$K_4\left[Fe{\left(CN\right)}_6\right]$ is 50% dissociated then the value of Van't Hoff factor (i)
(1) 2
(2) 2.2
(3) 2.5
(4) 3

Two liquids X and Y from an ideal solution.  The mixture has a vapour pressure of 400 mm at 300 K when mixed in the molar ratio of 1:1 and a vapour pressure of 350 mm when mixed in the molar ratio 1:2 at the same temperatue.  The vapour pressures of the two pure liquids X and Y respectively are
(1) 250 mm, 550 mm
(2) 350 mm, 450 mm
(3) 350 mm, 700 mm
(4) 550 mm, 250 mm

Mole of $K_{2}S{O}_4$ to be dissolved in 12 moles water to lower its vapour pressure by 10 mm of Hg at a temperature at which vapour pressure of pure water is 50 mm of Hg is
(1) 3 mol
(2) 0.5 mol
(3) 1 mol
(4) 2 mol

When mercuric iodide is added to the aqueous solution of potassium iodide is 
(1) Freezing point is raised
(2) Freezing point is lowered
(3) Freezing point does not change
(4) Boiling point does not change

Aluminium phosphate is 100% ionized in 0.01 m aqueous solution.  Hence, $∆T_b/k_b$ is
(1) 0.01
(2) 0.015
(3) 0.0175
(4) 0.02

60 g m of Urea is dissolved in 1100 gm solution.  To keep $∆T_f/k_f$ as 1 mol/g, water separated in the form of ice is
1. 40 gm
2. 60 gm
3. 100 gm
4. 200 gm

At temperature 327$°$C and concentration 'C', osmotic pressure of a solution is 'P', the same solution at concentration 'C/2' at 427$°$C shows osmotic pressure 2 atm, value of 'P' will be
(1) 12/7
(2) 24/7
(3) 6/5
(4) 5/6

Van't Hoff factor for $SrC{l}_2$ at 0.01 M is 1.8.  Percentage dissociation of $SrC{l}_2$ will be
(1) 70
(2) 55
(3) 40
(4) 30

If the relative decrease in vapour pressure is 0.4 for a solution containing 1 mol NaCl in 3 mol of ${\mathrm{H}}_2\mathrm{O}$, then percentage ionisation of NaCl will be -
1. 60%
2. 80%
3. 40%
4. 100%

2.56 g of sulphur in 100 g of CS₂  has depression in a freezing point of 0. 01 °C  and  K_f = 0.1 K / molal.  The atomicity of sulphur in the solution will be:
1. 2
2. 4
3. 6
4. 8