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The Van't Hoff factor for 0.1 M $\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ solution is 2.74. The degree of dissociation is [IIT 1999]
(1) 91.3%
(2) 87%
(3) 100%
(4) 74%

The depression in freezing point of 0.01 M aqueous solutions of urea, sodium chloride and sodium sulphate is in the ratio of [Roorkee 1990; DCE 1994]
(1) 1 : 1 : 1
(2) 1 : 2 : 3
(3) 1 : 2 : 4
(4) 2 : 2 : 3

The molar freezing point constant for water is 1.86°C/mole. If 342 g of cane sugar $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$ is dissolved in 1000 g of water, the solution will freeze at 
1. –1.86°C
2. 1.86°C
3. –3.92°C
4. 2.42°C

The vapour pressure of a solvent A is 0.80 atm. When a non-volatile substance B is added to this solvent its vapour pressure drops to 0.6 atm. The mole fraction of B in the solution is [MP PMT 2000]
(1) 0.25
(2) 0.50
(3) 0.75
(4) 0.90

Lowering in vapour pressure is the highest for:
1. 0.2 m urea
2. 0.1 m glucose
3. 0.1 m MgSO₄
4. 0.1 m BaCl₂

The density of H₂SO₄ solution is 1.84 g ml^–1. In a 1 litre solution if H₂SO₄ is 93 % by (w/v) then the molality of the solution is -

The molarity of a $0.2\mathrm{N}{\mathrm{Na}}_2{\mathrm{CO}}_3$ solution will be [MP PMT 1987]
(1) 0.05 M
(2) 0.2 M
(3) 0.1 M
(4) 0.4 M

Amount of oxalic acid ${\left(\mathrm{COOH}\right)}_2.2{\mathrm{H}}_2\mathrm{O}$ in grams that is required to obtain 250 ml of a semi-molar solution is 
(1) 17.25 g
(2) 17.00 g
(3) 15.75 g
(4) 15.00 g

10.6 g of Na₂CO₃ was exactly neutralised by 100 ml of H₂SO₄ solution. Its normality is
(1) 1 N
(2) 2 N
(3) 1.5 N
(4) 0.5 N

Amount of NaOH present in 200 ml of 0.5 N solution is 
(1) 40 g
(2) 4 g
(3) 0.4 g
(4) 4.4 g

3.24 g of Hg(NO₃)₂ (molar mass = 324) dissolved in 1000 g of water constitutes a solution having a freezing point of –0.0558°C while 21.68 g of HgCl₂ (molar mass = 271) in 2000 g of water constitutes a solution with a freezing point of –0.0744°C. The K_f for water is 1.86 $\frac{\text{K\hspace{0.17em}– Kg}}{\text{Mol}}$. About the state of ionization of these two solids in water it can be inferred that:
(1) Hg(NO₃)₂ and HgCl₂ both are completely ionized
(2) Hg(NO₃)₂ is fully ionized but HgCl₂ is fully unionized
(3) Hg(NO₃)₂ and HgCl₂ both are completely unionized
(4) Hg(NO₃)₂ is fully unionized but HgCl₂ is fully ionized  

An ideal mixture of liquids A and B with 2 moles of A and 2 moles of B has a total vapour pressure of 1 atm at a certain temperature. Another mixture with 1 mole of A and 3 moles of B has a vapour pressure greater than 1 atm. But if 4 moles of C are added to the second mixture, the vapour pressure comes down to 1 atm. Vapour pressure of C, P_c° = 0.8 atm. Calculate the vapour pressures of pure A and pure B.
(1) P_A° = 1.4 atm, P_B° = 0.7 atm
(2) P_A = 1.2 atm, P_B° = 0.6 atm
(3) P_A = 1.4 atm, P_B° = 0.6 atm
(4) P_A° = 0.6 atm, P_B° = 1.4 atm

A solution of x moles of sucrose in 100 grams of water freezes at −0.2°C. As ice separated the freezing point goes down to 0.25°C. How many grams of ice would have separated?
(1) 10 grams
(2) 20 grams
(3) 25 grams
(4) 23 grams

How many mili moles of sucrose should be dissolved in 500 gms of water so as to get a solution which has a difference of 103.57°C between boiling point and freezing point.
(K₁ = 1.86 K Kg mol⁻¹, K_b = 0.52 K Kg mo1⁻¹)
(1) 500 mmoles
(2) 900 mmoles
(3) 750 mmoles
(4) 650 mmoles

A solution of acetone in ethanol:
1. Shows a negative deviation from Raoult's law.
2. Shows a positive deviation from Raoult's law.
3. Behaves like a near ideal solution.
4. Obeys Raoult's law.

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_f for water is 1.86 K kg mol^-1, the lowering in freezing point of the solution is:
(1) -1.12 K
(2) 0.56 K
(3) 1.12 K
(4) - 0.56 K

p_A and p_B are the vapour pressure of pure liquid components, A and B, respectively of an
ideal binary solution.If x, represents the mole fraction of component A, the total pressure
of the solution will be.
1. p_A + x_A(p_B-p_A)
2. p_A + x_A(p_A-p_B)
3. p_B + x_A(p_B-p_A)
4. p_B + x_A(p_A-p_B)

Compound PdCl₄.6H₂O is a hydrated complex, 1 molal aqueous solution of it has freezing point 269.28 K. Assuming 100 % ionization of complex, the molecular formula of the complex is-
(K_f for water = 1.86 K kg mole^-1)
1. [Pd(H₂O)₆]Cl₄
2. [Pd(H₂O)₄Cl₂]Cl₂.2H₂O
3. [Pd(H₂O)₃Cl₃]Cl.3H₂O
4. [Pd(H₂O)Cl₄]4H₂O

What amount of CaCl₂(i=2.47) is dissolved in 2L water so that its osmotic pressure is 0.5 atm at 27$°\mathrm{C}$:-
(1) 13.42 g
(2) 19.24 g
(3) 8.834 g
(4) 1.820 g

If partial pressure of oxygen is 0.5 atm and K_H = 1.4 × 10^-3 M/atm, then the amount of oxygen dissolved in 100 ml water at 298K is-

The lubricating action of an oil is more if it possess:-
(1) High vapour pressure
(2) low vapour pressure
(3) High surface tension
(4) High density