The Van't Hoff factor for 0.1 M Ba(NO3)2 solution is 2.74. The degree of dissociation is [IIT 1999]

(1) 91.3%

(2) 87%

(3) 100%

(4) 74%

Subtopic:  Van’t Hoff Factor |
 83%
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Mole fraction of solute in an aqueous solution that boils at 100.104 is :

Kb for H2O = 0.52 K molality-1)

1.  0.008

2.  0.004

3.  0.061

4.  0.996

Subtopic:  Elevation of Boiling Point |
 59%
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Freezing point of an aqueous solution is -0.166°C. Elevation of boiling point of same solution would be-

(Kb = 0.512 K m-1 and Kf = 1.66 K m-1)

1. 0.18°C 2. 0.05°C
3. 0.09°C 4. 0.23°C
Subtopic:  Depression of Freezing Point |
 86%
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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

Subtopic:  Depression of Freezing Point |
 85%
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The molal freezing point constant for water is 1.86°C/m. Therefore, the freezing point of 0.1 m NaCl solution in water is expected to be [MLNR 1994]

(1) –1.86°C

(2) –0.186°C

(3) –0.372°C

(4) +0.372°C

Subtopic:  Depression of Freezing Point |
 54%
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The molar freezing point constant for water is 1.86°C/mole. If 342 g of cane sugar (C12H22O11) 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

Subtopic:  Depression of Freezing Point |
 82%
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A solution containing 6.8 g of a non-ionic solute in 100 g of water was found to freeze at −0.93 oC. The freezing point depression constant of water is 1.86. The molecular weight of the solute is-

1. 13.6 m 2. 34 m
3. 68 m 4. 136 m
Subtopic:  Depression of Freezing Point |
 78%
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What is the molality of the solution of a certain solute in a solvent if there is a freezing point depression of 0.184° and if the freezing point constant is 18.4 K kg 

1. 0.01

2. 1.00

3. 0.001

4. 100

Subtopic:  Depression of Freezing Point |
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An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7 g of water freezes at 272.817K. If the value of Kf for water is 1.86 K kg mol–1, the molecular mass of the acid is [AMU 2002]

(1) 46.0

(2) 48.6

(3) 48.8

(4) 46.8

Subtopic:  Depression of Freezing Point |
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Solution of sucrose (Mol. Mass = 342) is prepared by dissolving 34.2 gm of it in 1000 gm of water. Freezing point of the solution is (Kf for water is 1.86 K kg mol–1) [AIEEE 2003]

(1) 272.814 K

(2) 278.1 K

(3) 273.15 K

(4) 270 K

Subtopic:  Depression of Freezing Point |
 76%
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