Depression in Freezing Point
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On dissolving 0.5 g of non-volatile, non-ionic solute to 39 g of benzene, its vapour pressure decreases from 650 mm of Hg to 640 mm of Hg. The depression of freezing point of benzene (in K) upon addition of the solute is __________________. [Given data: Molar mass & molar freezing point depression of benzene is & ]
The freezing point of aqueous solution that contains mass urea, mass and mass of glucose is-
Cd(CN)2⇌Cd2++2CN−NaCN→Na++CN−
- 2×10−8
- 1.0×10−6
- 4×10−6
- 1.0×10−8
- 2.05 M
- 2.50 M
- 3.15 M
- 1.25 M
Two elements A and B form compounds of formula AB2 and AB4. When dissolved in 20.0g of benzene 1.0g of AB2 lowers freezing point by 2.3°C whereas 1.0g of AB4 lowers freezing point by 1.3°C. The Kf for benzene. The atomic masses of A and B are
- 27, 45
- 42, 25
- 52, 48
- 48, 52
- −0.654 ∘C
- −0.98 ∘C
- −1.54 ∘C
- +0.101 ∘C
Of the following 0.10 m aqueous solution, which one will exhibit the largest freezing point depression?
KCl
C6 H12 O6
Al2(SO4)3
K2SO4
Molal depression constant for water is 1.86°C. The freezing point of a 0.05 molal solution of a non-electrolyte in water is
-1.86°C
-0.93°C
-0.093°C
0.93°C
- C6H5NH3Cl
- Ca(NO3)2
- La(NO3)3
- C6H12O6 (glucose)
- 0.01 M NaCl
- 0.005MC2H5OH
- 0.005MMgI2
- 0.005MMgSO4
The molar freezing point constant for water is 1.86 °C mole-1. If 342 gm of canesugar (C12H22O11) are dissolved in 1000 gm of water, the solution will freeze at
-1.86°C
1.86°C
-3.92°C
2.42°C
An aqueous solution of a non-electrolyte boils at 100.52°C. The freezing point of the solution will be
0°C
-1.86°C
1.86°C
None of the above
- 562
- 462
- 362
- 232
The freezing point of one molal NaCl solution assuming NaCl to be 100% dissociated in water is (molal depression constant = 1.86)
-1.86°C
-3.72°C
+1.86°C
+3.72°C
- NaCl increases the freezing point of water
- NaCl decreases the freezing point of water
- NaCl decreases the boiling point of water
- NaCl lowers the vapour pressure of water
- Doubled
- Halved
- Tripled
- Unchanged
If molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be
Halved
Tripled
Unchanged
Doubled
What is the freezing point of a solution containing 8.1 g HBr in 100g water assuming the acid to be 90% ionised (Kf for water =1.86 Kmole-1)
0.85∘C
−3.53∘C
0∘C
−0.35∘C
- 161.29g
- 38.71g
- 200g
- 31.7g
Heavy water freezes at
0°C
3.8°C
38°C
-0.38°C
Which of the following will have hightest boiling point at 1 atm pressure?
- 0.1M NaCl
- 0.1M Sucrose
- 0.1M BaCl2
- 0.1M glucose
How much water is needed to dilute 10 ml of 10 N HCl to make it exactly deci-normal?
990ml
1000ml
1010ml
100ml
- C6H6
- C6H12
- C8H18
- C10H6
- −6.54 ∘C
- −0.05 ∘C
- −1.308 ∘C
- −0.654 ∘C
The figures shown below represent plots of vapour pressure (V.P.) versus temperature (T). [Molecular weight of ethanol is 46 g mol−1]
Among the following, the option representing change in the freezing point is?
- That having low freezing point and small enthalpy of fusion
- That having high freezing point and small enthalpy of fusion
- That having low freezing point and small enthalpy of vapourization.
- That having large surface tension
- 2.13gcm−3
- 1.13gcm−3
- 4.13gcm−3
- 3.13gcm−3
- 804.32g
- 904.32 g
- 704.32 g
- 1004.32 g
[molecular weight of ethanol is 46 gmol−1]
Among the following, the option
representing change in the freezing point is: