Depression in Freezing Point
A 5% solution (by mass) of cane sugar in water has freezing point 271 K. Calculate freezing point of 5% glucose in water if freezing point of pure water is 273.15K.
The value of observed and calculated molecular weight of silver nitrate are 92.64 and 170 respectively. The degree of dissociation of AgNO3 will be:
What is meant by Equivalent weight give me a simple formula to understand it?
Calculate the depression in the freezing point of water when 10g of CH3CH2CHClCOOH is added to 250 g of water, Ka=1.4×10−3; Kf=1.86 K kg mol−1
A solute A dimerizes in water. The boiling point of a molal solution of A is . The percentage association of A is (round off to the nearest integer) (use for water ; boiling point of water ) -
If molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be
The depression in freezing point of water observed for the same amount of acetic acid, triehloroacetie acid and trifluoroacctie acid increases in the order given above. Explain briefly.
What is the effect of temperature on the solubility of a solid in liquid.
What is depression of freezing point?
- 0.05 M KNO3>0.04 M CaCl2>0.14 M sugar >0.075 M CuSO4
- 0.04 M BaCl2>0.14 M sucrose>0.075 M CuSO4>0.05 M KNO3
- 0.075 M CuSO4>0.14 M sucrose >0.04 M BaCl2>0.05 M KNO3
- 0.075 M CuSO4>0.05 M NaNO3>0.14 M sucrose>0.04 M BaCl2
Benzoic acid dissolved in benzene shows a molecular mass of _______ g/mol.
The van't Hoff factor "i" for 0.2 molal aqueous solution of urea is:
is dissociated in water to and . The boiling point of a molal aqueous solution of is ____________ . (Round off to the Nearest Integer).
[Given: Molal elevation constant of water boiling point of pure water ].
( Molar mass of urea = 60 g/mol)
- 6 g
- 3 g
- 0.5 g
Molecules of benzoic acid dimerises in benzene. of the acid dissolved in of benzene shows a depression in freezing point equal to . If the percentage association of the acid to form a dimer in solution is, then w is:
(Given that , Molar mass of benzoic acid)
Assertion (A) When NaCl is added to water a depression in freezing point is observed.
Reason (R) The Lowering of vapour pressure of a solution causes depression in the freezing point.
- Liquid solvent, solid solvent
- Liquid solvent, solid solute
- Liquid solute, solid solute
- Liquid solute, solid solvent
The freezing point of a solution prepared from 1.25 gm of a non-electrolyte and 20gm of water is 271.9 K. If molar depression constant is 1.86 K mole-1, then molar mass of the solute will be
- 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
Which among the following will show maximum osmotic pressure?
(A) 1M Nacl
(B) 1M Mgcl2
(C) 1M (NH4)3PO4
(D) 1M Na2SO4
Please specify the reasons