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Why do gases always tend to be less soluble in liquids as the temperature is raised?
Concept: Solubility >> Solubility of a Gas in a Liquid
Calculate the amount of CaCl2 (molar mass = 111 g mol−1) which must be added to 500 g of water to lower its freezing point by 2 K, assuming CaCl2 is completely dissociated. (Kf for water = 1.86 K kg mol−1)
Concept: Colligative Properties and Determination of Molar Mass >> Depression of Freezing Point
A solution of a substance having mass 1.8 x 10-3 kg has the osmotic pressure of 0.52 atm at 280 K. Calculate the molar mass of the substance used.
[Volume = 1 dm3, R = 8.314 J K-1 mol-1]
Concept: Colligative Properties and Determination of Molar Mass
The boiling point of benzene is 353.23 K. When 1.80 gram of non-volatile solute was dissolved in 90 gram of benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of solute.
[Kb for benzene = 2.53 K kg mol-1]
Concept: Colligative Properties and Determination of Molar Mass
An organic substance (M = 169 gram mol–1) is dissolved in 2000 cm3 of water. Its osmotic pressure at 12°C was found to be 0.54 atm. If R = 0.0821 L atm K–1 mol–1, calculate the mass of the solute.
Concept: Colligative Properties and Determination of Molar Mass
Define Freezing point.
Concept: Colligative Properties and Determination of Molar Mass >> Depression of Freezing Point
The temperature at which vapour pressure of a liquid becomes equal to the atmospheric
pressure is _______.
(A) melting point
(B) boiling point
(C) 273 K
(D) 373 K
Concept: Colligative Properties and Determination of Molar Mass >> Relative Lowering of Vapour Pressure
Which mixture is used for respiration by deep sea divers?
(A) He + O2
(B) Ne + O2
(C) Ar + O2
(D) Kr + O2
Concept: Solubility >> Solubility of a Gas in a Liquid
How does solubility of a gas in water varies with the temperature?
Concept: Solubility >> Solubility of a Gas in a Liquid
Derive the relation ∆H − ∆U = ∆nRT.
Concept: Solubility >> Solubility of a Solid in a Liquid
When KOH solution is added to potassium dichromate solution the colour of solution
changes to yellow, because _______
(A) chromate ion changes to dichromate ion
(B) dichromate ion changes to chromate ion
(C) oxidation number of chromium changes from + 6 to + 4
(D) oxidation number of chromium changes from + 4 to +6
Concept: Expressing Concentration of Solutions
How van’t Hoff factor is related to the degree of dissociation?
Concept: Abnormal Molar Masses
Which of the following 0.1 M aqueous solutions will exert the highest osmotic pressure?
Concept: Colligative Properties and Determination of Molar Mass >> Osmosis and Osmotic Pressure
Which of the following 0.1 M aqueous solutions will exert the highest osmotic pressure?
Concept: Colligative Properties and Determination of Molar Mass >> Osmosis and Osmotic Pressure
Derive the relation between the elevation of boiling point and molar mass of solute.
Concept: Colligative Properties and Determination of Molar Mass >> Elevation of Boiling Point
Define Semipermeable membrane
Concept: Colligative Properties and Determination of Molar Mass >> Osmosis and Osmotic Pressure
Define Semipermeable membrane
Concept: Colligative Properties and Determination of Molar Mass >> Osmosis and Osmotic Pressure
22.22 gram of urea was dissolved in 300 grams of water. Calculate the number of moles of urea and molality of the urea solution. (Given: a Molar mass of urea = 60 gram mol-1)
Concept: Expressing Concentration of Solutions
Derive van’t Hoff general solution equation.
Concept: Types of Solutions
Derive van’t Hoff general solution equation.
Concept: Types of Solutions
