Indian Learners Own Academy, Kuwait

Indian Learners Own Academy, Kuwait

INDIAN LEARNERS OWN ACADEMY, KUWAIT

CLASS / ASSIGNMENT BY / SYBJECT / LESSON/TOPIC
XII / Mr. BINU MATHEW / CHEMISTRY / SOLUTIONS

Answer the following

  1. Define the following(1) Molarity (2) Mole fraction
  2. A solution of glucose in water is labelled as 10% by weight. what would be the Molality of the Solution( Molar mass= 180)
  3. State Raoult’s law of solution containing Volatile component. How does Raoult’s law become a special case of Henry's law
  4. What type of deviation is shown by a mixture of ethanol and acetone? give reason
  5. Define the following (1) ideal solution (2) Azeotrope
  6. Why does a solution containing non-volatile solute have higher boiling point than pure solvent? Why is the elevation of boiling point a colligative property?
  7. 18g of glucose (molar mass= 180) is dissolved in 1kg of water in a pan. At what temperature will this solution boil (Kb for water= 0.512 Kkgmol-1 Boiling point of water

= 373.15K]

  1. l g of non-electrolyte solute is dissolved in 50g of benzene lowered the freezing point of benzene by 0.40 K.Find The molar mass of the solute ( Kf of benzene= 5. 12 Kkgmol-1
  2. Define molal elevations constant (Kb)
  3. Determine the osmotic pressure of a solution prepared by dissolving 2.5 ×10-2 g of K2SO4 in 2L of water at 25°C assuming that it is completely disassociated ( R=0.0821 L atm K-l mol-1 , Molar mass of K2SO4 =174 gmol-1
  4. Which Colligative property is used to determine the molar mass of bio molecule
  5. 3·9 g benzoic acid dissolved in 49 g of benzene shows a depression in freezing point of 1·62K.Calculate the van’t Hofffactor and predict the nature of solute (associated/dissociated).[Given : Molar mass ofBenzoic Acid = 122 g mol–1, Kf (H2O) = 1·86 K kg mol–1]
  6. 30 g of urea (M = 60 g mol-1) is dissolved in 846 g of water. Calculate the vapour pressure of water for this solution if vapour pressure of pure water at 298 K is 23.8 mm Hg.
  7. A 10% solution (by mass) of sucrose in water has a freezing point of 269·15 K. Calculate the freezing point of 10% glucose in water if the freezing point of pure water is 273·15 K.

(Molar mass of sucrose = 342 g mol-1) (Molar mass of glucose = 180 g mol-1)

  1. A solution of glucose (Molar mass = 180 g mol–1) in water has a boiling point of 100·20 0C. Calculate the freezing point of the same solution. Molal constants for water Kf and Kb are 1·86 K kg mol–1 and 0·512 K kg mol–1 respectively

LAST DATE OF SUBMISSION- 31/03/2018

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