Question 3
Calculate the molarity of each of the following solutions:
(a)30 g of Co(NO₃)₂. 6H₂O in 4.3 L of solution
(b)30 mL of 0.5 M H₂SO₄ diluted to 500 mL.

Exercise 2
Question 1
Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.

Exercise 2
Question 2
Suppose a solid solution is formed between two substances, one whose particles are very large and the other whose particles are very small. What kind of solid solution is this likely to be?

Exercise 2
Question 3
Define the following terms:
(i) Mole fraction    (ii) Molality    (iii) Molarity   (iv) Mass percentage.

Exercise 2
Question 4
Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL^-1?

Exercise 2
Question 5
A solution of glucose in water is labelled as 10% w/w, what would be the molality and mole fraction of each component in the solution? If the density of solution is 1.2 g mL^-1, then what shall be the molarity of the solution?

Exercise 2
Question 6
How many mL of 0.1 M HCl are required to react completely with 1 g mixture of Na₂CO₃ and NaHCO₃ containing equimolar amounts of both?

Exercise 2
Question 8
An antifreeze solution is prepared from 222.6 g of ethylene glycol (C₂H₆O₂) and 200 g of water. Calculate the molality of the solution. If the density of the solution is 1.072 g mL^-1, then what shall be the molarity of the solution?

Excersie 2
Question 9
A sample of drinking water was found to be severely contaminated with chloroform (CHCl₃) supposed to be a carcinogen. The level of contamination was 15 ppm (by mass):
(i) express this in percent by mass
(ii) determine the molality of chloroform in the water sample.

Exercise 2
Question 10
What role does the molecular interaction play in a solution of alcohol and water?

Exersice 2
Question 11
Why do gases always tend to be less soluble in liquids as the temperature is raised?

Exercise 2
Question 12
State Henry's law and mention some important applications?

Exercise 2

Question 13
The partial pressure of ethane over a solution containing 6.56 x 10^-3 g of ethane is 1 bar. If the solution contains 5.00 x 10^-2 g of ethane, then what shall be the partial pressure of the gas?

Exercise 2
Question 14
What is meant by positive & negative deviations from raoult’s law & how is the sign of ΔmixH related to positive & negative deviations from Raoult’s law?

Exercise 2
Question 15
An aqueous solution of 2% non-volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molar mass of the solute?

Exercise 2
Question 16
Heptane and octane form an ideal solution. At 373 K, the vapour pressures of the two liquid components are 105.2 kPa and 46.8 kPa respectively. What will be the vapour pressure of a mixture of 26.0 g of heptane and 35 g of octane?

Exercise 2
Question 19
A solution containing 30 g of non-volatile solute exactly in 90 g of water has a vapour pressure of 2.8 kPa at 298 K. Further, 18 g of water is then added to the solution and the new vapour pressure becomes 2.9 kPa at 298 K. Calculate:
1) Molar mass of the solute
2) Vapour pressure of water at 298 K.

Exercise 2
Question 22
At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration?

Exercise 2
Question 25
Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
(i) phenol  (ii) toluene  (iii) formic acid  (iv) ethylene glycol  (v) chloroform  (vi) pentanol.