2.1 Define the terra solution. How many types of solutions are formed? Write briefly about each type with an example. 2.2 Give an example of a solid solution in which the solute is a gas. 2.3 Define the following terms: 2.4 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}? 2.5 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 m L^{1}, then what shall be the molarity of the solution? 2.6 How many mL of 0.1 M HCl are required to react completely with 1 g mixture of Na_{2}C0_{3} and NaHCO_{3} containing equimolar amounts of both? 2.7 A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the resulting solution. 2.8 An antifreeze solution is prepared from 222.6 g of ethylene glycol, (C_{2} H_{6}O_{2} ) and200 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? 2.9 A sample of drinking water was found to be severely contaminated with chloroform (CHCl_{3}), supposed to be a carcinogen. The level of contamination was 15 ppm (by mass). 2.10 What role does the molecular interaction play in a solution of alcohol and water? 2.11 Why do gases always tend to be less soluble in liquids as the temperature is raised? 2.12 State Henry’s law and mention some important applications. 2.13 The partial pressure of ethane over a solution containing 6.56 × 10^{3} g of ethane is 1 bar. If the solution contains 5.00 × 10^{2} g of ethane, then what shall be the partial pressure of the gas? 2.14 What is meant by positive and negative deviations from Raoult’s law and how is the sign of AmixH related to positive and negative deviations from Raoult’s law? 2.15 An aqueous solution of 2% nonvolatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molar mass of the solute? 2.16 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 35.0 g of octane? 2.17 The vapour pressure of water is 12.3 kPa at 300 K. Calculate vapour pressure of 1 molal solution of a nonvolatile solute in it 2.18 Calculate the mass of a nonvolatile solute (molar mass 40 g mol^{1}) which should be dissolved in 114 g octane to reduce its vapour pressure to 80%. 2.19 A solution containing 30g of nonvolatile solute exactly in 90 g of water has a vapour pressure of 2.8 kPa at 298 K. Further, 18g of water is then added to the solution and the new of vapour pressure becomes 2.9 kPa at 298 K. Calculate 2.20 A 5% solution (by mass) of cane sugar in water has freezing point of 271 K. Calculate the freezing point of 5% glucose in water if freezing point of pure water is 273.15 K. 2.21 Two elements A and B form compounds having formula AB_{2} and AB_{4}. When dissolved in 20g of benzene (C_{6}H_{6}), 1 g of AB_{2} lowers the freezing point by 2.3 K whereas 1.0 g of AB_{4} lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^{1}. Calculate atomic masses of A and B. 2.22 At 300 K, 36g of glucose present in a litre of its solution has an osmotic pressure of 4.08 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration? 2.23 Suggest the most important type of intermolecular attractive interaction in the following pairs: 2.24 Based on solutesolvent interactions, arrange the following in order of increasing solubility in noctanc and explain. 2.25 Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water? 2.26 If the density of some lake water is 1.25 g mL^{1} and contains 92g of Na^{+} ions per kg of water, calculate the molality of Na^{+} ions in the lake. 2.27 If the solubility product of CuS is 6 x 10^{16}, calculate the maximum molarity of CuS in aqueous solution.
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