| Question 1 | Calculate the molarity of the solution containing 5 g of NaOH in 450 ML solution. |
| Question 2 | If N2 gas is bubbled through water at 293K, how many millimoles of N2 gas would dissolve in 1L of water? Assume that N2 exerts a partial pressure of 0.987 bar. Given that Henry's law constant for N2 at 293K is 76.48 kbar. |
| Question 3 | The vapour pressure of pure benzene at a certain temperature is 0.850 bar. A non-volatile, non-electrolyte solid weighing 0.5g is added to 39.0g of benzene (molar mass 78g/mol). The vapour pressure of the solution then is 0.845 bar. What is the molecular mass of the solid substance? |
| Question 4 | 18 g of glucose C6H12O6 is dissolved in 1 kg of water in a saucepan. At what temperature will water boil at 1.013 bar? Kb for water is 0.52 K kg mol-1. |
| Question 5 | 2g of benzoic acid (C6H5COOH) dissolved in 25g of benzene shows a depression in freezing point equal to 1.62K. Molal depression constant for benzene is 4.9kg m−1. What is the percentage association of acid if it forms a dimer in solution? |
| Question 6 | 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? |
| Question 7 | 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? |
| Question 8 | What is meant by positive and negative deviations from Raoult's law, and how is the sign of DmixH related to positive and negative deviations from Raoult's law? |
| Question 9 | Calculate the mass of a non-volatile solute (molar mass 40 g mol–1), which should be dissolved in 114 g octane to reduce its vapour pressure to 80%. |
| Question 10 | Calculate the amount of benzoic acid (C6H5COOH) required for preparing 250 mL of 0.15 M solution in methanol. |
| Question 11 | Vapour pressure of water at 293 K is 17.535 mm Hg. Calculate the vapour pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water. |
| Question 12 | Benzene and toluene form an ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at 300 K is 50.71 mm Hg and 32.06 mm Hg respectively. Calculate the mole fraction of benzene in the vapour phase if 80 g of benzene is mixed with 100 g of toluene. |
| Question 13 | Determine the amount of CaCl2 (i = 2.47) dissolved in 2.5 litres of water such that its osmotic pressure is 0.75 atm at 27° C. |
| Question 14 | Determine the osmotic pressure of a solution prepared by dissolving 25mg of K2SO4 in 2 litres of water at 25 degrees c. Assuming that it is completely dissociated. |
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