1. Calculate the molality and mole fraction of the solute in aqueous solution containing 3.0g of urea (molar mass =60 g/mol) per 250g of water.2. Calculate the molarity of the solution containing 0.5 g of NaOH dissolved in 500 cm3 of solution.3. Calculate the molality of a solution containing 9.8g of H2SO4 in 250 cm3 of the solution.4. Calculate the mole fraction of ethanol and water in a sample of rectified spirit which contains 95% of ethanol by weight.5. Find the molarity and molality of a 155 solution of H2SO4 (density of H2SO4 is 1.020 g/cm3 (Atomic mass : H=1,O=16, S=32).6. A solution contains 25% of water, 25% of ethanol and 50% of acetic acid by mass. Calculate the mole fraction of each component.7. A solution of ethanol in water is 1.54 molal. How many grams of it are there in 2500g of the solvent? (Mol. Wt. Of ethanol =46).8. Calculate the molality of a sulphuric acid solution in which the mole fraction of water is 0.85.9. What volume of 95% of sulphuric acid (density=1.85 g/cm3) and what mass of water must be taken to prepare 100 cm3 of 15% solution of sulphuric acid (density=1.10 g/cm3).10. The mol fraction of benzene in a solution in toluene is 0.50. Calculate the weight percent of benzene in the solution.11. What is the mole fraction of a solute in 2.5m aqueous solution?12. A 6.90M solution of KOH in water contains 30% by mass of KOH. Calculate the density of the KOH solution. (Molar mass of KOH is 56 g/mol).13. Calculate the mole fraction of the solute in an aqueous solution containing 18g of glucose (mol. Mass=180) in 100 gram of water.14. Calculate the molality and mole fraction of the solute in an aqueous solution containing 23.4g of NaCl in 90g of water. (Na=23,Cl=35.5).15. Calculate the molarity and molality of 20% aqueous ethanol (C2H5OH) solution by volume. Density of the solution is 0.960 g per cm3.16. A 10 cm3 sample of human urine was found to have 5mg of urea on analysis. Calculate the molarity of the given sample with respect to urea.(Mol. Mass of urea =60).17. An aqueous solution of a dibasic acid (mol. Mass =118) containing 35.4g of the acid per litre of the solution has density 1.0077 g/cm3. Express the concentration of the solution in many ways as you can.18. The concentration of H2SO4 is 18M. The solution had a density of 1.84 g/cm3. What is the mole fraction and weight percentage of H2SO4in this solution?19. If 4g NaOH are dissolved in 100 cm3 of the solution, what will be the Molarity?20. A solution contains 2.80 moles of acetone and 8.20 moles of chloroform. Calculate the mole fraction of acetone.21. What is the molarity of a solution of sodium chloride ( Na=23, Cl=35.5) which contains 60g of sodium chloride in 2000 cm3 of a solution?22. A 100 cm3 solution of sodium carbonate is prepared by dissolving 8.653g of the salt in water. The density of solution is 1.0816 per millimetre. What are the molarity and molality of the solution? (Na=23, C=12,O=16)23. 4.0 g of NaOH is contained in one decilitre of a solution. Calculate the following in this solution. a. Mole Fraction of NaOH b. Molality of NaOHc. Molarity of NaOH24. The percentage composition of a solution is 45% X, 15% Y, 40% Z. Calculate the mole fraction of each component of the solution.(Molecular mass of X=18, Y=60,Z=60)25. Calculate the mass fraction and mole fraction of ethyl alcohol and water in a solution containing 9.2g of alcohol in 18.0 g of water.26. A solution contains 410.3 g of H2SO4 per litre if the solution at 20 degree Celsius. If its density is 1.243g/cm3, what will be its molality and molarity?27. Sugar syrup of weight 214.2g contains 34.2g of sugar. Calculate molal concentration and mole fraction of sugar in the syrup.28. Concentrated nitric acid used as laboratory reagent is usually 69% by mass of nitric acid. Calculate the volume of the solution which contains 23g of HNO3. (Density of con. Nitric acid solution is 1.41 g/cm3).29.