6 g of urea was dissolved in 500 g of water. calculate the percentage by mass of urea in the solution. (1.186 % by mass) problems
34.2 g of glucose is dissolved in 400 g of water. Calculate the percentage by mass of glucose solution. (7.48 % by mass. problems
A solution is prepared by dissolving a certain amount of solute in 500 g of water. The percentage by mass of a solute in a solution is 2.38. Calculate mass of solute (12.19 g)
58 cm3 of ethyl alcohol was dissolved in 400 cm3 of water to form 454 cm3 of a solution of ethyl alcohol. Calculate percentage by volume of ethyl alcohol in water. (12.78 % by volume)
12.8 cm3 of benzene is dissolved in 16.8 cm3 of xylene. Calculate percentage by volume of benzene. (43.24 % by volume.
23 g of ethyl alcohol (molar mass 46 g mol-1) is dissolved in 54 g of water (molar mass 18 g mol-1). Calculate the mole fraction of ethyl alcohol and water in solution. (0.1429 and 0.8571)
4.6 cm3 of methyl alcohol is dissolved in 25.2 g of water. Calculate a) percentage by mass of methyl alcohol b) mole fraction of methyl alcohol and water. Given density of methyl alcohol = 0.7952 g cm-3, and C = 12, H = 1 and O = 16. (12.68, 0.0755, 0.9245)
Calculate the mole fraction of HCl in a solution of HCl containing 24.8 % of HCl by mass. Given H = 1, Cl = 35.5 (0.0347)
A solution of NaOH (molar mass 40 g mol-1) was prepared by dissolving 1.6 g of NaOH in 500 cm3 of water. Calculate the molarity of NaOH solution. (0.08 mol dm-3)
11.11 g of urea (NH2CONH2) was dissolved in 100 g of water. calculate the molarity of the solution. Given N = 14, H = 1, C = 12, O = 16. (1.852 mol kg-1).
34.2 g of sugar was dissolved in water to produce 214.2 g of sugar syrup. Calculate molality and mole fraction of sugar in the syrup. Given C = 12, H = 1 and O = 16. (0.556 mol kg-1, 0.0099)
Calculate the mole fraction of solute in its 2 molal aqueous solution. (0.0347)
Calculate molarity and molality of the sulphuric acid solution of density 1.198 g cm-3 containing 27 % by mass of sulphuric acid (molar mass 98 g mol-1). (3.77 mol kg-1, 3.301 mol dm-3)
Calculate the mole fraction, molality and molarity of HNO3 in a solution containing 12.2 % HNO3. Given density of HNO3 as 1.038 g cm-3, H = 1, N = 14, O = 16. (0.0396, 2.205 mol kg-1, 2.01mol dm-3)
Sulphuric acid is 95.8 % by mass. Calculate mole fraction and molarity of H2SO4 of density 1.91 g cm-3. Given H = 1, S = 32, O = 16. (0.80730, 17.98 mol dm-3)
Commercially available concentrated hydrochloric acid is an aqueous solution containing 38% HCl gas by mass. If its density is 1.1 g cm-3, calculate the molarity of HCl solution and also calculate the mole fraction of HCl and H2O. (11.45 mol dm-3, 0.232, 0.768)
An aqueous solution of NaOH is marked 10% (w/w). The density of the solution is 1.070 g cm-3. Calculate molarity, molality and mole fraction of NaOH in water. Given Na = 23, H =1 , O = 16 (2.675 mol dm-3, 2.77 mol kg-1, 0.0476, 0.9523)
Battery acid 4.22 M aqueous H2SO4 solution, and has density 1.21 g cm-3. What is the molality of H2SO4. Given H = 1, S = 32, O = 16 (5.298 mol kg-1)
Calculate the mole fraction and molality of HNO3 in a solution containing 12.2 % HNO3. Given atomic masses H = 1, N = 14 and O = 16.
Calculate molarity and molality of 6.3 % solution of nitric acid having density 1.04 g cm-3. Given atomic masses H = 1, N = 14 and O = 16.
A solution of glucose in water is labelled as 10 % (w/w). Calculate a) molality and b) molarity of the solution. Given the density of the solution is 1.20 g mL-1 and molar mass of glucose is 180 g mol-1.
Sulphuric acid is 95.8 % by mass. Calculate the mole fraction and molarity of H2SO4. Density of H2SO4 solution is 1.91 g cm-3.
The density of 5.35 M H2SO4 solution is 1.22 g cm-3. What is molality of a solution?
10.0 g KCl is dissolved in 1000 g of water. If the density of the solution is 0.997 g cm-3, calculate a) molarity and b) molality of the solution. Atomic masses K = 39 g mol-1 , Cl = 35.5 g mol-1.