Complete the following table for water solutions of ammoniumsulfate Density Mola
ID: 684113 • Letter: C
Question
Complete the following table for water solutions of ammoniumsulfate Density Molarity Molality MassPercent of Solute a)1.06 0.886 _____ ________________ b)1.23 _____ 3.11 ________________ Complete the following table for water solutions of ammoniumsulfate Density Molarity Molality MassPercent of Solute a)1.06 0.886 _____ ________________ b)1.23 _____ 3.11 ________________Explanation / Answer
Density = mass/volume Molarity = mol / volume Molality = mol / mass of solvent in kg (a) Density = 1.06 (There is 1.06g of solution in 1mL) Molarity = 0.886 (There is 0.886mol of solute in 1 litre ofsolution) Mass of solute = nM = 0.886 x 132.14 = 117.08g Mass of solvent = 1060 - 117.08 = 942.92g = 0.94292kg Molality = 0.886/0.94292 = 0.9396m Mass percent = 117.08/1060 x 100% = 11.04% (b) Molality = 3.11m (There is 3.11mol of solute in 1kg of solvent) Mass of solute = nM = 3.11 x 132.14 = 410.96g Mass of solution = 1000 + 410.96 = 1410.96g Density = 1.23 Density = mass/volume 1.23 = 1410.96/volume Volume = 1147.1mL = 1.147L Molarity = 3.11/1.147 = 2.71M Mass percent = 410.96/1410.96 x 100% = 29.13% Hope this helps!