CU 13 = SXS = S- s2 = 6 x 10-16 or S=V6 x 10-16 = 2.45 x 10-8 mol L-1 .: Maximum molarity of CuS in aqueous solution = 2.45 x 10-8 mol L-1 An antifreeze solution is prepared from 222.6 g of ethylene glycol, C2H4OH)2 and 200 g Calculate the molality of the solution. If the density of the solution is 1.072 g mL-1, then be the molarity of the solution? [NCERT; CBSE Mass of ethylene glycol = 222.6 g Molar mass of ethylene glycol, C H (OH)2 = 62 g mol! _ 222.6 g Number of moles of ethylene glycol =- 59 mol 62 g mol-1 Mass of water = 200 g = 0.20 kg Moles of ethylene glycol _3.59 mol - 17.95 mol kg Molality of solution = Mass of solvent(in kg) 0.20 kg Total mass of the solution = 222.6 g + 200 g = 422.6 g Mocs of solution 422.6 g 204ml