Question

Chemists often use molarity M, in moles/liter, to measure the concentration of solutions Molarity is a common unt of concentration because the volume of a liquid is very easy to measure. However, the drawback of using molarity is that volume is a temperature-dependent quantity. As temperature changes, density changes, which affects volume Volume markings for most laboratory glassware are calibrated for room temperature, about 20°C Fortunately, there are several other ways of expressing concentration that do not involve volume and are therefore temperature independent.

Answer 1

prumber of moles of glycool prosent = 21850X16mol/L XD.OOOL = 2.850X10 mass of solvent (water) present = 998.8 ml x 0.9982 g/ml = 997.00 216 g. part A part B: molality of glycerol = No. of moles of glyneol 2.850x 10 mol mass of solvent (in kg) 997.60216x10 3 kg molality = 2.8585695 X15h molly m Calgo = 2,859 x10² molling (Answer) v moles of glyceul - 2.850x102 ml - 0.02850 XGg - total number of moles 2.850x10+997.00 2169 55.370468 18.0153 glmel = 0.000514715 X Ghez = 5.147X10" (Answer) 2.850x1ö molx 92.09382g/mol x 100 f. percent by mass C₂ 403 = (2-850X15* * 92.093 82 + 997 00216) 3 = 0.00262565 Xlooy = 0.264565 4. = 0.2626 %. (Anower) parte: part D: mass of solute x 16 Concentration in ppm = in - mass of solution - 2.62467387 qx100 ppm = 2625.65 ppm 999.626834 g parts per million ho = 2626. ppm (Answer)