14. The density of an aqueous solution prepared by mixing equal amounts of ethyl

Question

14. The density of an aqueous solution prepared by mixing equal amounts of ethylene glycol (CH.O2) and water is 1.65 g/mL Calculate the molality, the mol fraction, and the molarity of this solution. 15. The density of a .125-M aqueous NHs solution is 2.05 g/mL. What is the mol fraction of the solution? 16. Calculate the %v/v of a solution prepared by dissolving 357 mL of ethylene glycol (d 1.11g/mL) in 255 g of water to make a 1.23-g/mL aqueous solution. 17. Calculate the respective molarity and molality of an isopropyl alcohol aqueous solution that is 15.0% v/v (The densities of isopropyl alcohol (C3H,O) and water are .79 g/mL and 1.00 g/mL, respectively). 53

Explanation / Answer

(15)

Assume that we take 1 L of this solution.

Moles of solute = Molarity*Volume = 0.125*1 = 0.125

Mass of solute = Moles*MW = 0.125*17 = 2.125 g

Mass of solution = Density*Volume = 2.05*1000 = 2050 g

Mass of water = 2050-2.125 = 2047.875 g

Moles of water = Mass/MW = 2047.875/18 = 113.77

So,

Mole fraction of solute = 0.125/(0.125+113.77) = 0.0010975

Hope this helps !

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