Question

1. 2.9 moles of blue fruit drink mix is added to 1.11 L of water in a pitcher on a hot summer’s day. Assuming a density of 1.00 g/mL and given the vapor pressure of pure water is 25.4 mmHg, what is the vapor pressure of the pitcher of blue fruit drink?

2. A 2.20 g sample of a non-electrolyte is dissolved in 51.1 g of water. The solution freezes at −1.23℃ . Calculate the molar mass of the solute. (Use Table 12.4)

3. What is the mass percent of ethanol (CHCHOH) if 0.0789 moles of ethanol is added to 0.271 kg of water?

Answer 1

Amsl. vapor pressure of solution can be calculated by Psoin = Xsow Psow , Pow= 25.4 mm Hg moles of solute = 2.9 moles, volume of H₂O=1:11h man of water = Voturme x density = HH11X1000 mt x 1.00 glue =1110 g moly = 62. Moles of water = 1110 g . = 61.667 mol . Tegnult - r moles solvent Psolutions = - - Psolvent (moles soluti)+(nieles of selvent) - (61 667 mol ) L x 25.4 mm Hg (2.9 +61.667 mol) Psolution = 24.25 9 mm Hg =) soln = 24. 26 mm Hg