117.0 g of NaCl is dissolved in 500.0 g of H2O at 70 °C, with the vapor pressure of pure water at 70°C being 233.7 mm Hg. Kb = 0.51 °C/m and Kf = 1.86° C/m for water. Density of the solution is 1.2 g/mL. Assume complete dissociation of the solute. What is the osmotic pressure of the solution at 70 °C?
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Molality (m) = moles of solute / mass of solvent in kg The molar mass of NaCl is approximately 58.44 g/mol. So, the moles of NaCl = 117.0 g / 58.44 g/mol = 2.003 mol The mass of water is 500.0 g, which is 0.500 kg. So, the molality (m) = 2.003 mol / 0.500 kg Show more…
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