14. Solutions

Boiling Point Elevation

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Which of the following substances would you predict to have a higher boiling point, and why?
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Carbon dioxide is dissolved in 722 mL of benzene with a density of 1.59 g/mL. What mass of carbon dioxide would you add to make the boiling point of the solution 104.7°C? (BP of benzene = 80.1 °C)
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Which of the following aqueous solutions has the lowest boiling point?
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Which of the following solutions has the higher boiling point?
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Which statement best helps to explain the observation that water boils at 100~^\(\text{o}\)C, whereas a 1~\(\text{molal}\) aqueous solution of NaCl boils at a higher temperature?
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Which of the following aqueous solutions would you expect to have the highest boiling point?
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What mass in grams of NaCl would need to be added to 2951 g of water to increase the boiling temperature of the solution by 1.500°C? (Kb for water is 0.5100°C/m)
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Which of the following compounds has the lowest boiling point?
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If a 3.90 m solution boils at 103.45 °C, what is the actual value of the van't Hoff factor, i, given that the boiling point of pure water is 100.00 °C and the ebullioscopic constant (Kb) is 0.512 °C/m?
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What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15°C?
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Arrange the following compounds in order from highest boiling point to lowest boiling point: NaCl, H2O, CH3OH, CH4.
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Which of the following solutes, when dissolved in equal molal amounts in water, will raise the boiling point of water the most?
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What is the boiling point of a solution that contains 50.0 g of FeBr3 in 200.0 g of water, given that the boiling point elevation constant (Kb) for water is 0.512 °C/m?
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Which of the following best describes the effect of adding a nonvolatile solute to a solvent on the boiling point of the solution?
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What mass in grams of NaCl would need to be added to 2051 g of water to increase the boiling temperature of the solution by 1.500 °C? (Kb for water is 0.5100 °C/m)
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