14. Solutions

A 3.60 m aqueous sucrose solution is prepared. Given that the boiling point elevation constant (K_b) for water is 0.512 °C·kg/mol and pure water boils at 100.00 °C, what is the boiling point of the solution? Assume sucrose does not ionize in water.

A solution is prepared by dissolving 0.50 mol of NaCl in 1.00 kg of water. If the boiling point elevation constant (K_b) for water is 0.512 °C·kg/mol, what is the boiling point of the solution? (Assume complete dissociation of NaCl and the normal boiling point of water is 100.00 °C.)

Which of the following ions will contribute most to elevating the boiling point of H_2O when added at equal molal concentrations?

Which of the following statements best explains why the boiling point of NBr3 is higher than that of NH3?

Which of the following best describes the effect of adding a nonvolatile solute to a solvent on its boiling and freezing points?

Which of the following is a practical application of boiling point elevation?

Which of the following aqueous solutions would have the higher boiling point?

Which of the following aqueous solutions should have the lowest boiling point?

Which of the following aqueous solutions has the lowest boiling point?

Which of the following substances would you predict to have a higher boiling point, and why?

Which of the following aqueous solutions has the lowest boiling point?

Which of the following solutions has the higher boiling point?

Which statement best helps to explain the observation that water boils at 100~^ext{o}C, whereas a 1~ext{molal} aqueous solution of NaCl boils at a higher temperature?

Which of the following aqueous solutions would you expect to have the highest boiling point?

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)