Multiple Choice
Which of the following substances would you predict to have a higher boiling point, and why?
14. Solutions
Boiling Point Elevation
Back14. Solutions
Boiling Point Elevation
- Multiple ChoiceWhat 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)
- Multiple Choice
What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15°C?
- Multiple Choice
An ethylene glycol solution contains 25.2 g of ethylene glycol (C2H6O2) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.
- Multiple Choice
Pure water boils at 100°C. What is the new boiling point of water after the addition of 13.12 g aluminum chloride, AlCl3, to 615 g water?
- Multiple Choice
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?
- Multiple ChoiceCalculate ΔTb for a solution that is prepared by dissolving 2.50 g Ca(NO3)2 in 2.00 L of water. Assume that the density of water = 1.00 g/mL and that ;Kb for water is 0.512 °C /m
- Open Question
Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/ml). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.
- Open Question
A solution of toluene (C₇H₈) in 301 g of cyclohexane (C₆H₁₂) has a boiling point of 90.30°C. what quantity in moles of toluene are in the solution? (for cyclohexane kb = 2.92°C/m, normal boiling point, Tb = 80.90°C)
- Open Question
Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 ml of benzene (d = 0.877 g/ml). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.
- Multiple Choice100.0 g of urea (CO(NH2)2) is dissolved in 550.0 g of liquid chloroform. Given that urea is a covalent compound with a molar mass of 60.07 g/mol and the boiling point elevation constant (Kb) for chloroform is 3.63 °C/m, what is the boiling point of the solution if the normal boiling point of chloroform is 61.2 °C?
- Multiple ChoiceA glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the boiling point of the solution. The boiling point elevation constant (Kb) for water is 0.512 °C/m. What is the boiling point of the solution?
- Multiple ChoiceA solution of a nonvolatile solute in water has a boiling point of 380.5 K. Calculate the vapor pressure of water above this solution at 338 K. The vapor pressure of pure water at this temperature is 0.2467 atm. Which of the following is the vapor pressure of water above the solution?
- Multiple ChoiceA solution of water (Kb=0.512 °C/m) and glucose boils at 103.56 °C. What is the molal concentration of glucose in this solution? Assume that the boiling point of pure water is 100.00 °C.
- Multiple ChoiceChloroform has a normal boiling point of 61.2°C and a boiling point elevation constant (Kb) of 3.63°C·kg/mol. You dissolve 1.08 moles of a compound (non-electrolyte) into 8 grams of chloroform. What is the boiling point of this solution?