Colligative Properties Boiling point elevation

Have you ever wondered why cars overheat in traffic most often in the summertime?

Why do you think the antifreeze-water mixture has a higher boiling point than does pure water?

How will a solution require a higher temperature to achieve any given vapor pressure?

What is the relationship between vapor pressure and boiling point elevation?

What do you think are some of the limitations of determining molar mass when using boiling point elevation?

Calculate the boiling point of an aqueous solution where enough lactic acid (C6H10O5) is added to make a 0.37 molal solution. The Kb for water is 0.512 °C/m.

Calculate the boiling point of an aqueous solution where enough lactic acid (C6H10O5) is added to make a 0.40 molal solution. The Kb for water is 0.512 °C/m?

What is the boiling point elevation when 120 g of lactic acid (C6H10O5) is dissolved in 600 g of cyclohexane (C6H12)? The boiling point constant for cyclohexane 2.79 °C/m, and the boiling point of pure cyclohexane is 80.74 oC.

What is the boiling point elevation when 250g of lactic acid (C6H10O5) is dissolved in 754 g of cyclohexane (C6H12)? The boiling point constant for cyclohexane 2.79 °C/m, and the boiling point of pure cyclohexane is 80.74 oC.

A solution was prepared by dissolving some acetone, (CH3)2CO, in 55.0 g of pure water. The boiling point of the solution at 1 atm was 100.25 °C. How many grams of acetone was dissolved to yield the solution? (Kb for water is 0.512 °C/m)